1.5a Atomic structure and periodic table
1.5a Relative massesThe unit of mass is 1/12 of the mass of an atom of the isotope Carbon-12 (12C=12 exactly)
The Relative Atomic Mass (Ar)of an element is the ratio of the mass of an average atom of that element to 1/12 of the mass of an atom of the nuclide Carbon-12.
The Relative Isotopic Mass of a nuclide is the ratio of the mass of one atom of that nuclide to 1/12 of the mass of a Carbon-12 atom.
The Relative Molecular Mass (Mr)of a substance is the ratio of the mass of an average molecule of that substance to 1/12 of the mass of an atom of the nuclide Carbon-12.
Task1.5a Explain what is meant by
The relative atomic mass of helium is 4.002602.
The relative isopotic mass of deuterium is 2.0000.
The relative molecular mass of water is 18.
1.5b mass spectrometer
Uses of mass spectrometers
The mass spectrometer can detect the abundance of isotopes such as U-238 and Pb-206.
In any one place the Earth concentrates some minerals like uranium but not others like lead. So some rocks form containing uranium but not lead.
U-238 is radioactive and decays to form Pb-206 over time.
This process is controlled by the half life of U-238 which is 4.5*109 years. The relative abundance of U-238 to Pb-206 can be used to calculate the age of the rock.
Rock is found to have ages up to about 4 thousand million years, but not older. This is the age of the Earth when the first solid rock formed from the magma on the surface of the cooling planet.
Radiocarbon dating using C-14 can be used to similarly date organic matter.
The mass spectrum of an element shows the relative isotopic mass (m/e) and relative abundance of each isotope of the element being tested.
In a mass spectrum the height of each peak = the relative abundance.
The Relative Atomic Mass of an element can be found by finding the sum of the products of the relative abundance of each isotope and its relative isotopic mass and the dividing by the total relative abundance.
work sheets mass spetrometer ( AS level)
Write a sentence for each stage in the formation of a mass spectrum.
Isotopes are atoms of the same element with different numbers of neutrons in the nucleus
The Relative Atomic Mass of an element is the weighted (to take account of relative abundance) average of the the Relative Isotopic Masses of all of the isotopes of that element.E.g. Chlorine has two isotopes with mass numbers (and relative isotopic masses
35 and37
35 37
75% is Cl and 25% is Cl
17 17
Let there be 100 atomsTotal mass of 100 atoms = (75 * 35) + (25 * 37) = 3550
Average mass of an atom (relative atomic mass of chlorine) = Total mass /Number of atoms=3550/100so relative atomic mass of chlorine = 35.5
PRACTICE QUASTIONS
1. Bromine exists as two isotopes with mass numbers 81 and 79. If there is 50% of each isotope in a sample what is the relative atomic mass of bromine?
2. Calculate the relative atomic mass of the following:(a) gallium 60% Ga 69 and 40% Ga 71
(b) neon 90% Ne 20 and 10% Ne 22
(c) silver 50% Ag 107 and 50% Ag 109
(d) boron 20% B 10 and 80% B 11
(e) neon 90.92% Ne 20, 8.82% Ne 22 and 0.26% Ne 21.
(f) lead 52.3% Pb 208, 22.6% Pb 207, 23.6% Pb 206 and 1.5% Pb 204.
ionization energies
The first ionisation energy is the enthalpy change when 1 mole of gaseous atoms of an element each lose an electron to form gaseous ions each with a single positive charge.
It is the enthalpy change for the reaction: M(g) ---> M+(g) + e-
The second ionisation energy is the enthalpy change when 1 mole of gaseous ions of an element each with a single positive charge each lose an electron to form gaseous ions each with a double positive charge.
It is the enthalpy change for the reaction: M+(g)---> M2+(g) + e-
All of these ionizations involve the removal of a negative electron from a positive nucleus. The attraction between these must be over come by supplying energy. The process is always endothermic. Example 1st IE of Na = +500kJmol-1
Task1.5d.1 Define the third ionisation enthalpy for the element M and give an equation.
Task1.5d.2 Define the first ionisation enthalpy for sodium, magnesium, chlorine and neon.
Task1.5d.3 Define the second ionisation enthalpy for lithium, aluminium and oxygen.
1.5e Electronic structureThe graph of successive ionisation energies against ionisation number shows electrons grouped into three energy levels or quantum shells with similar energies.
Electron 1 (ionisation number = 1, removed first) from the third shell, electrons 2-9 in second shell, electrons 10 and 11(removed last) from first shell closest to the nucleus.
Electron 1 is on its own in the outer shell indicating that this element is in group 1. The graph of first ionisation energy against atomic number shows the grouping of electrons into s, p (and d) subshells (orbitals) within the (quantum shells) energy levels. The general trend is for ionisation energy to increase with increasing atomic number across a period but 1st IE B < 1st IE Be and 1st IE O < 1st IE N.
PRACTICE QUSTIONS
Label the diagram with symbols for the elements.
Label electrons removed as s or p.
Write two sentences using the frame: The ionisation energy (increases/decreases) (from left to right across a period/down a group) because (distance from outer electrons to nucleus is increasing/the nuclear charge in increasing)
Monday, December 15, 2008
Saturday, December 13, 2008
Revision sheet
Chemistry of elements
1. In the periodic table the elements are arranged according to the ………………
……………. Number
2. In the periodic table the elements are arranged according to the ………………
……………. No of particle in the nucleus
3. Give any two property of metal
………………………………………………………………………………….
4. Give any two properties of non metal
……………………………………...
5. NAME THE FIRST GROUP ELEMENTS
……………………………………………..
6. Name the second group elements
…………………………………………………….
7. Name the seventh group elements
………………………………….
8. Group 1 element are always has a …………………. Charge
9. Group 2 element are always has a …………………. Charge
9. Group 7 element are always has a …………………. Charge
10. Group 6 element are always has a …………………. Charge
11. Element A put in water to produce a gas B
And an alkali C It will give lilac color to the flame
Name the element A ……………………
Name the gas B ………………………………………….
NAME THE ALKALI C ………………………………………
Write three things that you see in this experiment
………………………………………………………………………………………………
……………………………………………………………………
What is color change shown by the universal indicator in the solution?
………………………………………….
12. Write down the word equation for the above reaction
…………………………………………………..
13. Write down the balanced equation for the above reaction
…………………………………………………..
14. What is the effect of blue litmus red litmus in the beaker
…………………………………………
15. How will you test the gas evolved………………………………
16. Name a non metal for the same period as lithium ………………………..
17. Name another metal in the same period as lithium……………………………..
18. What is similar in the arrangement of electron in alkali metals?
…………………………………………….
19. Why diamond and graphite have similar properties
………………………………………….
20. Why diamond and graphite have different properties
………………………………………….
21why graphite conducts electricity but diamond not. Why?
………………………………………………………………………………………..
22. Give the equation for the burning of graphite in air
…………………………………………………………..
23.give the word equation for the burning of magnesium
……………………………………………………..
24.
halogen
colour
Physical state
chlorine
fluorine
bromine
Periodic table
1. Periodic table is the arrangement of elements according to…………………………
2. Periodic table contains 3/4…………… and 1/4………………………………
3. Define semimetals
……………………………………………………………………………
4. Give examples……………………………….
5. Give uses of metalloids …………………………………………
6. Name a non metal in the same period as lithium……………………………
7. Elements in the same group have …………….. Properties
1. Same 2. Similar
8. Group one elements are having similar properties. Why?
………………………………………………………………………………
9. The vertical columns are called ………………, there are ……….no of groups
10. Horizontal columns are called ………………, there are ……….no of periods
10 give the uses of noble gases ……………………………………….
11. Why noble gases are uncreative……………………………………………………………………………………………………………………………………………….
12. Name the group I elements ………………………………………………………..
13. In group I the reactivity increases down the group …………………………………………………………………………………………………………………………………………………
14why potassium is more reactive than sodium …………………………………………………………………………………………………………………………………………………
15. Name the gas produced when sodium is kept in water. Give effect of litmus in the remaining solution ……………………………………………………………..
16. Write down three observations that you see when sodium is kept in water
……………………………………………………………………………………………
17. Give the reaction of group I metals( sodium, potassium,lithum) in water. Write the balances equation
…………………………………………………………………………………….
…………………………………………………………………………………….
17. Give the reaction of group 2 metals (magnesium, calcium) in water. Write the balances equation ………………………………………………………………………………………………………………………………………………………………
Work sheet
1.Which of the following is ionic compound? Why?
Element
Melting point
A
6754 C
B
31 C
ANS …………………………………………
WHY? ………………………………………………………………………………………………
…………………………………………………………………
2.Draw and explain the structure of diamond
3.Why magnesium chloride is having a high melting point than sodium chloride
4.Molten sodium chloride conducts electricity. Why?
5 .Molten sodium chloride conducts electricity. Why?
6. Graphite is a good conductor of electricity .why?
7. Why sodium chloride do not conduct electricity in solid state
8. Graphite is having a high sublimation point .why?
9. Give the structure of silicon dioxide
……………………………………………………………………………..
10. Give the structure of solid carbon dioxide
……………………………………………………………………………..
11. Give the structure of diamond
……………………………………………………………………………..
12. Give the structure of copper
……………………………………………………………………………..
13. Give the structure of solid methane
……………………………………………………………………………..
14. Give the structure of sodium chloride
……………………………………………………………………………..
15. Give the structure of graphite
……………………………………………………………………………..
16. Why diamond and graphite is having similar properties
……………………………………………………………………………………….
17. Why diamond and graphite is having different properties
……………………………………………………………………………………….
18. Draw the dot and cross diagram
Calcium chloride
Hydrogen
Chlorine molecule
Magnesium oxide
19.Draw the dot and cross diagram of the following. (USE THE PERIODIC TABLE)
N N
O C O
20.A small piece of potassium per magnate is kept in a beaker of water. What will be the observation after some minutes?
………………………………………………………………………………………………
……………………………………………………………………………
Name the phenomenon
………………………………………………………………………………
If you using hot water in place of cold what is the observation
………………………………………………
……………………………………….
Reason ………………………………………………………………………………………………
…………………………………………………………………………………….
21.Draw the particle arrange in gas and liquid
22.Explain in terms of kinetic theory what happen if the temperature of a solid is increased
………………………………………………………………………………………………
………………………………………………………………………………………………
………………………………………………………………………………………………
……………………………………………………….
A pollen grain is kept under beaker of water what do you observe through the microscope
Name………………………………………………………..
Draw the path
1. Draw the bonding in metals
2. Why metals are malleable
3. Why metals conduct electricity
4. Sodium chloride is having a high melting point. why?
5. Draw and explain the structure of diamond
6. Diamond is having a high melting point .why?
7. Why sodium chloride do not conduct electricity in solid state
8. Diamond is having a high sublimation point .why?
9. Why is diamond used for cutting?
10. Draw the structure of sodium chloride and magnesium chloride
11Why magnesium chloride is having a high melting point than sodium chloride
12.Molten sodium chloride conducts electricity. Why?
13.Define alloys. Why they are hard. Draw the structure of alloys
1. In the periodic table the elements are arranged according to the ………………
……………. Number
2. In the periodic table the elements are arranged according to the ………………
……………. No of particle in the nucleus
3. Give any two property of metal
………………………………………………………………………………….
4. Give any two properties of non metal
……………………………………...
5. NAME THE FIRST GROUP ELEMENTS
……………………………………………..
6. Name the second group elements
…………………………………………………….
7. Name the seventh group elements
………………………………….
8. Group 1 element are always has a …………………. Charge
9. Group 2 element are always has a …………………. Charge
9. Group 7 element are always has a …………………. Charge
10. Group 6 element are always has a …………………. Charge
11. Element A put in water to produce a gas B
And an alkali C It will give lilac color to the flame
Name the element A ……………………
Name the gas B ………………………………………….
NAME THE ALKALI C ………………………………………
Write three things that you see in this experiment
………………………………………………………………………………………………
……………………………………………………………………
What is color change shown by the universal indicator in the solution?
………………………………………….
12. Write down the word equation for the above reaction
…………………………………………………..
13. Write down the balanced equation for the above reaction
…………………………………………………..
14. What is the effect of blue litmus red litmus in the beaker
…………………………………………
15. How will you test the gas evolved………………………………
16. Name a non metal for the same period as lithium ………………………..
17. Name another metal in the same period as lithium……………………………..
18. What is similar in the arrangement of electron in alkali metals?
…………………………………………….
19. Why diamond and graphite have similar properties
………………………………………….
20. Why diamond and graphite have different properties
………………………………………….
21why graphite conducts electricity but diamond not. Why?
………………………………………………………………………………………..
22. Give the equation for the burning of graphite in air
…………………………………………………………..
23.give the word equation for the burning of magnesium
……………………………………………………..
24.
halogen
colour
Physical state
chlorine
fluorine
bromine
iodine
25. How will you convert the hydrogen chloride gas into hydrochloric acid?
……………………………………………..
26. A solution in which the hydrochloric acid is dissolved is tested with blue litmus. What do you observe?
…………………………………………………………………………………
27. Hydro choric acid is dissolved in methyl benzene. What do the change in the blue litmus?
……………………………………………………….
28. Describe the laboratory preparation of chlorine from hydro choric acid ( important)
………………………………………………………………………………………
………………………………………………………………………………..
29. Name the oxidizing agent in this reaction……………………………………
30. Give the test for chlorine…………………………………………………………….
31. Chlorine and bromine have similar properties why?
……………………………………………………………………………….
32. Chlorine is passed through a solution of potassium bromide
Name the type of reaction………………………………………….
The solution became red in color. Why?
…………………………………………………………………………..
Explain why no displacement reaction when we add bromine to potassium chloride …………………………………………………………………………………………
Write the ionic equation for the reaction……………………………………………….
Chlorine is bubbled through the potassium iodide solution. What will be the color of the
Final solution ……………………………………………..
Write down the ionic half equation for the reaction …………………………………
What is the color change during the below reaction
……………………………………………………
H2 + Cl 2___________ 2HCl
Name the process of the industrial extraction of oxygen
………………………………………………..
complete the table
78 %
21%
.9%
What is oxidation?
……………………………………….
What is reduction?
…………………………
Give example for oxidizing agent
…………………………………………….
Give example for reducing agent
………………………………………
Complete these reactions ( balance )
S+ O2__________
Fe + O2__________
Mg + O2 _____________
Cu + O 2_________
C +O 2 ___________
CH4 + O2_____________
Describe an experiment to determine the % of oxygen in air (copper turning )
Give the reaction of sulphur dioxide with water
…………………………………………….
Give two equations for the reactions in contact process ( impor)
…………………………………………………………….
……………………………………………………….
Which one is reversible reaction?
……………………………………………
Describe the laboratory preparation of carbon dioxide
Give the equation for reaction
……………………………………………………………………………….
Give the uses of carbon dioxide
………………………………………………………………
What is dry ice?
……………………………
Give two uses of dry ice
………………………………………..
Give the reaction of nitrogen with oxygen ( 2 equations)
…………………………………………………….
…………………………………………………..
Give the conditions needed for the rusting of iron
……………………………………………………………………………….
Give method for the prevention of rusting
……………………………………………………………………………..
How this method work in preventing rusting of iron
……………………………………………………………………………
Explain sacrificial protection. Give example.
……………………………………………………………………………….
Sodium can be prepared by electrolysis only were as iron fro blast furnace give your answer (in terms of reactivity)
………………………………………………………………………………………
Give the allotropes of sulphur
……………………………………………………………………………
Name the process by which nitrogen is industrially extracted
………………………………………………………………..
Give one use of nitrogen
……………………………………….
Why nitrogen is used for protecting dry foods
……………………………………………….
Describe the laboratory preparation of ammonia (page-244 text book)
Give the equation for the preparation
………………………………………………………………..
Give physical properties of ammonia
………………………………………………………………………………………
ammonia dissolve in water forms …………………………………………
give the equation…………………………………………
Give the uses of ammonia
to prepare nitric acid
to prepare fertilizer
Give the reaction between sulphuric acid and ammonia ( important)
NH 3 + H2SO4 ----------- (NH4)2 SO4 ( AMMONIUM SULPHATE)
Give the reaction between NITRIC acid and ammonia ( important)
NH3+ HNO3 ------- NH 4 NO3( AMMONIUM NITRATE)
What are the elements present in NPK FERTILIZER?
………………………………………………………..
Describe the chemical test for water
……………………………………………………………..
Describe the physical test for water
………………………………………………………………
Describe the laboratory preparation of hydrogen
Name the gas produced when a metal react with dilute acid
…………………………………………………….
Give the test for this gas
…………………………………………………….
Give word equation for the reaction between hydrogen and oxygen
…………………………………………………..
Give balanced equation for the reaction between hydrogen and oxygen
…………………………………………………..
Give one example for transition metal which is used as catalyst
…………………………………………………….
Iron react with chlorine to form a yellow( brown) color solid
Name it…………………………….
Give equation for the reaction
…………………………………………………..
Give the color of ion with sodium hydroxide
Fe2+ …………………
Fe3+…………………
Cu2+ ………………
Name the compounds……………………………………………………..
Write down the action of iron over steam. Give the balanced equation ( notes)
…………………………………………………………………..
Write down the action of iron hydrogen chloride gas Give the balanced equation (notes)
………………………………………………………………………….
Color
Copper oxide-red
Copper hydroxide – blue
Copper nitrate –green
Copper sulfate- blue
Copper carbonate-black
Copper chloride- green
Write down the reaction of ammonia with copper (II) ions ( important)
………………………………………………………………………………
Give the properties of transitional metals( answer given below)
1) variable valency
2) colored compounds
3) catalytic property
Give example for Fe shows variable valency
…………………………………………………………………….
What is reactivity series? Give the order
…………………………………………………………………………………
What do you know about the reactivity of and displacement reaction?
………………………………………………………………………….
A copper dipped in silver nitrate solution .What is observation that you see
After 2hours…………………………………………………….
.
Iron nail dipped in copper sulphate ……………………………………
Silver nail dipped ii copper sulphate……………………………………
Copper nail in iron sulphate……………………………..
(Important portion)
Cat ion
Flame color
Lithium(Li+)
Sodium (Na+)
Potassium( k+)
Calcium( ca2+)
gas
test
result
oxygen
carbon dioxide
hydrogen
chlorine
Sulpher dioxide
ammonia
Test for anions
TEST
result
Chloride(Cl-)
Bromide(Br -
Iodide (I-)
Sulphate(so42+)
Sulphite( S2_)
Carbonate(CO32_)
Test for cat ion
TEST
result
Ammonia (NH4+)
Copper (Cu2+)
Iron( Fe2+)
Iron ( Fe3+)
1. Name the three particles in the atom
2. ……………………………….. is the negative particle in the atom
3. …………………………………..is the positive particle in an atom
4 …………………………………… is the neutral particle in the atom
5. In an atom the number of ……………………………and
…………………………. are same
6. Name the particle out side the nucleus
7. Name the negligible particle in an atom
8. The mass of the atom is concentrated at …………………
9. Define atomic number
………………………………………………………………………………………………
…………………………………………………………………………………………….
10. Define mass number
………………………………………………………………………………………………
………………………………………………………………………………………………
11. find the 1) mass number2) atomic number 3) no. of neutron 4) no. of protons 5) no. of electron
12. Define isotope
………………………………………………………………………………………………
………………………………………………………………………………………………
13. Which one pair of the following is isotope?
Ans…………………………………
14. The following pair represents some gases
Which is 1) mono atomic …………………………..
2) Water molecule …………………………………
3) Mixture of gases ……………………………….
4) Elements ……………………………………….
5) Compounds………………………………………
6) Diatomic molecule ………………………………
15. Define element. Give example
……………………………………………………………………………………………
16. Carbon dioxide is a compound. What is a compound?
…………………………………………………………………………………………
17. Which one of the following belongs to the second group?
Ans : ……………………………………….
Give your answer
……………………………………………………………………………………………
Name the element ……………………………………………….(use periodic table)
18. find the outer electrons in the following atoms
1) bromine 2) carbon 3) boron
19) How many outer electrons are their in radium, iodine and radon
19) The below fig shows the nucleus of an atom
Find the atomic no……………………………
Mass no …………………………………
No of electrons ………………………………….
This atom belongs to ……………………………..group of the periodic table.
Give your answer for the above statement ………………………………………………………………………………………………
…………………………………………………………….
Work sheet 2
States of matter
define matter
complete the fig
A ……………………………
B……………………………..
c………………………………
D……………………………
E………………………………
complete the arrangement of solid particle
Explain what happens when a solid changes to liquid. give your answer using kinetic theory.
define sublimation
Define diffusion. Give example.
A small piece of potassium permanganate is kept under a beaker of water for one hour. What do you see after one hour?
A small piece of copper sulphate ( blue color) is kept under a beaker of water for one hour. What do you see after one hour?
Bromine vapor is kept in a jar and the lid is removed. What do you see after 10
min
A pollen grain is kept on the surface of water and viewed through the micro scope.
What do you see ……………………………………………………………………
Draw the path of the pollen grain
What is dry ice? How is it prepared? Give the use.
A smoke particle in air is viewed through the micro scope.
What do you see ……………………………………………………………………
Draw the path of the smoke particle
1. How will you find the purity of a solid?
…………………………………………………………………………………………
…………………………………………………………………………………………
………………………………………………………………………………… 2
2. Table below shows the melting and boiling points of some substance
SUBSTANCE
MELTING POINT
BOILING POINT
A
-123
-56
B
0
100
C
45
111
D
-23
23
E
-11
1
1) which one of the following is representing water
………………………………………………..
2) which one is a solid at room temperature
………………………………………………….
3) which substances are liquids at -15 c
………………………………………………….
4) which substance a liquid at short range of temperature
……………………………………………………….
3) The below graph represent the meting of a solid
What is the physical state at?
A ……………………………………………
B ………………………………………………..
C …………………………………………….
D ……………………………………………….
WHAT IS THE MELTING POINT
…………………………………
What is the boiling point?
……………………………………….
Some salt is added to the solid what will be the observation in boiling and melting point
……………………………………………………………………..
Reason ………………………………………………………………………………………………
A small piece of potassium per magnate is kept in a beaker of water. What will be the observation after some minutes?
………………………………………………………………………………………………
……………………………………………………………………………
Name the phenomenon
………………………………………………………………………………
If you using hot water in place of cold what is the observation
………………………………………………………………………………………………
……………………………………….
Reason ………………………………………………………………………………………………
…………………………………………………………………………………….
Draw the particle arrange in gas and liquid
Explain in terms of kinetic theory what happen if the temperature of a solid is increased
………………………………………………………………………………………………
………………………………………………………………………………………………
………………………………………………………………………………………………
……………………………………………………….
In the below diagram shows piece of potassium per magnate kept under water
(The substance is purple in color)
What do you see after 1hour?
Observation …………………………………………………………………………………………
Name it and define
………………………………………………………………………………………………
………………………………………………………………………………………………
……………………………………………….
Explain what happen if use hot water
………………………………………………………………………………
Reason ………………………………………………………………………………………………
………………………………………………………………………………………………
………………………………………………………………
The below apparatus shows diffusion
1) Which one diffuse fast? Why?..........................................................................................................................
...................................................
2) what happens if you hot solution
………………………………………………………………………………………
…………………………
A pollen grain is kept under beaker of water what do you observe through the microscope
Name………………………………………………………..
Draw the path
Atomic structure
1) Which one is mono atomic gas ………………….
2) Which one are an element ……………………………………
3) Which one are compounds ……………………………………….
4) Which one represent solid…………………………….
5) Which one represent liquid……………………..
6) Which one represent water molecule ……………………
7) Which one represent oxygen molecule ………………………..
8) Which one represent argon …………………………………
1. How will you find the purity of a solid?
…………………………………………………………………………………………
…………………………………………………………………………………………
………………………………………………………………………………… 2
2. Table below shows the melting and boiling points of some substance
SUBSTANCE
MELTING POINT
BOILING POINT
A
-123
-56
B
0
100
C
45
111
D
-23
23
E
-11
1
5) which one of the following is representing water
………………………………………………..
6) which one is a solid at room temperature
………………………………………………….
7) which substances are liquids at -15 c
………………………………………………….
8) which substance a liquid at short range of temperature
……………………………………………………….
3) The below graph represent the meting of a solid
What is the physical state at?
A ……………………………………………
B ………………………………………………..
C …………………………………………….
D ……………………………………………….
WHAT IS THE MELTING POINT
…………………………………
What is the boiling point?
……………………………………….
Some salt is added to the solid what will be the observation in boiling and melting point
……………………………………………………………………..
Reason ………………………………………………………………………………………………
A small piece of potassium per magnate is kept in a beaker of water. What will be the observation after some minutes?
………………………………………………………………………………………………
……………………………………………………………………………
Name the phenomenon
………………………………………………………………………………
If you using hot water in place of cold what is the observation
………………………………………………………………………………………………
……………………………………….
Reason ………………………………………………………………………………………………
…………………………………………………………………………………….
Draw the particle arrange in gas and liquid
Explain in terms of kinetic theory what happen if the temperature of a solid is increased
………………………………………………………………………………………………
………………………………………………………………………………………………
………………………………………………………………………………………………
……………………………………………………….
In the below diagram shows piece of potassium per magnate kept under water
(The substance is purple in color)
What do you see after 1hour?
Observation …………………………………………………………………………………………
Name it and define
………………………………………………………………………………………………
………………………………………………………………………………………………
……………………………………………….
Explain what happen if use hot water
………………………………………………………………………………
Reason ………………………………………………………………………………………………
………………………………………………………………………………………………
………………………………………………………………
The below apparatus shows diffusion
3) Which one diffuse fast? Why?..........................................................................................................................
...................................................
4) what happens if you hot solution
………………………………………………………………………………………
…………………………
A pollen grain is kept under beaker of water what do you observe through the microscope
Name………………………………………………………..
Draw the path
Atomic structure
9) Which one is mono atomic gas ………………….
10) Which one are an element ……………………………………
11) Which one are compounds ……………………………………….
12) Which one represent solid…………………………….
13) Which one represent liquid……………………..
14) Which one represent water molecule ……………………
15) Which one represent oxygen molecule ………………………..
16) Which one represent argon …………………………………
define ionic bonding
………………………………………………………………………………………………
…………………………………………………………………..
draw the dot and cross diagram
Lithium fluoride
Calcium chloride
Magnesium oxide
Calcium chloride
Potassium chloride
Magnesium oxide is having a high melting point than sodium chloride why?
Which one of the following is an ion?
Draw the electronic configuration of chloride ion
Draw the electronic configuration of following
Define covalent bonding
Draw the cross and dot diagram for the following
Hydrogen
Water
Methane
Hydrogen chloride
Nitrogen
Ehane
Carbondixide
iodine
25. How will you convert the hydrogen chloride gas into hydrochloric acid?
……………………………………………..
26. A solution in which the hydrochloric acid is dissolved is tested with blue litmus. What do you observe?
…………………………………………………………………………………
27. Hydro choric acid is dissolved in methyl benzene. What do the change in the blue litmus?
……………………………………………………….
28. Describe the laboratory preparation of chlorine from hydro choric acid ( important)
………………………………………………………………………………………
………………………………………………………………………………..
29. Name the oxidizing agent in this reaction……………………………………
30. Give the test for chlorine…………………………………………………………….
31. Chlorine and bromine have similar properties why?
……………………………………………………………………………….
32. Chlorine is passed through a solution of potassium bromide
Name the type of reaction………………………………………….
The solution became red in color. Why?
…………………………………………………………………………..
Explain why no displacement reaction when we add bromine to potassium chloride …………………………………………………………………………………………
Write the ionic equation for the reaction……………………………………………….
Chlorine is bubbled through the potassium iodide solution. What will be the color of the
Final solution ……………………………………………..
Write down the ionic half equation for the reaction …………………………………
What is the color change during the below reaction
……………………………………………………
H2 + Cl 2___________ 2HCl
Name the process of the industrial extraction of oxygen
………………………………………………..
complete the table
78 %
21%
.9%
What is oxidation?
……………………………………….
What is reduction?
…………………………
Give example for oxidizing agent
…………………………………………….
Give example for reducing agent
………………………………………
Complete these reactions ( balance )
S+ O2__________
Fe + O2__________
Mg + O2 _____________
Cu + O 2_________
C +O 2 ___________
CH4 + O2_____________
Describe an experiment to determine the % of oxygen in air (copper turning )
Give the reaction of sulphur dioxide with water
…………………………………………….
Give two equations for the reactions in contact process ( impor)
…………………………………………………………….
……………………………………………………….
Which one is reversible reaction?
……………………………………………
Describe the laboratory preparation of carbon dioxide
Give the equation for reaction
……………………………………………………………………………….
Give the uses of carbon dioxide
………………………………………………………………
What is dry ice?
……………………………
Give two uses of dry ice
………………………………………..
Give the reaction of nitrogen with oxygen ( 2 equations)
…………………………………………………….
…………………………………………………..
Give the conditions needed for the rusting of iron
……………………………………………………………………………….
Give method for the prevention of rusting
……………………………………………………………………………..
How this method work in preventing rusting of iron
……………………………………………………………………………
Explain sacrificial protection. Give example.
……………………………………………………………………………….
Sodium can be prepared by electrolysis only were as iron fro blast furnace give your answer (in terms of reactivity)
………………………………………………………………………………………
Give the allotropes of sulphur
……………………………………………………………………………
Name the process by which nitrogen is industrially extracted
………………………………………………………………..
Give one use of nitrogen
……………………………………….
Why nitrogen is used for protecting dry foods
……………………………………………….
Describe the laboratory preparation of ammonia (page-244 text book)
Give the equation for the preparation
………………………………………………………………..
Give physical properties of ammonia
………………………………………………………………………………………
ammonia dissolve in water forms …………………………………………
give the equation…………………………………………
Give the uses of ammonia
to prepare nitric acid
to prepare fertilizer
Give the reaction between sulphuric acid and ammonia ( important)
NH 3 + H2SO4 ----------- (NH4)2 SO4 ( AMMONIUM SULPHATE)
Give the reaction between NITRIC acid and ammonia ( important)
NH3+ HNO3 ------- NH 4 NO3( AMMONIUM NITRATE)
What are the elements present in NPK FERTILIZER?
………………………………………………………..
Describe the chemical test for water
……………………………………………………………..
Describe the physical test for water
………………………………………………………………
Describe the laboratory preparation of hydrogen
Name the gas produced when a metal react with dilute acid
…………………………………………………….
Give the test for this gas
…………………………………………………….
Give word equation for the reaction between hydrogen and oxygen
…………………………………………………..
Give balanced equation for the reaction between hydrogen and oxygen
…………………………………………………..
Give one example for transition metal which is used as catalyst
…………………………………………………….
Iron react with chlorine to form a yellow( brown) color solid
Name it…………………………….
Give equation for the reaction
…………………………………………………..
Give the color of ion with sodium hydroxide
Fe2+ …………………
Fe3+…………………
Cu2+ ………………
Name the compounds……………………………………………………..
Write down the action of iron over steam. Give the balanced equation ( notes)
…………………………………………………………………..
Write down the action of iron hydrogen chloride gas Give the balanced equation (notes)
………………………………………………………………………….
Color
Copper oxide-red
Copper hydroxide – blue
Copper nitrate –green
Copper sulfate- blue
Copper carbonate-black
Copper chloride- green
Write down the reaction of ammonia with copper (II) ions ( important)
………………………………………………………………………………
Give the properties of transitional metals( answer given below)
1) variable valency
2) colored compounds
3) catalytic property
Give example for Fe shows variable valency
…………………………………………………………………….
What is reactivity series? Give the order
…………………………………………………………………………………
What do you know about the reactivity of and displacement reaction?
………………………………………………………………………….
A copper dipped in silver nitrate solution .What is observation that you see
After 2hours…………………………………………………….
.
Iron nail dipped in copper sulphate ……………………………………
Silver nail dipped ii copper sulphate……………………………………
Copper nail in iron sulphate……………………………..
(Important portion)
Cat ion
Flame color
Lithium(Li+)
Sodium (Na+)
Potassium( k+)
Calcium( ca2+)
gas
test
result
oxygen
carbon dioxide
hydrogen
chlorine
Sulpher dioxide
ammonia
Test for anions
TEST
result
Chloride(Cl-)
Bromide(Br -
Iodide (I-)
Sulphate(so42+)
Sulphite( S2_)
Carbonate(CO32_)
Test for cat ion
TEST
result
Ammonia (NH4+)
Copper (Cu2+)
Iron( Fe2+)
Iron ( Fe3+)
Chemistry of elements
1. In the periodic table the elements are arranged according to the ………………
……………. Number
2. In the periodic table the elements are arranged according to the ………………
……………. No of particle in the nucleus
3. Give any two property of metal
………………………………………………………………………………….
4. Give any two properties of non metal
……………………………………...
5. NAME THE FIRST GROUP ELEMENTS
……………………………………………..
6. Name the second group elements
…………………………………………………….
7. Name the seventh group elements
………………………………….
8. Group 1 element are always has a …………………. Charge
9. Group 2 element are always has a …………………. Charge
9. Group 7 element are always has a …………………. Charge
10. Group 6 element are always has a …………………. Charge
11. Element A put in water to produce a gas B
And an alkali C It will give lilac color to the flame
Name the element A ……………………
Name the gas B ………………………………………….
NAME THE ALKALI C ………………………………………
Write three things that you see in this experiment
………………………………………………………………………………………………
……………………………………………………………………
What is color change shown by the universal indicator in the solution?
………………………………………….
12. Write down the word equation for the above reaction
…………………………………………………..
13. Write down the balanced equation for the above reaction
…………………………………………………..
14. What is the effect of blue litmus red litmus in the beaker
…………………………………………
15. How will you test the gas evolved………………………………
16. Name a non metal for the same period as lithium ………………………..
17. Name another metal in the same period as lithium……………………………..
18. What is similar in the arrangement of electron in alkali metals?
…………………………………………….
19. Why diamond and graphite have similar properties
………………………………………….
20. Why diamond and graphite have different properties
………………………………………….
21why graphite conducts electricity but diamond not. Why?
………………………………………………………………………………………..
22. Give the equation for the burning of graphite in air
…………………………………………………………..
23.give the word equation for the burning of magnesium
……………………………………………………..
24.
halogen
colour
Physical state
chlorine
fluorine
bromine
Periodic table
1. Periodic table is the arrangement of elements according to…………………………
2. Periodic table contains 3/4…………… and 1/4………………………………
3. Define semimetals
……………………………………………………………………………
4. Give examples……………………………….
5. Give uses of metalloids …………………………………………
6. Name a non metal in the same period as lithium……………………………
7. Elements in the same group have …………….. Properties
1. Same 2. Similar
8. Group one elements are having similar properties. Why?
………………………………………………………………………………
9. The vertical columns are called ………………, there are ……….no of groups
10. Horizontal columns are called ………………, there are ……….no of periods
10 give the uses of noble gases ……………………………………….
11. Why noble gases are uncreative……………………………………………………………………………………………………………………………………………….
12. Name the group I elements ………………………………………………………..
13. In group I the reactivity increases down the group …………………………………………………………………………………………………………………………………………………
14why potassium is more reactive than sodium …………………………………………………………………………………………………………………………………………………
15. Name the gas produced when sodium is kept in water. Give effect of litmus in the remaining solution ……………………………………………………………..
16. Write down three observations that you see when sodium is kept in water
……………………………………………………………………………………………
17. Give the reaction of group I metals( sodium, potassium,lithum) in water. Write the balances equation
…………………………………………………………………………………….
…………………………………………………………………………………….
17. Give the reaction of group 2 metals (magnesium, calcium) in water. Write the balances equation ………………………………………………………………………………………………………………………………………………………………
Work sheet
1.Which of the following is ionic compound? Why?
Element
Melting point
A
6754 C
B
31 C
ANS …………………………………………
WHY? ………………………………………………………………………………………………
…………………………………………………………………
2.Draw and explain the structure of diamond
3.Why magnesium chloride is having a high melting point than sodium chloride
4.Molten sodium chloride conducts electricity. Why?
5 .Molten sodium chloride conducts electricity. Why?
6. Graphite is a good conductor of electricity .why?
7. Why sodium chloride do not conduct electricity in solid state
8. Graphite is having a high sublimation point .why?
9. Give the structure of silicon dioxide
……………………………………………………………………………..
10. Give the structure of solid carbon dioxide
……………………………………………………………………………..
11. Give the structure of diamond
……………………………………………………………………………..
12. Give the structure of copper
……………………………………………………………………………..
13. Give the structure of solid methane
……………………………………………………………………………..
14. Give the structure of sodium chloride
……………………………………………………………………………..
15. Give the structure of graphite
……………………………………………………………………………..
16. Why diamond and graphite is having similar properties
……………………………………………………………………………………….
17. Why diamond and graphite is having different properties
……………………………………………………………………………………….
18. Draw the dot and cross diagram
Calcium chloride
Hydrogen
Chlorine molecule
Magnesium oxide
19.Draw the dot and cross diagram of the following. (USE THE PERIODIC TABLE)
N N
O C O
20.A small piece of potassium per magnate is kept in a beaker of water. What will be the observation after some minutes?
………………………………………………………………………………………………
……………………………………………………………………………
Name the phenomenon
………………………………………………………………………………
If you using hot water in place of cold what is the observation
………………………………………………
……………………………………….
Reason ………………………………………………………………………………………………
…………………………………………………………………………………….
21.Draw the particle arrange in gas and liquid
22.Explain in terms of kinetic theory what happen if the temperature of a solid is increased
………………………………………………………………………………………………
………………………………………………………………………………………………
………………………………………………………………………………………………
……………………………………………………….
A pollen grain is kept under beaker of water what do you observe through the microscope
Name………………………………………………………..
Draw the path
1. Draw the bonding in metals
2. Why metals are malleable
3. Why metals conduct electricity
4. Sodium chloride is having a high melting point. why?
5. Draw and explain the structure of diamond
6. Diamond is having a high melting point .why?
7. Why sodium chloride do not conduct electricity in solid state
8. Diamond is having a high sublimation point .why?
9. Why is diamond used for cutting?
10. Draw the structure of sodium chloride and magnesium chloride
11Why magnesium chloride is having a high melting point than sodium chloride
12.Molten sodium chloride conducts electricity. Why?
13.Define alloys. Why they are hard. Draw the structure of alloys
1. In the periodic table the elements are arranged according to the ………………
……………. Number
2. In the periodic table the elements are arranged according to the ………………
……………. No of particle in the nucleus
3. Give any two property of metal
………………………………………………………………………………….
4. Give any two properties of non metal
……………………………………...
5. NAME THE FIRST GROUP ELEMENTS
……………………………………………..
6. Name the second group elements
…………………………………………………….
7. Name the seventh group elements
………………………………….
8. Group 1 element are always has a …………………. Charge
9. Group 2 element are always has a …………………. Charge
9. Group 7 element are always has a …………………. Charge
10. Group 6 element are always has a …………………. Charge
11. Element A put in water to produce a gas B
And an alkali C It will give lilac color to the flame
Name the element A ……………………
Name the gas B ………………………………………….
NAME THE ALKALI C ………………………………………
Write three things that you see in this experiment
………………………………………………………………………………………………
……………………………………………………………………
What is color change shown by the universal indicator in the solution?
………………………………………….
12. Write down the word equation for the above reaction
…………………………………………………..
13. Write down the balanced equation for the above reaction
…………………………………………………..
14. What is the effect of blue litmus red litmus in the beaker
…………………………………………
15. How will you test the gas evolved………………………………
16. Name a non metal for the same period as lithium ………………………..
17. Name another metal in the same period as lithium……………………………..
18. What is similar in the arrangement of electron in alkali metals?
…………………………………………….
19. Why diamond and graphite have similar properties
………………………………………….
20. Why diamond and graphite have different properties
………………………………………….
21why graphite conducts electricity but diamond not. Why?
………………………………………………………………………………………..
22. Give the equation for the burning of graphite in air
…………………………………………………………..
23.give the word equation for the burning of magnesium
……………………………………………………..
24.
halogen
colour
Physical state
chlorine
fluorine
bromine
iodine
25. How will you convert the hydrogen chloride gas into hydrochloric acid?
……………………………………………..
26. A solution in which the hydrochloric acid is dissolved is tested with blue litmus. What do you observe?
…………………………………………………………………………………
27. Hydro choric acid is dissolved in methyl benzene. What do the change in the blue litmus?
……………………………………………………….
28. Describe the laboratory preparation of chlorine from hydro choric acid ( important)
………………………………………………………………………………………
………………………………………………………………………………..
29. Name the oxidizing agent in this reaction……………………………………
30. Give the test for chlorine…………………………………………………………….
31. Chlorine and bromine have similar properties why?
……………………………………………………………………………….
32. Chlorine is passed through a solution of potassium bromide
Name the type of reaction………………………………………….
The solution became red in color. Why?
…………………………………………………………………………..
Explain why no displacement reaction when we add bromine to potassium chloride …………………………………………………………………………………………
Write the ionic equation for the reaction……………………………………………….
Chlorine is bubbled through the potassium iodide solution. What will be the color of the
Final solution ……………………………………………..
Write down the ionic half equation for the reaction …………………………………
What is the color change during the below reaction
……………………………………………………
H2 + Cl 2___________ 2HCl
Name the process of the industrial extraction of oxygen
………………………………………………..
complete the table
78 %
21%
.9%
What is oxidation?
……………………………………….
What is reduction?
…………………………
Give example for oxidizing agent
…………………………………………….
Give example for reducing agent
………………………………………
Complete these reactions ( balance )
S+ O2__________
Fe + O2__________
Mg + O2 _____________
Cu + O 2_________
C +O 2 ___________
CH4 + O2_____________
Describe an experiment to determine the % of oxygen in air (copper turning )
Give the reaction of sulphur dioxide with water
…………………………………………….
Give two equations for the reactions in contact process ( impor)
…………………………………………………………….
……………………………………………………….
Which one is reversible reaction?
……………………………………………
Describe the laboratory preparation of carbon dioxide
Give the equation for reaction
……………………………………………………………………………….
Give the uses of carbon dioxide
………………………………………………………………
What is dry ice?
……………………………
Give two uses of dry ice
………………………………………..
Give the reaction of nitrogen with oxygen ( 2 equations)
…………………………………………………….
…………………………………………………..
Give the conditions needed for the rusting of iron
……………………………………………………………………………….
Give method for the prevention of rusting
……………………………………………………………………………..
How this method work in preventing rusting of iron
……………………………………………………………………………
Explain sacrificial protection. Give example.
……………………………………………………………………………….
Sodium can be prepared by electrolysis only were as iron fro blast furnace give your answer (in terms of reactivity)
………………………………………………………………………………………
Give the allotropes of sulphur
……………………………………………………………………………
Name the process by which nitrogen is industrially extracted
………………………………………………………………..
Give one use of nitrogen
……………………………………….
Why nitrogen is used for protecting dry foods
……………………………………………….
Describe the laboratory preparation of ammonia (page-244 text book)
Give the equation for the preparation
………………………………………………………………..
Give physical properties of ammonia
………………………………………………………………………………………
ammonia dissolve in water forms …………………………………………
give the equation…………………………………………
Give the uses of ammonia
to prepare nitric acid
to prepare fertilizer
Give the reaction between sulphuric acid and ammonia ( important)
NH 3 + H2SO4 ----------- (NH4)2 SO4 ( AMMONIUM SULPHATE)
Give the reaction between NITRIC acid and ammonia ( important)
NH3+ HNO3 ------- NH 4 NO3( AMMONIUM NITRATE)
What are the elements present in NPK FERTILIZER?
………………………………………………………..
Describe the chemical test for water
……………………………………………………………..
Describe the physical test for water
………………………………………………………………
Describe the laboratory preparation of hydrogen
Name the gas produced when a metal react with dilute acid
…………………………………………………….
Give the test for this gas
…………………………………………………….
Give word equation for the reaction between hydrogen and oxygen
…………………………………………………..
Give balanced equation for the reaction between hydrogen and oxygen
…………………………………………………..
Give one example for transition metal which is used as catalyst
…………………………………………………….
Iron react with chlorine to form a yellow( brown) color solid
Name it…………………………….
Give equation for the reaction
…………………………………………………..
Give the color of ion with sodium hydroxide
Fe2+ …………………
Fe3+…………………
Cu2+ ………………
Name the compounds……………………………………………………..
Write down the action of iron over steam. Give the balanced equation ( notes)
…………………………………………………………………..
Write down the action of iron hydrogen chloride gas Give the balanced equation (notes)
………………………………………………………………………….
Color
Copper oxide-red
Copper hydroxide – blue
Copper nitrate –green
Copper sulfate- blue
Copper carbonate-black
Copper chloride- green
Write down the reaction of ammonia with copper (II) ions ( important)
………………………………………………………………………………
Give the properties of transitional metals( answer given below)
1) variable valency
2) colored compounds
3) catalytic property
Give example for Fe shows variable valency
…………………………………………………………………….
What is reactivity series? Give the order
…………………………………………………………………………………
What do you know about the reactivity of and displacement reaction?
………………………………………………………………………….
A copper dipped in silver nitrate solution .What is observation that you see
After 2hours…………………………………………………….
.
Iron nail dipped in copper sulphate ……………………………………
Silver nail dipped ii copper sulphate……………………………………
Copper nail in iron sulphate……………………………..
(Important portion)
Cat ion
Flame color
Lithium(Li+)
Sodium (Na+)
Potassium( k+)
Calcium( ca2+)
gas
test
result
oxygen
carbon dioxide
hydrogen
chlorine
Sulpher dioxide
ammonia
Test for anions
TEST
result
Chloride(Cl-)
Bromide(Br -
Iodide (I-)
Sulphate(so42+)
Sulphite( S2_)
Carbonate(CO32_)
Test for cat ion
TEST
result
Ammonia (NH4+)
Copper (Cu2+)
Iron( Fe2+)
Iron ( Fe3+)
1. Name the three particles in the atom
2. ……………………………….. is the negative particle in the atom
3. …………………………………..is the positive particle in an atom
4 …………………………………… is the neutral particle in the atom
5. In an atom the number of ……………………………and
…………………………. are same
6. Name the particle out side the nucleus
7. Name the negligible particle in an atom
8. The mass of the atom is concentrated at …………………
9. Define atomic number
………………………………………………………………………………………………
…………………………………………………………………………………………….
10. Define mass number
………………………………………………………………………………………………
………………………………………………………………………………………………
11. find the 1) mass number2) atomic number 3) no. of neutron 4) no. of protons 5) no. of electron
12. Define isotope
………………………………………………………………………………………………
………………………………………………………………………………………………
13. Which one pair of the following is isotope?
Ans…………………………………
14. The following pair represents some gases
Which is 1) mono atomic …………………………..
2) Water molecule …………………………………
3) Mixture of gases ……………………………….
4) Elements ……………………………………….
5) Compounds………………………………………
6) Diatomic molecule ………………………………
15. Define element. Give example
……………………………………………………………………………………………
16. Carbon dioxide is a compound. What is a compound?
…………………………………………………………………………………………
17. Which one of the following belongs to the second group?
Ans : ……………………………………….
Give your answer
……………………………………………………………………………………………
Name the element ……………………………………………….(use periodic table)
18. find the outer electrons in the following atoms
1) bromine 2) carbon 3) boron
19) How many outer electrons are their in radium, iodine and radon
19) The below fig shows the nucleus of an atom
Find the atomic no……………………………
Mass no …………………………………
No of electrons ………………………………….
This atom belongs to ……………………………..group of the periodic table.
Give your answer for the above statement ………………………………………………………………………………………………
…………………………………………………………….
Work sheet 2
States of matter
define matter
complete the fig
A ……………………………
B……………………………..
c………………………………
D……………………………
E………………………………
complete the arrangement of solid particle
Explain what happens when a solid changes to liquid. give your answer using kinetic theory.
define sublimation
Define diffusion. Give example.
A small piece of potassium permanganate is kept under a beaker of water for one hour. What do you see after one hour?
A small piece of copper sulphate ( blue color) is kept under a beaker of water for one hour. What do you see after one hour?
Bromine vapor is kept in a jar and the lid is removed. What do you see after 10
min
A pollen grain is kept on the surface of water and viewed through the micro scope.
What do you see ……………………………………………………………………
Draw the path of the pollen grain
What is dry ice? How is it prepared? Give the use.
A smoke particle in air is viewed through the micro scope.
What do you see ……………………………………………………………………
Draw the path of the smoke particle
1. How will you find the purity of a solid?
…………………………………………………………………………………………
…………………………………………………………………………………………
………………………………………………………………………………… 2
2. Table below shows the melting and boiling points of some substance
SUBSTANCE
MELTING POINT
BOILING POINT
A
-123
-56
B
0
100
C
45
111
D
-23
23
E
-11
1
1) which one of the following is representing water
………………………………………………..
2) which one is a solid at room temperature
………………………………………………….
3) which substances are liquids at -15 c
………………………………………………….
4) which substance a liquid at short range of temperature
……………………………………………………….
3) The below graph represent the meting of a solid
What is the physical state at?
A ……………………………………………
B ………………………………………………..
C …………………………………………….
D ……………………………………………….
WHAT IS THE MELTING POINT
…………………………………
What is the boiling point?
……………………………………….
Some salt is added to the solid what will be the observation in boiling and melting point
……………………………………………………………………..
Reason ………………………………………………………………………………………………
A small piece of potassium per magnate is kept in a beaker of water. What will be the observation after some minutes?
………………………………………………………………………………………………
……………………………………………………………………………
Name the phenomenon
………………………………………………………………………………
If you using hot water in place of cold what is the observation
………………………………………………………………………………………………
……………………………………….
Reason ………………………………………………………………………………………………
…………………………………………………………………………………….
Draw the particle arrange in gas and liquid
Explain in terms of kinetic theory what happen if the temperature of a solid is increased
………………………………………………………………………………………………
………………………………………………………………………………………………
………………………………………………………………………………………………
……………………………………………………….
In the below diagram shows piece of potassium per magnate kept under water
(The substance is purple in color)
What do you see after 1hour?
Observation …………………………………………………………………………………………
Name it and define
………………………………………………………………………………………………
………………………………………………………………………………………………
……………………………………………….
Explain what happen if use hot water
………………………………………………………………………………
Reason ………………………………………………………………………………………………
………………………………………………………………………………………………
………………………………………………………………
The below apparatus shows diffusion
1) Which one diffuse fast? Why?..........................................................................................................................
...................................................
2) what happens if you hot solution
………………………………………………………………………………………
…………………………
A pollen grain is kept under beaker of water what do you observe through the microscope
Name………………………………………………………..
Draw the path
Atomic structure
1) Which one is mono atomic gas ………………….
2) Which one are an element ……………………………………
3) Which one are compounds ……………………………………….
4) Which one represent solid…………………………….
5) Which one represent liquid……………………..
6) Which one represent water molecule ……………………
7) Which one represent oxygen molecule ………………………..
8) Which one represent argon …………………………………
1. How will you find the purity of a solid?
…………………………………………………………………………………………
…………………………………………………………………………………………
………………………………………………………………………………… 2
2. Table below shows the melting and boiling points of some substance
SUBSTANCE
MELTING POINT
BOILING POINT
A
-123
-56
B
0
100
C
45
111
D
-23
23
E
-11
1
5) which one of the following is representing water
………………………………………………..
6) which one is a solid at room temperature
………………………………………………….
7) which substances are liquids at -15 c
………………………………………………….
8) which substance a liquid at short range of temperature
……………………………………………………….
3) The below graph represent the meting of a solid
What is the physical state at?
A ……………………………………………
B ………………………………………………..
C …………………………………………….
D ……………………………………………….
WHAT IS THE MELTING POINT
…………………………………
What is the boiling point?
……………………………………….
Some salt is added to the solid what will be the observation in boiling and melting point
……………………………………………………………………..
Reason ………………………………………………………………………………………………
A small piece of potassium per magnate is kept in a beaker of water. What will be the observation after some minutes?
………………………………………………………………………………………………
……………………………………………………………………………
Name the phenomenon
………………………………………………………………………………
If you using hot water in place of cold what is the observation
………………………………………………………………………………………………
……………………………………….
Reason ………………………………………………………………………………………………
…………………………………………………………………………………….
Draw the particle arrange in gas and liquid
Explain in terms of kinetic theory what happen if the temperature of a solid is increased
………………………………………………………………………………………………
………………………………………………………………………………………………
………………………………………………………………………………………………
……………………………………………………….
In the below diagram shows piece of potassium per magnate kept under water
(The substance is purple in color)
What do you see after 1hour?
Observation …………………………………………………………………………………………
Name it and define
………………………………………………………………………………………………
………………………………………………………………………………………………
……………………………………………….
Explain what happen if use hot water
………………………………………………………………………………
Reason ………………………………………………………………………………………………
………………………………………………………………………………………………
………………………………………………………………
The below apparatus shows diffusion
3) Which one diffuse fast? Why?..........................................................................................................................
...................................................
4) what happens if you hot solution
………………………………………………………………………………………
…………………………
A pollen grain is kept under beaker of water what do you observe through the microscope
Name………………………………………………………..
Draw the path
Atomic structure
9) Which one is mono atomic gas ………………….
10) Which one are an element ……………………………………
11) Which one are compounds ……………………………………….
12) Which one represent solid…………………………….
13) Which one represent liquid……………………..
14) Which one represent water molecule ……………………
15) Which one represent oxygen molecule ………………………..
16) Which one represent argon …………………………………
define ionic bonding
………………………………………………………………………………………………
…………………………………………………………………..
draw the dot and cross diagram
Lithium fluoride
Calcium chloride
Magnesium oxide
Calcium chloride
Potassium chloride
Magnesium oxide is having a high melting point than sodium chloride why?
Which one of the following is an ion?
Draw the electronic configuration of chloride ion
Draw the electronic configuration of following
Define covalent bonding
Draw the cross and dot diagram for the following
Hydrogen
Water
Methane
Hydrogen chloride
Nitrogen
Ehane
Carbondixide
iodine
25. How will you convert the hydrogen chloride gas into hydrochloric acid?
……………………………………………..
26. A solution in which the hydrochloric acid is dissolved is tested with blue litmus. What do you observe?
…………………………………………………………………………………
27. Hydro choric acid is dissolved in methyl benzene. What do the change in the blue litmus?
……………………………………………………….
28. Describe the laboratory preparation of chlorine from hydro choric acid ( important)
………………………………………………………………………………………
………………………………………………………………………………..
29. Name the oxidizing agent in this reaction……………………………………
30. Give the test for chlorine…………………………………………………………….
31. Chlorine and bromine have similar properties why?
……………………………………………………………………………….
32. Chlorine is passed through a solution of potassium bromide
Name the type of reaction………………………………………….
The solution became red in color. Why?
…………………………………………………………………………..
Explain why no displacement reaction when we add bromine to potassium chloride …………………………………………………………………………………………
Write the ionic equation for the reaction……………………………………………….
Chlorine is bubbled through the potassium iodide solution. What will be the color of the
Final solution ……………………………………………..
Write down the ionic half equation for the reaction …………………………………
What is the color change during the below reaction
……………………………………………………
H2 + Cl 2___________ 2HCl
Name the process of the industrial extraction of oxygen
………………………………………………..
complete the table
78 %
21%
.9%
What is oxidation?
……………………………………….
What is reduction?
…………………………
Give example for oxidizing agent
…………………………………………….
Give example for reducing agent
………………………………………
Complete these reactions ( balance )
S+ O2__________
Fe + O2__________
Mg + O2 _____________
Cu + O 2_________
C +O 2 ___________
CH4 + O2_____________
Describe an experiment to determine the % of oxygen in air (copper turning )
Give the reaction of sulphur dioxide with water
…………………………………………….
Give two equations for the reactions in contact process ( impor)
…………………………………………………………….
……………………………………………………….
Which one is reversible reaction?
……………………………………………
Describe the laboratory preparation of carbon dioxide
Give the equation for reaction
……………………………………………………………………………….
Give the uses of carbon dioxide
………………………………………………………………
What is dry ice?
……………………………
Give two uses of dry ice
………………………………………..
Give the reaction of nitrogen with oxygen ( 2 equations)
…………………………………………………….
…………………………………………………..
Give the conditions needed for the rusting of iron
……………………………………………………………………………….
Give method for the prevention of rusting
……………………………………………………………………………..
How this method work in preventing rusting of iron
……………………………………………………………………………
Explain sacrificial protection. Give example.
……………………………………………………………………………….
Sodium can be prepared by electrolysis only were as iron fro blast furnace give your answer (in terms of reactivity)
………………………………………………………………………………………
Give the allotropes of sulphur
……………………………………………………………………………
Name the process by which nitrogen is industrially extracted
………………………………………………………………..
Give one use of nitrogen
……………………………………….
Why nitrogen is used for protecting dry foods
……………………………………………….
Describe the laboratory preparation of ammonia (page-244 text book)
Give the equation for the preparation
………………………………………………………………..
Give physical properties of ammonia
………………………………………………………………………………………
ammonia dissolve in water forms …………………………………………
give the equation…………………………………………
Give the uses of ammonia
to prepare nitric acid
to prepare fertilizer
Give the reaction between sulphuric acid and ammonia ( important)
NH 3 + H2SO4 ----------- (NH4)2 SO4 ( AMMONIUM SULPHATE)
Give the reaction between NITRIC acid and ammonia ( important)
NH3+ HNO3 ------- NH 4 NO3( AMMONIUM NITRATE)
What are the elements present in NPK FERTILIZER?
………………………………………………………..
Describe the chemical test for water
……………………………………………………………..
Describe the physical test for water
………………………………………………………………
Describe the laboratory preparation of hydrogen
Name the gas produced when a metal react with dilute acid
…………………………………………………….
Give the test for this gas
…………………………………………………….
Give word equation for the reaction between hydrogen and oxygen
…………………………………………………..
Give balanced equation for the reaction between hydrogen and oxygen
…………………………………………………..
Give one example for transition metal which is used as catalyst
…………………………………………………….
Iron react with chlorine to form a yellow( brown) color solid
Name it…………………………….
Give equation for the reaction
…………………………………………………..
Give the color of ion with sodium hydroxide
Fe2+ …………………
Fe3+…………………
Cu2+ ………………
Name the compounds……………………………………………………..
Write down the action of iron over steam. Give the balanced equation ( notes)
…………………………………………………………………..
Write down the action of iron hydrogen chloride gas Give the balanced equation (notes)
………………………………………………………………………….
Color
Copper oxide-red
Copper hydroxide – blue
Copper nitrate –green
Copper sulfate- blue
Copper carbonate-black
Copper chloride- green
Write down the reaction of ammonia with copper (II) ions ( important)
………………………………………………………………………………
Give the properties of transitional metals( answer given below)
1) variable valency
2) colored compounds
3) catalytic property
Give example for Fe shows variable valency
…………………………………………………………………….
What is reactivity series? Give the order
…………………………………………………………………………………
What do you know about the reactivity of and displacement reaction?
………………………………………………………………………….
A copper dipped in silver nitrate solution .What is observation that you see
After 2hours…………………………………………………….
.
Iron nail dipped in copper sulphate ……………………………………
Silver nail dipped ii copper sulphate……………………………………
Copper nail in iron sulphate……………………………..
(Important portion)
Cat ion
Flame color
Lithium(Li+)
Sodium (Na+)
Potassium( k+)
Calcium( ca2+)
gas
test
result
oxygen
carbon dioxide
hydrogen
chlorine
Sulpher dioxide
ammonia
Test for anions
TEST
result
Chloride(Cl-)
Bromide(Br -
Iodide (I-)
Sulphate(so42+)
Sulphite( S2_)
Carbonate(CO32_)
Test for cat ion
TEST
result
Ammonia (NH4+)
Copper (Cu2+)
Iron( Fe2+)
Iron ( Fe3+)
Wednesday, November 26, 2008
Worksheet 4 / Periodic table
1. Periodic table is the arrangement of elements according to…………………………
2. Periodic table contains 3/4…………… and 1/4………………………………
3. Define semimetals
……………………………………………………………………………
4. Give examples……………………………….
5. Give uses of metalloids …………………………………………
6. Name a non metal in the same period as lithium……………………………
7. Elements in the same group have …………….. Properties
1. Same 2. Similar
8. Group one elements are having similar properties. Why?
………………………………………………………………………………
9. The vertical columns are called ………………, there are ……….no of groups
10. Horizontal columns are called ………………, there are ……….no of periods
10 give the uses of noble gases ……………………………………….
11. Why noble gases are uncreative……………………………………………………………………………………………………………………………………………….
12. Name the group I elements ………………………………………………………..
13. In group I the reactivity increases down the group …………………………………………………………………………………………………………………………………………………
14. Why potassium is more reactive than sodium …………………………………………………………………………………………………………………………………………………
15. Name the gas produced when sodium is kept in water. Give effect of litmus in the remaining solution ……………………………………………………………..
16. Write down three observations that you see when sodium is kept in water
……………………………………………………………………………………………
17. Give the reaction of group I metals (sodium, potassium, lithium) in water. Write the balances equation
…………………………………………………………………………………….
…………………………………………………………………………………….
17. Give the reaction of group 2 metals (magnesium, calcium) in water. Write the balances equation ………………………………………………………………………………………………………………………………………………………………
18. Which one of the following can form a single positive ion?
Sodium, chlorine, neon, calcium
………………………………………………………………………
1. Periodic table is the arrangement of elements according to…………………………
2. Periodic table contains 3/4…………… and 1/4………………………………
3. Define semimetals
……………………………………………………………………………
4. Give examples……………………………….
5. Give uses of metalloids …………………………………………
6. Name a non metal in the same period as lithium……………………………
7. Elements in the same group have …………….. Properties
1. Same 2. Similar
8. Group one elements are having similar properties. Why?
………………………………………………………………………………
9. The vertical columns are called ………………, there are ……….no of groups
10. Horizontal columns are called ………………, there are ……….no of periods
10 give the uses of noble gases ……………………………………….
11. Why noble gases are uncreative……………………………………………………………………………………………………………………………………………….
12. Name the group I elements ………………………………………………………..
13. In group I the reactivity increases down the group …………………………………………………………………………………………………………………………………………………
14. Why potassium is more reactive than sodium …………………………………………………………………………………………………………………………………………………
15. Name the gas produced when sodium is kept in water. Give effect of litmus in the remaining solution ……………………………………………………………..
16. Write down three observations that you see when sodium is kept in water
……………………………………………………………………………………………
17. Give the reaction of group I metals (sodium, potassium, lithium) in water. Write the balances equation
…………………………………………………………………………………….
…………………………………………………………………………………….
17. Give the reaction of group 2 metals (magnesium, calcium) in water. Write the balances equation ………………………………………………………………………………………………………………………………………………………………
18. Which one of the following can form a single positive ion?
Sodium, chlorine, neon, calcium
………………………………………………………………………
Work sheet
Alkanes
Reactions of alkanes
chlorination of methane
Give the Condition for the reaction: ………………………
--------------------------------------------------------------------------------
…………………………………………………………………………………………………………………………….
------------------------------------------------------------------------------
……………………………………………………………………………………………………………………………….
Give the equation for the burning of methane in air
----------------------------------------------------------
3. Draw the isotopes of butane and pentane
Alkenes
What are unsaturated compounds?
……………………………………………………………………………………………………………………………………….
2. Which one of the following are unsaturated compounds
Ans ……………………………..
Give the test for unsaturated compounds
--------------------------------------------------------------------------------------
Which one of the following can decolorize the bromine water?
………………………………………………………………………………………………………………………………………….
4.Draw the first 3 alkenes
What is cracking? ( imp)
-------------------------------------------------------------------------------------4. What are the conditions for cracking?
------------------------------------------------------------------------------
5. Give the complete equation for the following
C H ------------------ +
C H --------------------- +
C H ----------------------- +
COMPLETE COMBUTION OF HYDROCARBONS
Hydrocarbon + oxygen ----------------- +
Petrol + oxygen __________ +
Methane + oxygen __________ +
INCOMPLETE COMBUTION OF HYDROCARBONS (imp)
Hydrocarbon + oxygen ----------------- +
Petrol + oxygen __________ +
Methane + oxygen __________ +
6. Explain the health problem associated with the incomplete combustion of hydrocarbon
------------------------------------------------------------------------------
7. Give the environmental problem associated with burning of hydrocarbon
---------------------------------------------------------
Ethanol
1. What is the functional group in alcohol?
Draw the displayed formula of ethanol showing the entire bonds
2. Explain the two methods of preparation of ethanol
WHAT IS THE DIFFERENCE BETWEEN THE TWO METHOD
Hydration
fermentation
Which method is prefers in Middle East and in a cold country like Spain
Middle East ………………………………………………….
Reason………………………………………………………………………………………………………………………………
Spain ……………………………………………………………….
Reason………………………………………………………………………………………………………………………………
COMPOUND
FUNCTIONAL GROUP
ALCOHOL
ACID
ESTER
REACTIONS OF ALCOHOL
Natural oil and gas
Crude oil –
Explain FRACTIONAL DISTILATION OF CRUDE OIL
Uses of different fractions
Petrol -
Naphtha-
Kerosene-
Diesel -
Bitumen -
Boiling point and no of carbon atoms in a mixture of hydrocarbon
1. Boiling point and hydrocarbon are given below
Hydrocarbon
Boiling point
No of carbon atoms
gas
-40-40 c
C1-C4
petrol
40-100 c
C4-C8
Naphtha
100-160 c
C6-C10
kerosene
250-350c
C10-C16
Diesel oil
350-450c
C16-C20
What is the trend in the boiling point in the series? Relate the trend with the number of carbon atoms in the chain of each compound. GIVE THE REASON
………………………………………………………………………………………….
…………………………………………………………………………………
Synthetic polymers
1.What are Monomer------------------------------------------
-----------------------------------------------
2.Polymers –
…………………………………………………………………………………………..
3.Give the two types polymers – …………………………………………………………………..
4.Name the monomer of polyethene
5.Draw the repeating unit of polyethene
6. Draw the equation for the formation of polythene
7. Name the monomer of polypropene
………………………………………………………
8.Draw the repeating unit of poly propene
9.Draw the equation for the formation of polypropene
10.Name the monomer of polychloroethene
………………………………………………………………
11.Draw the repeating unit of polychloroethene
12.Draw the equation for the formation of polychloroethene
13Use of addition polymers
polymer
properties
Uses
Poly ethene
Polymer
Poly propene
Properties
Uses
Polymer
Properties
Uses
Poly chloro ethene
14.what are condensation polymers .give examples
15.Give the monomers of nylon
Carboxylic acid =
acid chloride =
Amines =
16. Draw the structure of nylon
Name the monomers…………………………………
Name the linkage …………………………………..
Name the molecule removed ……………………….
Give the type of condensation …………………………………
Name the polymer ……………………………….
2. Draw the structure of nylon
Name the monomers…………………………………
Name the linkage …………………………………..
Name the molecule removed ……………………….
Give the type of condensation …………………………………
Use of nylon –…………………………………………
Terelene (polyester )
17.Give the monomers of nylon
Carboxylic acid =
Diol =
18. Draw the structure of terelene
Name the monomers…………………………………
Name the linkage …………………………………..
Name the molecule removed ……………………….
Give the type of condensation …………………………………
Name the polymer ……………………………….
Use of polyester –
Alkanes
Reactions of alkanes
chlorination of methane
Give the Condition for the reaction: ………………………
--------------------------------------------------------------------------------
…………………………………………………………………………………………………………………………….
------------------------------------------------------------------------------
……………………………………………………………………………………………………………………………….
Give the equation for the burning of methane in air
----------------------------------------------------------
3. Draw the isotopes of butane and pentane
Alkenes
What are unsaturated compounds?
……………………………………………………………………………………………………………………………………….
2. Which one of the following are unsaturated compounds
Ans ……………………………..
Give the test for unsaturated compounds
--------------------------------------------------------------------------------------
Which one of the following can decolorize the bromine water?
………………………………………………………………………………………………………………………………………….
4.Draw the first 3 alkenes
What is cracking? ( imp)
-------------------------------------------------------------------------------------4. What are the conditions for cracking?
------------------------------------------------------------------------------
5. Give the complete equation for the following
C H ------------------ +
C H --------------------- +
C H ----------------------- +
COMPLETE COMBUTION OF HYDROCARBONS
Hydrocarbon + oxygen ----------------- +
Petrol + oxygen __________ +
Methane + oxygen __________ +
INCOMPLETE COMBUTION OF HYDROCARBONS (imp)
Hydrocarbon + oxygen ----------------- +
Petrol + oxygen __________ +
Methane + oxygen __________ +
6. Explain the health problem associated with the incomplete combustion of hydrocarbon
------------------------------------------------------------------------------
7. Give the environmental problem associated with burning of hydrocarbon
---------------------------------------------------------
Ethanol
1. What is the functional group in alcohol?
Draw the displayed formula of ethanol showing the entire bonds
2. Explain the two methods of preparation of ethanol
WHAT IS THE DIFFERENCE BETWEEN THE TWO METHOD
Hydration
fermentation
Which method is prefers in Middle East and in a cold country like Spain
Middle East ………………………………………………….
Reason………………………………………………………………………………………………………………………………
Spain ……………………………………………………………….
Reason………………………………………………………………………………………………………………………………
COMPOUND
FUNCTIONAL GROUP
ALCOHOL
ACID
ESTER
REACTIONS OF ALCOHOL
Natural oil and gas
Crude oil –
Explain FRACTIONAL DISTILATION OF CRUDE OIL
Uses of different fractions
Petrol -
Naphtha-
Kerosene-
Diesel -
Bitumen -
Boiling point and no of carbon atoms in a mixture of hydrocarbon
1. Boiling point and hydrocarbon are given below
Hydrocarbon
Boiling point
No of carbon atoms
gas
-40-40 c
C1-C4
petrol
40-100 c
C4-C8
Naphtha
100-160 c
C6-C10
kerosene
250-350c
C10-C16
Diesel oil
350-450c
C16-C20
What is the trend in the boiling point in the series? Relate the trend with the number of carbon atoms in the chain of each compound. GIVE THE REASON
………………………………………………………………………………………….
…………………………………………………………………………………
Synthetic polymers
1.What are Monomer------------------------------------------
-----------------------------------------------
2.Polymers –
…………………………………………………………………………………………..
3.Give the two types polymers – …………………………………………………………………..
4.Name the monomer of polyethene
5.Draw the repeating unit of polyethene
6. Draw the equation for the formation of polythene
7. Name the monomer of polypropene
………………………………………………………
8.Draw the repeating unit of poly propene
9.Draw the equation for the formation of polypropene
10.Name the monomer of polychloroethene
………………………………………………………………
11.Draw the repeating unit of polychloroethene
12.Draw the equation for the formation of polychloroethene
13Use of addition polymers
polymer
properties
Uses
Poly ethene
Polymer
Poly propene
Properties
Uses
Polymer
Properties
Uses
Poly chloro ethene
14.what are condensation polymers .give examples
15.Give the monomers of nylon
Carboxylic acid =
acid chloride =
Amines =
16. Draw the structure of nylon
Name the monomers…………………………………
Name the linkage …………………………………..
Name the molecule removed ……………………….
Give the type of condensation …………………………………
Name the polymer ……………………………….
2. Draw the structure of nylon
Name the monomers…………………………………
Name the linkage …………………………………..
Name the molecule removed ……………………….
Give the type of condensation …………………………………
Use of nylon –…………………………………………
Terelene (polyester )
17.Give the monomers of nylon
Carboxylic acid =
Diol =
18. Draw the structure of terelene
Name the monomers…………………………………
Name the linkage …………………………………..
Name the molecule removed ……………………….
Give the type of condensation …………………………………
Name the polymer ……………………………….
Use of polyester –
Fill in the blanks
20)HALOGEN HALOGEN IONS PHYSICL STATE COLOR
FLURINE F ……………… ……………….
CLORINE Cl …………………. …………………
BROMINE Br ………………….. …………………
IODINE I ………………….. ……………….
Fill in the blanks
ELEMENT ELECTON ARRANGEMENT
FLURINE ………………
CLORINE ………………..
BROMINE 2, 8,18,7
IODIDNE 2,8,18,18,7
21) Name the USES OF FLURINE
…………………………………………………………
22)Complete the following
SODIUM+ CLORINE ____________________ …………………………….
2Na + Cl _________________________
2 ………………………………..
23)Explain the test for chlorine gas?
………………………………………
24) Explain the how the chlorine dissolve in water? Write the equation
…………………………………………………………………………………………
…………………………………………………………………………………………
……………………………………..
20)HALOGEN HALOGEN IONS PHYSICL STATE COLOR
FLURINE F ……………… ……………….
CLORINE Cl …………………. …………………
BROMINE Br ………………….. …………………
IODINE I ………………….. ……………….
Fill in the blanks
ELEMENT ELECTON ARRANGEMENT
FLURINE ………………
CLORINE ………………..
BROMINE 2, 8,18,7
IODIDNE 2,8,18,18,7
21) Name the USES OF FLURINE
…………………………………………………………
22)Complete the following
SODIUM+ CLORINE ____________________ …………………………….
2Na + Cl _________________________
2 ………………………………..
23)Explain the test for chlorine gas?
………………………………………
24) Explain the how the chlorine dissolve in water? Write the equation
…………………………………………………………………………………………
…………………………………………………………………………………………
……………………………………..
Chemicals needed for A levels
ammonium hydroxide
ammonium chloride
iron ammonium sulphate ( Mohr’s salt)
aluminum powder
barium nitrate
copper nitrate
copper chloride
chromium chloride
cobalt nitrate
lead nitrate
magnesium chloride
magnesium sulphate
magnesium carbonate
magnesium bicarbonate
iron (III) chloride
magnesium ribbon
hydrogen peroxide
ferrous sulphate
phenolphthalein
zinc powder
potassium iodide
potassium chloride
potassium bromide
potassium dichromate
potassium bi carbonate
nickel chloride
sodium bi carbonate
hydrated sodium carbonate
universal indicator
sodium thiosulphate
sodium hydrogen sulphate
zinc sulphate
zinc chloride
oxalic acid
methyl orange
benedict solution
sodium nitrate
Apparatus
Electronic balance
reagent bottles -
ammonium hydroxide
ammonium chloride
iron ammonium sulphate ( Mohr’s salt)
aluminum powder
barium nitrate
copper nitrate
copper chloride
chromium chloride
cobalt nitrate
lead nitrate
magnesium chloride
magnesium sulphate
magnesium carbonate
magnesium bicarbonate
iron (III) chloride
magnesium ribbon
hydrogen peroxide
ferrous sulphate
phenolphthalein
zinc powder
potassium iodide
potassium chloride
potassium bromide
potassium dichromate
potassium bi carbonate
nickel chloride
sodium bi carbonate
hydrated sodium carbonate
universal indicator
sodium thiosulphate
sodium hydrogen sulphate
zinc sulphate
zinc chloride
oxalic acid
methyl orange
benedict solution
sodium nitrate
Apparatus
Electronic balance
reagent bottles -
1. Draw the bonding in metals
2. Why metals are malleable
3. Why metals conduct electricity
4. Sodium chloride is having a high melting point. why?
5. Draw and explain the structure of diamond
6. Diamond is having a high melting point .why?
7. Why sodium chloride do not conduct electricity in solid state
8. Diamond is having a high sublimation point .why?
9. Why is diamond used for cutting?
10. Draw the structure of sodium chloride and magnesium chloride
11Why magnesium chloride is having a high melting point than sodium chloride
12.Molten sodium chloride conducts electricity. Why?
13.Define alloys. Why they are hard. Draw the structure of alloys
2. Why metals are malleable
3. Why metals conduct electricity
4. Sodium chloride is having a high melting point. why?
5. Draw and explain the structure of diamond
6. Diamond is having a high melting point .why?
7. Why sodium chloride do not conduct electricity in solid state
8. Diamond is having a high sublimation point .why?
9. Why is diamond used for cutting?
10. Draw the structure of sodium chloride and magnesium chloride
11Why magnesium chloride is having a high melting point than sodium chloride
12.Molten sodium chloride conducts electricity. Why?
13.Define alloys. Why they are hard. Draw the structure of alloys
Chemistry in society
1. Name the ore of iron-----------------------
2. Give the chemical name of hematite -----------------
3. Name the apparatus used for extraction of iron ----------------------------
4. Give the chemical formula of hematite---------------------------
5. Why the furnace is lined with bricks ---------------------------
6. Draw the blast furnace. Label it
7. Name the three raw materials needed for the extraction of iron…………………………………
8. Name the reducing agent in the blast furnace ……………………….
9. What is the role of carbon dioxide in the furnace? Give equation(imp)
………………………………………………………….
10. What is the role of calcium carbonate in the blast furnace?( imp)
………………………………………………………………………….
11. Give all the equations in blast furnace (imp)
………………………………………………………………………
……………………………………………………………………..
……………………………………………………………………..
………………………………………………………………………
………………………………………………………………………
………………………………………………………………………..`
`
12. Why hot air is blast from the bottom of the furnace
………………………………………………………………………………………
13) Explain the extraction of zinc by reduction
………………………………………………………………………………….
14. Name the reducing agent for the extraction of zinc
………………………………………………………………………………….
15. 1.Name the ore of zinc. Give the chemical name and chemical formula
………………………………………………………………………….
2. What is termite reaction. Give example. Give the use of thermite reaction ( imp)
…………………………………………………………………………………….
16. Explain the Purification of copper from impure copper block
At cathode …………………………………… at anode ……………………………..
Name the electrolyte used in the purification of copper …………………………….
17. Give the uses of metals
Iron –
Copper-
Aluminum-
Zinc-
Chromium
18. Give the name of the ore of aluminum ----------------------------
19. Give the chemical name of the ore of aluminum -------------------------
20. Give the chemical formula of the ore of aluminum ----------------------------
21. Name the substance used as anode and cathode in the extraction of aluminum
…………………………………………………………………………………..
22. Name the process of extraction of aluminum
……………………………………………………………………………
23. Give reaction at cathode ……………………………………
24. Give reaction at anode………………………………………….
25. Why electricity is used for the extraction of aluminum
…………………………………………………………………….
Manufacture of some important chemicals
Haber process
Name the process of manufacture of ammonia ……………………….
Name the raw material. Give the sources ……………………………………………………………………………………
give the condition for haber process
………………………………………………………………………………………
Name the catalyst ………………………………………..
how the ammonia gas is removed from the chamber
………………………………………………………………………………………..
what do we do for the un reacted hydrogen and nitrogen
…………………………………………………………………………………………..
7. Give important uses of ammonia …………………………………………………………………………………………
8. Describe the manufacture of nitric acid from ammonia
……………………………………………………………………………………..
9. Name the catalyst used for the manufacture of ammonia
…………………………………………………………………………
10. Give uses of nitric acid ……………………………………………..
11. Name the process of manufacture of sulphuric acid
………………………………………………………………………
12. Name the raw material. Give the sources ……………………………………………………………………………………
13. Give the condition for contact process
………………………………………………………………………………………
14. Name the catalyst……………………………………………..
15. Give reversible and irreversible reactions in contact process
………………………………………………………………………
16. Give all the equation in contact process
……………………………………………………………………………………………………………………………………………………………………………………..
17. Give the uses of sulphuric acid
………………………………………………………………………………………………
18. Name the main pollutant gases in acid rain
…………………………………………………………………………………
19. Give two environmental problems of acid rain
………………………………………………………………………………………………
20. Explain the extraction of sodium hydroxide for sea water( draw the diaphragm cell)
Name the gases at anode and cathode …………………………………………………….
Name the substance remaining in the solution……………………………..
Give the use of chlorine …………………………………………………..
Sodium hydroxide ………………………………………………..
1. Name the ore of iron-----------------------
2. Give the chemical name of hematite -----------------
3. Name the apparatus used for extraction of iron ----------------------------
4. Give the chemical formula of hematite---------------------------
5. Why the furnace is lined with bricks ---------------------------
6. Draw the blast furnace. Label it
7. Name the three raw materials needed for the extraction of iron…………………………………
8. Name the reducing agent in the blast furnace ……………………….
9. What is the role of carbon dioxide in the furnace? Give equation(imp)
………………………………………………………….
10. What is the role of calcium carbonate in the blast furnace?( imp)
………………………………………………………………………….
11. Give all the equations in blast furnace (imp)
………………………………………………………………………
……………………………………………………………………..
……………………………………………………………………..
………………………………………………………………………
………………………………………………………………………
………………………………………………………………………..`
`
12. Why hot air is blast from the bottom of the furnace
………………………………………………………………………………………
13) Explain the extraction of zinc by reduction
………………………………………………………………………………….
14. Name the reducing agent for the extraction of zinc
………………………………………………………………………………….
15. 1.Name the ore of zinc. Give the chemical name and chemical formula
………………………………………………………………………….
2. What is termite reaction. Give example. Give the use of thermite reaction ( imp)
…………………………………………………………………………………….
16. Explain the Purification of copper from impure copper block
At cathode …………………………………… at anode ……………………………..
Name the electrolyte used in the purification of copper …………………………….
17. Give the uses of metals
Iron –
Copper-
Aluminum-
Zinc-
Chromium
18. Give the name of the ore of aluminum ----------------------------
19. Give the chemical name of the ore of aluminum -------------------------
20. Give the chemical formula of the ore of aluminum ----------------------------
21. Name the substance used as anode and cathode in the extraction of aluminum
…………………………………………………………………………………..
22. Name the process of extraction of aluminum
……………………………………………………………………………
23. Give reaction at cathode ……………………………………
24. Give reaction at anode………………………………………….
25. Why electricity is used for the extraction of aluminum
…………………………………………………………………….
Manufacture of some important chemicals
Haber process
Name the process of manufacture of ammonia ……………………….
Name the raw material. Give the sources ……………………………………………………………………………………
give the condition for haber process
………………………………………………………………………………………
Name the catalyst ………………………………………..
how the ammonia gas is removed from the chamber
………………………………………………………………………………………..
what do we do for the un reacted hydrogen and nitrogen
…………………………………………………………………………………………..
7. Give important uses of ammonia …………………………………………………………………………………………
8. Describe the manufacture of nitric acid from ammonia
……………………………………………………………………………………..
9. Name the catalyst used for the manufacture of ammonia
…………………………………………………………………………
10. Give uses of nitric acid ……………………………………………..
11. Name the process of manufacture of sulphuric acid
………………………………………………………………………
12. Name the raw material. Give the sources ……………………………………………………………………………………
13. Give the condition for contact process
………………………………………………………………………………………
14. Name the catalyst……………………………………………..
15. Give reversible and irreversible reactions in contact process
………………………………………………………………………
16. Give all the equation in contact process
……………………………………………………………………………………………………………………………………………………………………………………..
17. Give the uses of sulphuric acid
………………………………………………………………………………………………
18. Name the main pollutant gases in acid rain
…………………………………………………………………………………
19. Give two environmental problems of acid rain
………………………………………………………………………………………………
20. Explain the extraction of sodium hydroxide for sea water( draw the diaphragm cell)
Name the gases at anode and cathode …………………………………………………….
Name the substance remaining in the solution……………………………..
Give the use of chlorine …………………………………………………..
Sodium hydroxide ………………………………………………..
structure
Chemistry: Structure.
Metallic bonding.
Metallic bonding is the array of positive ions surrounded by sea of free mobile electrons.
Metals are strong because of the powerful attraction between the positive centres and the free electrons.
Metals can conduct electricity because the free electrons can move through out the structure carrying heat energy.
Metals are malleable and ductile because the layers of atoms can slide over each other when force is applied.
An alloy is a mixture of metals
Example of alloy: brass [mixture of copper & zinc]
Alloys are hard because in alloys, the different metals have slightly different size. This breaks up the regular arrangement & makes it more difficult for the layers to slide.
Structure of Diamond
Diamond & graphite are having a giant co-valent structure.
In diamond, each carbon atom is strongly co-valently bonded with four other carbon atoms leading to a three dimentional network.
Diamond is hard due to the strong carbon-carbon co-valent bonds.
Diamond does not conduct electricity because all the electrons in the outer level of the carbon atoms are tightly held in co-valent bonds between the atoms. So no free electrons to move around and carry electricity.
Diamond does not dissolve in water or any other solvents because of the powerful co-valent bonds between the atoms.
Diamond is used in cutting concrete and glass because it is hard.
Diamond is used for making jewellery because it is shiny in nature.
Diamond is having a high sublimation point because of the strong co-valent bonds between the carbon atoms.
Structure of graphite
In graphite, each carbon atom is strongly co-valently bonded to three other carbon atoms leading to a hexagonal ring. Graphite has a layer structure and the layers are held by weak vanderwall’s force of attraction.
Graphite can conduct electricity because each carbon atom is strongly co-valently bonded to three other carbon atoms leaving an electron free. This free electron can carry electricity through out the structure.
Graphite is soft because the layers can slide over each other with the help of weak vanderwall’s force of attraction.
Graphite is not soluble in any solvent because of the strong co-valent bonding between the carbon atoms in the hexagonal ring.
Graphite is having a high sublimation point because of the strong co-valent bond between the carbon atoms.
Allotropy: some elements occur in more than one physical form. Eg: carbon (diamond & graphite).
Structure of sodium chloride.
Sodium chloride is having a giant ionic structure.
In solid sodium chloride, each sodium ion [Na+] is surrounded by 6 other chloride ion [Cl-] with strong electrostatic force of attraction.
Sodium chloride is having high melting point due to the strong electrostatic force of attraction between the ions.
Sodium chloride does not conduct electricity because the ions are held by strong electrostatic force of attraction. They are not free to move.
Sodium chloride conduct electricity in liquid state because the ions are free to move and can carry electricity.
Simple molecular structure
The molecules exist in simple molecules and weak force of attraction held them together. So they may be solid, liquid, or gas.
Simple molecules have low melting & boiling point due to the weak intermolecular force of attraction.
Ice, solid iodine, & solid carbondioxide are examples of simple molecular crystals. They have low melting point due to the weak intermolecular force.
Carbondioxide shape: linear.
Methane shape: tetrahydral.
Water shape: non-linear.
Ammonia shape: pyramidal.
Metallic bonding.
Metallic bonding is the array of positive ions surrounded by sea of free mobile electrons.
Metals are strong because of the powerful attraction between the positive centres and the free electrons.
Metals can conduct electricity because the free electrons can move through out the structure carrying heat energy.
Metals are malleable and ductile because the layers of atoms can slide over each other when force is applied.
An alloy is a mixture of metals
Example of alloy: brass [mixture of copper & zinc]
Alloys are hard because in alloys, the different metals have slightly different size. This breaks up the regular arrangement & makes it more difficult for the layers to slide.
Structure of Diamond
Diamond & graphite are having a giant co-valent structure.
In diamond, each carbon atom is strongly co-valently bonded with four other carbon atoms leading to a three dimentional network.
Diamond is hard due to the strong carbon-carbon co-valent bonds.
Diamond does not conduct electricity because all the electrons in the outer level of the carbon atoms are tightly held in co-valent bonds between the atoms. So no free electrons to move around and carry electricity.
Diamond does not dissolve in water or any other solvents because of the powerful co-valent bonds between the atoms.
Diamond is used in cutting concrete and glass because it is hard.
Diamond is used for making jewellery because it is shiny in nature.
Diamond is having a high sublimation point because of the strong co-valent bonds between the carbon atoms.
Structure of graphite
In graphite, each carbon atom is strongly co-valently bonded to three other carbon atoms leading to a hexagonal ring. Graphite has a layer structure and the layers are held by weak vanderwall’s force of attraction.
Graphite can conduct electricity because each carbon atom is strongly co-valently bonded to three other carbon atoms leaving an electron free. This free electron can carry electricity through out the structure.
Graphite is soft because the layers can slide over each other with the help of weak vanderwall’s force of attraction.
Graphite is not soluble in any solvent because of the strong co-valent bonding between the carbon atoms in the hexagonal ring.
Graphite is having a high sublimation point because of the strong co-valent bond between the carbon atoms.
Allotropy: some elements occur in more than one physical form. Eg: carbon (diamond & graphite).
Structure of sodium chloride.
Sodium chloride is having a giant ionic structure.
In solid sodium chloride, each sodium ion [Na+] is surrounded by 6 other chloride ion [Cl-] with strong electrostatic force of attraction.
Sodium chloride is having high melting point due to the strong electrostatic force of attraction between the ions.
Sodium chloride does not conduct electricity because the ions are held by strong electrostatic force of attraction. They are not free to move.
Sodium chloride conduct electricity in liquid state because the ions are free to move and can carry electricity.
Simple molecular structure
The molecules exist in simple molecules and weak force of attraction held them together. So they may be solid, liquid, or gas.
Simple molecules have low melting & boiling point due to the weak intermolecular force of attraction.
Ice, solid iodine, & solid carbondioxide are examples of simple molecular crystals. They have low melting point due to the weak intermolecular force.
Carbondioxide shape: linear.
Methane shape: tetrahydral.
Water shape: non-linear.
Ammonia shape: pyramidal.
Thursday, November 20, 2008
PERIODIC TABLE
The elements in the periodic table are arranged according ti the increasing atomic number. In the peridoic table there are eight main groups and seven periods. The elements in the same groups have similar properties because they have the same number of electrons in their outer shell. The group number of the elements is the same as the number of the outer electrons. 3/4 of the periodic table is filled with metals. There are other elements called the semi metals whos hare both the properties of metals and non metals.They conduct like metals and are brittle like non-metals.
GROUP 1
They are called alkali metals because they react with water to form strong alkali. The increase in number of shells and atomic size causes increase ub the reactivity down the group because bigger the atom, the less its attractive force towards the nucleus. Group 1 metals have one electron in the outermost shell which is why they are called group 1. They are less dense than group 2 metals because they have only one electron in the outermost shell and they're stored under oil to prevent them from reacting iwth oxygen and water vapour form at the atnoshpere as it is dangerous.
Reaction with water
Sodium is a strong alkali, when it reacts with water :
1) It floats and melts.
2) Hydrogen gas is produced.
3) It forms sodium hydroxide.
Sodium + water ---------------> Sodium hydroxide + hydrogen
Na + H2O ---------------------> NaOH + H2
Na + HOH -------------> NaOH + H2
Potassium when reacting with water :
1) It floats.
2) It catches fire and burns with a lilac flame.
3) It forms potassium hydroxide and hydrogen.
Potassium + water --------------------> Potassium hydroxide + hydrogen
K + H2O --------------------------------> KOH + H2
K + HOH -------------------------------> KOH + H2
Lithium
Lithium forms Lithium hydroxide and hydrogen gas when reacting with water.
Li + H2O ----------------> LiOH + H2
Rubedium (Rb)
Rb + H2O -----------> Rb (OH) + H2
When rubedium reacts with water :
1) Heat is produced.
2) Explosion takes place.
3) It forms Rubedium hydroxide and hydrogen gas.
The elements in the periodic table are arranged according ti the increasing atomic number. In the peridoic table there are eight main groups and seven periods. The elements in the same groups have similar properties because they have the same number of electrons in their outer shell. The group number of the elements is the same as the number of the outer electrons. 3/4 of the periodic table is filled with metals. There are other elements called the semi metals whos hare both the properties of metals and non metals.They conduct like metals and are brittle like non-metals.
GROUP 1
They are called alkali metals because they react with water to form strong alkali. The increase in number of shells and atomic size causes increase ub the reactivity down the group because bigger the atom, the less its attractive force towards the nucleus. Group 1 metals have one electron in the outermost shell which is why they are called group 1. They are less dense than group 2 metals because they have only one electron in the outermost shell and they're stored under oil to prevent them from reacting iwth oxygen and water vapour form at the atnoshpere as it is dangerous.
Reaction with water
Sodium is a strong alkali, when it reacts with water :
1) It floats and melts.
2) Hydrogen gas is produced.
3) It forms sodium hydroxide.
Sodium + water ---------------> Sodium hydroxide + hydrogen
Na + H2O ---------------------> NaOH + H2
Na + HOH -------------> NaOH + H2
Potassium when reacting with water :
1) It floats.
2) It catches fire and burns with a lilac flame.
3) It forms potassium hydroxide and hydrogen.
Potassium + water --------------------> Potassium hydroxide + hydrogen
K + H2O --------------------------------> KOH + H2
K + HOH -------------------------------> KOH + H2
Lithium
Lithium forms Lithium hydroxide and hydrogen gas when reacting with water.
Li + H2O ----------------> LiOH + H2
Rubedium (Rb)
Rb + H2O -----------> Rb (OH) + H2
When rubedium reacts with water :
1) Heat is produced.
2) Explosion takes place.
3) It forms Rubedium hydroxide and hydrogen gas.
Group 2
* Group 2 elements are known as alkaline earth metals.
* They can form strong alkali and they occur widely on earth crust.
* They are metals.
* They have melting points and densities that are quite low for metals.
* They react with air, water or steam to form oxides and hydroxides.
* They show the same reactivity trend as group 1, increasingly reactive as you go down the group.
* They form compounds in which the metal has a +2 ion.
* They form white or colorless compounds which gives colorless solutions.
* The alkaline earth metals are reactive, but less reactive than the alkali metals.
* Group 2 elements are known as alkaline earth metals.
* They can form strong alkali and they occur widely on earth crust.
* They are metals.
* They have melting points and densities that are quite low for metals.
* They react with air, water or steam to form oxides and hydroxides.
* They show the same reactivity trend as group 1, increasingly reactive as you go down the group.
* They form compounds in which the metal has a +2 ion.
* They form white or colorless compounds which gives colorless solutions.
* The alkaline earth metals are reactive, but less reactive than the alkali metals.
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