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Chemistry 9th Class
FILL IN THE BLANKS
Complete the following blanks with appropriate answers:
1.
3-5 litres =_________ millilitres.
2.
Bases are the donors of a pair of _________.
3.
The chemical formula of hematite is _________.
4.
The phenomenon which keeps surface of the earth warm is known as _________effect.
5.
Ozone is an allotrope of _________.
6.
K = C +_________.
7.
The chemical formula of ureas is _________.
8.
Acids are _________donors.
9.
All halogens have _________ electrons in their outermost shell.
10.
Water gas is a mixture of hydrogen and _________.
11.
The process of separating insoluble particles from liquids is called _________.
12.
The chemical formula of the phosgene gas is _________.
13.
The property which determines the direction of flow of heat from one body to another is called
_________.
14.
The iron containing about 5% unwanted elements is called _________.
15.
When water is added, the presence of _________retards the quick setting of cement.
16.
The chemical formula of octane is _________.
17.
The acids are the donors of _________.
18.
Hydrogen burns with a green flame in _________gas.
19.
The first organic compound prepared in the laboratory is _________.
20.
The vertical columns of the elements in the Periodic table are called _________.
21.
Formula mass of NaOH is _________.
22.
Mole is the unit of _________.
23.
The hardest form of carbon is _________.
24.
C6H12O6 is the formula of _________.
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25.
26.
In a dry cell, _________ act as the anode.
The early Greeks believed that every thing in the universe was made up of three things namely air, earth
_________ and water.
27.
Valency is a number giving the _________ power of an atom with another atom.
28.
Number of atoms in one mole atoms is called _________ ‘s number.
29.
Reactions must undergo a _________ change in order to form new products.
30.
In a _________ type of reaction there is only one reactant which must be a compound.
31.
_________ + Chlorine _________ potassium chloride + Bromine.
32.
The reacting materials and surroundings become hot during _________ reactions.
33.
The latent heat of _________ of water is approximately 6kJ per _________.
34.
When water turns into ice, the average distance between water _________ increases.
35.
A homogenous mixture of two or more than two substances is called a _________.
36.
The solubility of a solute in water at particular temperature is the maximum amount of solute that will
_________ in _________ g of water at that temperature.
37.
We can protect ourselves from cholera by _________ water before we drink it.
38.
The oxide and hydroxide of potassium metal are both _________ because they both neutralize.
39.
Since ammonium hydroxide is a weak base, its aqueous solution has a _________ concentration of
_________ ions that of sodium hydroxide.
40.
The indicator used to measure the relative strengths of acids and bases is called _________.
41.
In neutralization reaction, OH ions react with _________ ions to give _________.
42.
In a I M solution of NaCl, there are _________ grams of NaCl in each _________ of the solution.
43.
_________ is often used as an anti acid to treat excess acidity in the stomach.
44.
Number of elements in the first period is _________.
45.
Number of elements in the third period is _________.
46.
Number of elements in the fifth period is _________.
47.
Number of elements in the sixth period is _________.
48.
The total number of protons and _________ in an atom is called _________ number of the atom.
49.
7
50.
The _________metals have one electron in their _________ shell.
51.
3Li
contains three _________ and _________ neutrons.
The halogens have _________ electrons in their last shell and are found in group _________ of the
periodic table.
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52.
The reactivity of a group of metals gradually increase from the _________ to the _________ of the
group.
53.
Chlorine is _________ electronegative than bromine and iodine but _________ electronegative than
fluorine.
54.
During bonding, hydrogen atom can attain the electronic configuration of _________ atom.
55.
A potassium atom tends to lose electrons so as to leave _________ electrons in its outermost shell.
56.
When sodium reacts with sulphur an _________ bond is formed.
57.
Carbon usually forms bonds by sharing _________ pairs of electrons.
58.
The freezing point of H2O is much higher than that of H2S because of stronger _________ in water.
59.
The nitrogen atom in a molecule of ammonia gas has one _________ pair of electrons available for the
formation of a _________ covalent bond.
60.
The alkali metals, Group I A have electrons in their outermost shells and a valency of _________.
61.
Aluminium is a member of Group _________ of the periodic table.
62.
Naturally occurring hydrogen is a mixture of three isotopes, _________, _________ and _________.
63.
Sodium metal _________, occurs free in nature because of its extreme _________.
64.
Gypsum is one of the important, naturally occurring compounds of _________ metal.
65.
During the extraction of aluminium, bauxite is purified by dissolving it in _________; the soluble
impurities are removed by _________.
66.
Ores consist of a mixture of _________ which are naturally occurring associated with useless rocky
material.
67.
Haematite contains about 65% of _________. This is extracted in a blast furnace where haematite is
reduced by carbon _________ gas.
68.
Iron reacts with steam to form solid _________ and the gas _________.
69.
Zinc with an electronic configuration of 2, 8, 18 has an atomic number and a valency of _________.
70.
At one stage in the industrial extraction of zinc, ZnO is reduced by heating with _________ to give liquid
zinc and _________ gas.
71.
Lead is extracted from galena, its _________ ore, by roasting in _________ and then reducing the
roasted ore.
72.
An atom of carbon has _________ electrons in its valence shell and normally forms four _________
bonds.
73.
When a Coca-Cola is opened, bubbles of _________ form in the liquid due to the release of pressure.
74.
Green coloured glass is prepared by mixing a small quantity of _________ with sodium and calcium
silicates.
75.
The electronegativity of nitrogen must be _________ than that of oxygen because nitrogen comes earlier
in the period.
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76.
The yellow colour of commercial HNO3 is due to the presence of _________ gas dissolved in it.
77.
When one mole of N2 gas is mixed with _________ mole of hydrogen gas, 2 mole of NH3 gas is produced.
78.
NH4NO3 is one of the salts used as a fertilizer for crops and also in the making of certain _________.
79.
Among man made compounds _________ are thought to be mainly responsible for depletion of the ozone
in the _________.
80.
Oxygen from the air is used by all living things in the process called _________. Oxygen returned to the
air by plants in a process called _________.
81.
Removal of electrons from an atom of ion is termed _________ while addition of electrons is called
_________.
82.
Sulphuric acid can remove _________ from an organic dye making it colourless.
83.
In acid rain, oxides of _________ and nitrogen dissolve in rainwater to form their respective _________.
84.
_________ can replace all other halogens from solutions of their salts.
85.
When a compound burns easily and leaves no residue it is most likely to be an _________ compound.
86.
Any non-cyclic hydrocarbon whose name ends with ane must have a general formula _________.
87.
In a molecule of heptene there are _________ hydrogen atoms.
88.
Each H-C-H bond angle in methane is _________ degrees.
89.
The H-C-C bond angle in ethyne is _________ degrees.
90.
A mixture of kerosene, petrol and diesel oil can be separated by _________.
91.
The arrangement of carbon atoms in organic compounds may be described as _________ chain
_________ chain or _________.
MULTIPLE CHOICE QUESTIONS
Choose the correct answers from the following:
1.
The formula KAl(SO4)2 represents a total number of _________atoms.
(6, 7, 11, 12, 14)
2.
If an element ‘X’ forms an oxide with the formula ‘XO’ which of the following formula is correct.
(XCl, XS, XH3, X2S3, XF4)
3.
Which of the following compound is an alcohol?
(CH3-CH2-OH, CH3-O-CH3, CH3-COOH,
CH3-CH2-CHO, CH3-CH2-CH3)
4.
There are _________elements in the first period of the Periodic Table.
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(2, 8, 18, 32, 50)
5.
Which of the following formulae represents the alkyl group?
(C5H13, C5H12, C5H11, C5H10, C5H9)
6.
The S.I unit of length is _________.
(Millimetre, Centimetre, Metre, Kilometre)
7.
_________ is the driest and the hardest coal.
(Anthracite, Peat, Lignite, Bitumin)
8.
_________ is the second most abundant element in the earth’s crust.
(Oxygen, Carbon, Nitrogen, Silicon)
9.
The general formula of alkanes is _________.
(CnH2n-2, CnH2n, CnH2n+2, CnH2n+4)
10.
_________ is a noble gas.
(Hydrogen, Helium, Nitrogen, Oxygen)
11.
In a dry cell, the depolarizer is _________.
(NH4Cl, MnO2, ZnCl2)
12.
Only _________ reacts with copper at room temperature.
(Hydrochloric Acid, Sulphuric Acid, Nitric Acid)
13.
The chemical formula of fluorspar is _________.
(CaF2, Na2AlF6, NaF)
14.
_________ is a neutral oxide.
(ZnO, NO, CaO)
15.
The atmospheric gas which is essential for the manufacture of food of plants is _________.
(Oxygen, Nitrogen, Carbon dioxide)
16.
The molecular formula mass of ordinary water is _________ a.m.u
(16, 18, 20, 32)
17.
Cations are formed by _________.
(Sharing of electrons, losing of electrons, gaining of electrons)
18.
The printer’s ink contains _________.
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(Lamp Black, Bone Black, graphite)
19.
The chemical symbol of tin is _________.
(Ti, Sn, Sb)
20.
Aqua Regia is a mixture of hydrochloric acid and _________.
(Sulphuric Acid, Water, Nitric Acid)
21.
K2L6 is the electronic arrangement of _________.
(Neon, Nitrogen, Oxygen)
22.
Methane is generally known as _________.
(Coal gas, Marsh gas, Water gas)
23.
_________Generally takes place at the anode.
(Reduction, Solvation, Oxidation)
24.
The chemical formula of Haematite is _________.
(Fe2O3, Fe2O3.3H2O, Fe3O4)
25.
The pH value of human blood is _________.
(6.5, 7.3, 7.9)
26.
A chemist is studying the properties of a substance taken from the leaf of a tree in which branch of the
subject is the most likely to be working?
(Industrial chemistry, Physical Chemistry,
Environmental Chemistry, Organic Chemistry)
27.
The chemistry of soil would most probably be studied by _________.
(An organic chemist, an inorganic chemist,
A physical chemist, A bio-chemist)
28.
A chemical reaction occurs when _________.
(aluminium conducts electricity, water is frozen to ice, iron rusts, a solution of common salt is heated)
29.
A zinc plate is placed in a solution of copper sulphate. Select from the list all the changes that take place.
(copper is deposited on the zinc plate, the colour of the solution fades, the mass of zinc decreases, zinc sulphate is
formed, bubbles of hydrogen gas form on the zinc plate)
30.
Which of the following is the best definition of exothermic reaction.
(one which occurs between a metal and oxygen, one which takes in heat, one which occurs between metals and
non-metals, one which gives out heat)
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31.
From the list, select all the statements, which are properties of a good fuel?
(it is difficult to ignite, it keeps burning once lit, it produces large amounts of smoke, it gives out much heat, it
leaves little or no ash)
32.
During the electrolysis of water, one molecule of oxygen gas is formed at the anode when hydroxide ions
given up _________ electron.
(1, 2, 3, 4, 5)
33.
Equal amounts of each of the following salts are added to water. Which salt solution will be strongest
electrolyte?
(Potassium Carbonate K2CO3, Calsium Carbonate CaCO3, Nickel Carbonate NiCO3, Silver Carbonate Ag2CO3,
Magnesium Carbonate MgCO3)
34.
_________ is the strongest base.
(NH4OH, NaHCO3, Ca(OH)2, NaOH, K2CO3)
35.
10 ml of 3 M HCl was titrated with a standard solution of NaOH containing 80 grams per litre. The volume
of the standard solution required to neutralize the acid would be _________ ml.
(5, 10, 15, 20, 25)
36.
The pH of rainwater is about 6 because air contains _________.
(Nitrogen, Oxygen, carbon dioxide, Argon, water vapours)
37.
Which one of the following is the best approximation of the number of times one proton is heavier than
one electron?
(1, 18, 180, 1800)
38.
Less energy is required to remove one electron from an atom of strontium than to remove one electron
from an atom of _________.
(Barium, Rubidium, Calsium, Radium)
39.
An ionic bond will most likely form between element from Group _________.
(II and III, II and VI, III and IV, IV and V, V and VI)
40.
_________ contains chemical bonds non-polar in nature.
(Ammonia Gas, Sulphur dioxide gas, hydrogen sulphide gas, water in gaseous form, chlorine gas)
41.
In HCl gas, the bonds are _________.
(ionic, covalent (non-polar), covalent (polar), Coordinate covalent, hydrogen)
42.
Copper sulphate is written as CuSO4.5H2O. The number of water molecules that form coordinate covalent
bonds with the Cu+2 ion in each molecule is _________.
(0, 1, 2, 3, 4, 5)
43.
A hydride ion (H-) and a helium atom have the same _________.
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(number of protons, number of electrons, number of neutrons, valency, all of the above)
44.
When sodium is placed in a beaker of water then _________.
(Hydrogen is produced, the sodium disappears after sometime, the water becomes acidic, the water becomes
warmer)
45.
_________ has the smallest ionic radius.
(Radium, Barium, Strontium, Calsium, Magnesium)
46.
The cost of _________ will not contribute to the cost of aluminium metal.
(electricity, sulphuric acid, sodium hydroxide, bauxite, graphite)
47.
_________ is sometimes used for the reduction of Cr2O3 to get Cr metal.
(C, Al, H2, Fe, S)
48.
In the steel used to reinforce concrete in buildings, houses _________ is most likely to be found.
(carbon, manganese, chromium, silicon, nickel)
49.
_________ has the highest number of atoms in it.
(C2O4(NH4)2, (NH4)2SO4, CH3CO2NH2, NH4NO3, (NH4)2CO3)
50.
_________ fertilizer contain the highest proportion of nitrogen.
(Urea, Ammonium Nitrate, Diammonium Hydrogen Phosphate, Ammonium Sulphate)
51.
When a chlorine atom combines with a hydrogen atom then _________ bond is formed.
(ionic, polar covalent, coordinate covalent, non-polar covalent)
52.
_________ is the branch of chemistry which studies hydrocarbons.
(Inorganic chemistry, physical chemistry, organic chemistry, industrial chemistry, analytical chemistry)
53.
The number of carbon atoms in one molecule of octane is _________.
(4, 5, 6, 7, 8)
54.
An alkane with six carbon atoms have _________ isomers.
(3, 5, 6, 7, 9)
55.
An alkyl group R is attached to –COOH, the functional group of the compound is _________.
(Carboxylic acid, aldehyde, ketone, alcohol, halo)
56.
The organic compound with formula C4H10 is _________.
(alkane, alkene, alkyne)
57.
The organic compound with formula C6H10 is _________.
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(alkane, alkene, alkyne)
58.
Sui gas and kerosene oil both have the general formula _________.
(CnH2n+2, CnH2n+1, CnH2n-2, CnH2n-1)
59.
_________ is an alkyl group.
(C6H15, C6H14, C6H13, C6H12, C6H10)
60.
Symbol for Antimony is _________.
(Ag, Sn, Sb, Pb)
61.
Valency of Barium is _________.
(1, 2, 3, None)
62.
Formula for Aluminium Hydroxide is _________.
(AlOH, AlOH3,Al(OH)3)
63.
Molecular mass of NaOH is _________.
(80, 40, 60, 28)
64.
_________ is a liquid at ordinary temperature.
(Oxygen, Mercury, Sodium, Neon).
65.
_________ is a solid at ordinary temperature
(CO, Cl2, Br2, I2)
66.
Valency of X in Al2X3 is _________.
(2, 3, 4, 1)
67.
Percentage by mass of oxygen in Earth’s crust is _________.
(26, 50, 78, 7)
68.
The Hydroxide radical is _________.
(OH, OH-, O2-)
69.
Present standard for determining relative atomic mass
(Hydrogen, chlorine, carbon
70.
12)
I calorie is equal to _________ joules.
(4.0, 2.2, 0.5, 4.18)
71.
Atomic mass unit is _________.
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(6.02 x 1023, 1.66033x10-27Kg, 1.66 x 10-27Kg)
72.
Electrons were discovered during _________.
(Rutherford Experiment, Cathode Ray Experiment, Radioactivity)
73.
Lightest of all the fundamental particles is
(Electron, Proton, Neutron).
74.
Rutherford predicted the existence of _________.
(Neutron, Nucleus, Electron)
75.
Number of protons in an atom is called _________ .
(Mass number, Atomic number, Atomic mass)
76.
Isotopes have different number of _________.
(Protons, Neutrons, electrons)
77.
The sum of the number of protons and neutrons is called _________.
(Mass number, Atomic mass, Atomic number)
78.
The maximum number of electrons in M-shell is _________.
(8, 18, 32)
79.
An example of ionic compound is _________ .
(CH4, NaCl, CCl4)
80.
Ionic compounds are generally _________.
(Solids, Liquids, Gases)
81.
The relative tendency of attracting the shared electrons is called _________.
(Electronegativity, Electrovalency, Covalency)
82.
The bond formed by sharing of electrons is _________.
(Ionic, Covalent, Coordinate)
83.
Electronegativity of fluorine is _________.
(2.5, 3.0, 3.5, 4.0)
84.
In case of NaCl in water, the solvent-solute interaction are _________.
(Ion-dipole, dipole-dipole, vanderwaals)
85.
Millimolar solution is _________
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(0.1 M, 0.01M, 0.001M).
86.
_________ always takes place at anode.
(Reduction, Oxidation, Neutralization)
87.
CH3COOH is _________.
(strong electrolyte, weak electrolyte, non electrolyte)
88.
_________ is non electrolyte.
(Sugar, HCl, NH4OH)
89.
The solution of electrolytes contain _________.
(atom, molecules, ions).
90.
_________ is non electrolyte.
(Alcohol, tap water, vinegar, baking soda)
91.
Cations are _________.
(positively charged, negatively charged, neutral).
92.
When electricity is passed through an electrolytic solution then _________ takes place.
(Migration of ions, oxidation, dissociation)
93.
The base present in the milk of magnesia is _________.
(MgSO4. 7H2O, CaSO4, Mg(OH)2)
94.
When sulphuric acid reacts with sodium hydroxide, the salt produced is:
(Na2SO4, NaHSO4, NaCl)
95.
Milk is _________.
(Acidic, Neutral, basic)
96.
pH of sea water is
(7, greater than 7, less than 7)
97.
A weak base is _________.
(KOH, NaOH, NH4OH)
98.
Acid-base reaction is called Neutralization, Hydrolysis, Hydration).
99.
In acid phenolphthalein is
(colourless, pink, yellow)
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100.
Red litmus is changed to blue by _________.
(Acid, base, salt).
101.
The most common method of purification of substance is _________.
(Crystallization, filteration, heating)
102.
The solution which contains less solute than it could hold at given temperature is called _________.
(unsaturated, supersaturated, saturated)
103.
The conversion of SO2 to SO3 is _________ reaction.
(Fast, irreversible, reversible)
104.
Solubility of solids _________ at high temperature.
(increases, decreases, doesn’t change)
105.
With the rise of temperature, solubility of gases in liquid_________.
(increases, decreases, remain same)
106.
Exothermic reaction is favoured by _________.
(High pressure, low pressure, low temperature)
107.
Rate of reaction _________ with increasing temperature.
(Increases, decreases, not affected)
108.
With the passage of time, rate of a reaction
(increases, decreases, remains constant).
109.
Hydrogen is prepared by the _________.
(action of sodium on water, electrolysis of Brine, Reduction of steam)
110.
A metal that will produce H2 with cold water is _________.
(Zn, Ca, Fe)
111.
By mass, water is __________ hydrogen.
(one-fifth, one-ninth, one-half)
112.
Union of hydrogen and carbon monoxide represents
(combustion, oxidation, hydrogenation)
113.
Hydrogen is used as _________.
(Reducing agent, oxidizing agent, bleaching agent)
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114.
Formula of heavy water is _________.
(H2O, HDO, D2O)
115.
Boiling point of heavy water is
(0C, 100C, 101.4C)
116.
_________ is used as moderator in nuclear reactors.
(Heavy water, neutrons, protons)
117.
In H2O, the ration of hydrogen to oxygen by mass is _________ .
(1:8, 1:16, 1:2)
118.
Water has maximum density at _________.
(0C, -273C, 4C)
119.
Water never exists in pure state because it is _________.
(a good solvent, non-electrolyte, conductor)
120.
Permanent hard water may be softened by the addition of _________.
(Lime water, lime, chlorine)
121.
Molecular mass of heavy water is _________.
(18, 14, 20)
122.
Density of heavy water is _________.
(1.0gm/cm3, 1.11g/cm3, 1.008gm/cm3)
123.
_________ is used in sugar refining.
(Animal charcoal, lamp black, wood)
124.
Carbon is used as _________.
( Reducing agent, oxidizing agent, bleaching agent)
125.
_________ is the poisonous gas.
(CO2, CO, HCl)
126.
The formula of phogene gas is _________.
(PH3, COCl2, COS)
127.
_________ is used in fire extinguishers.
(Co, CO2, SO2)
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128.
_________ is the gas which in the atmosphere most essential for plant growth.
(O2, N2, CO2, He)
129.
A compound containing nitrogen and a metal is called _________ .
(Nitrate, Nitride, Nitrite)
130.
Nitrogen molecule is _________.
(Monoatomic, Diatomic, Tetra atomic).
131.
The formula for sodium nitride is
(Na3N, NaN, NaN3, NaNO2)
132.
Dilute nitric acid when reacts with copper it is reduced to _________.
(NO, NO2, NH3)
133.
Percentage of nitrogen in Urea is _________.
(40.66%, 46.66%, 20%)
134.
Chemically phosphorus resembles _________.
(Carbon, Nitrogen, Oxygen)
135.
_________ is used to make smoke bombs in war time.
(White phosphorus, Red phosphorus, NH3)
136.
The allotropic form of oxygen is _________.
(nascent oxygen, ozone, oxone)
137.
Oxygen gas is prepared from _________.
(Na2O2, KClO3, H2O)
138.
MnO2 when mixed with KclO3 and heated it _________.
(gives up its oxygen, is changed chemically, acts as ctalyst produces ozone)
139.
SO3 is _________.
(acid, basic, neutral, amphoteric oxide)
140.
The neutral oxide is _________.
(H2O, NO, ZnO, CaO)
141.
_________ protects the earth surface from the ultra violet rays.
(N2, O2, O3, He)
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142.
Loss of electrons is called _________.
(Oxidation, reduction, hydrogenation)
143.
SO2 is used as _________.
(oxidizing agent, reducing agent, bleaching agent)
144.
_________ is used as a dehydrating agent.
(HCl, HNO3, H2SO4)
145.
Air contains oxygen by volume _________.
(78%, 21%, 50%)
146.
When aqueous solution of NaCl is electrolysed the gas liberated at cathode is _________.
(Fluorine, Hydrogen, Chlorine)
147.
_________ is used in photography.
(NaCl, NaClO4, AgBr)
148.
Fluorspar is _________.
(CaF2, Na3AlF6, NaF)
149.
The most active halogen is _________.
(Chlorine, Iodine, Bromine, Fluorine)
150.
HOCl is the formula of _________.
(Hydrochloric acid, perchloric acid, Hypochlorous acid)
151.
When copper is treated with sulphur, it forms _________.
(copper sulphate, copper sulphide, copper sulphite)
152.
An acid which reacts with copper at room temperature is _________.
(Hydrocholic acid, Sulphuric acid, Nitric acid)
153.
Majority of the compounds of iron are _________ in colour.
(Green, blue, white)
154.
When aluminium is treated with sodium hydroxide it forms _________.
(Hydrogen, water, sodium aluminate)
155.
Colour of bronze is _________.
(Silvery white, Golden yellow, Brownish red)
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156.
Iron deposits found in Kala bagh are _________.
(Haematite, Limonite, Siderites)
157.
When methane is heated in presence of air, the heat released is known as _________.
(Heat of formation, Heat of combustion, Heat of neutralization)
158.
Formula of sucrose is _________.
(C6H12O6, C12H22O11, C6H10O5)
159.
The property of carbon atom to link with each other is known as _________.
(Catenation, Halogenation, combustion)
160.
In vast majority of carbon compounds, carbon behaves as _________.
(Divalent, Trivalent, Tetravalent)
NUMERICAL QUESTIONS
1.
Calculate the mass of oxygen produced by the decomposition of 5gm of potassium chlorate (KClO 3). (At.
Masses: K=39, Cl = 35.5, O=16)
2.
The normal temperature of human body is 98.6F. What are its corresponding temperatures on Celsius and
Kelvin scales?
3.
5.85 gm NaCl is dissolved in water so as to make 500cm3 solution. Determine the molarity of the solution.
(At. Masses: Na=23, Cl=35.5)
4.
Calculate the percentage composition of carbon and oxygen in carbon dioxide (CO2). (At. Masses: Carbon =
12, Oxygen = 16)
5.
The mass of a piece of gold is 482.5 gm. Its volume is 25cm3. Calculate its density.
6.
Calculate the density of a brick, which has the mass of 1.87Kg and volume of 750 cm 3.
7.
Determine the mass of sodium carbonate required to prepare 250 cm3 solution of 0.5 M.
8.
Calculate the percentage of nitrogen in Urea and Ammonium nitrate. (At. Masses = H= 1, O= 16, C = 12, N
= 14)
9.
The temperature of water is 45C. Find out the corresponding temperature in Fahrenheit and kelvin scales.
10. Determine the mass of sodium hydroxide required to prepare 500cm3 solution of O.25 M.
11. A cuboid of stone is 21 cm long, 6cm board and 10 cm thick. Its mass is 5.075 kg. Find its density.
12. Calculate the percentage of nitrogen in urea. (At. Masses: N = 14, C = 12, H = 1, O = 16)
13. How will you prepare 200cm3 solution of 10% NaOH by mass and decimolar solution of NaOH.
14. Determine the % concentration of the solution that contains 2gm common salt in 10g water.
15. Determine the number of moles in 900g of glucose (C6H12O6).
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16. Calculate the mass in g% in 0.1 mole of KOH.
17. What mass of Calcium bromide (CaBr2) is needed to prepare 150 cm3 of a 3.5 M solution?
18. A solutions of sulphuric acid was made by dissolving 20.0g of 98% sulphuric acid in 262cm 3 solution. What is
its molarity?
19. Calculate the molarity of a solution that contains 6.3gm crystalline oxalic acid dissolved in 100cm 3 solution.
20. Calculate the percentage of phosphorus present in calcium phosphate, calsium super phosphate and tripple
phosphate.
Write down the chemical formula of the following:
1.
Carbon Tetra Chloride
2.
Starch
3.
Ethyl Alcohol
4.
Otane
5.
Cuprite
6.
Malachite
7.
Azurite
8.
Copper Pyrite
9.
Sucrose
10. Acetic Acid
11. Citric Acid
12. Cholestrol
13. Baking Soda
14. Carbonic Acid
15. Hydrobromic Acid
16. Phosphoric Acid
17. Haematite
18. Limonite
19. Magnetite
20. Iron Pyrite
21. Chalcosite
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22. Copper Glance
23. Zinc Blende
24. Zincite
25. Smithsonite
26. Galena
27. Cerussite
28. Anglesite
29. Cinnabar
30. Epxom Salt
31. Gypsum
32. Heavy spar or Baryte
COMPLETION AND BALANCING OF EQUATIONS
Complete and balance the following equations:
1.
ZnCl2 + AgNO3

2.
Cu + H2SO4 (conc)
Heat

3.
NH4Cl + Ca(OH)2
Heat

4.
Al + Cl2
Heat

5.
NaBr + Cl2

6.
Mg + HCl (dil)

7.
NH3 + HCl (dil)

8.
CaCO3 + HCl (dil)

9.
AgNO3 + HCl (dil)

Pb(NO3)2 + HCl (dil)

10.
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11.
KClO3
Heat

12.
Na + Cl2

13.
CaCO3 + Cl2

14.
MnO2 + HCl

15.
CH4
Heat

16.
CH4 + Cl2

17.
Sn + Cl2

18.
Na + H2O

19.
Mg + H2O

20.
CO2 + H2O

21.
SO3 + H2O

22.
Zn + H2SO4 (dil)

23.
NaCl + H2SO4 (conc)

24.
Cu + H2SO4 (conc)

25.
C12H22O11 + H2SO4 (conc)
26.
Cu + H2SO4
Heat

27.
H2SO4SO3 + H2O

28.
H2S + O2
Heat

29.
CaCO3 + H2O + CO2


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30.
Na2SO3 + HCl

31.
Sb + Cl2

32.
CO + Cl2

33.
P + Cl2

34.
H2 + Cl2

35.
Fe + Cl2

36.
Al + O2

37.
Na2SO4 + Ca(NO3)2

38.
CaO + H2O

39.
NaHCO3 + Na2CO3

40.
CuO + H2

41.
Fe2O3

42.
S + O2

43.
SO2 + O2

44.
C + Cu2O

45.
Fe + HCl

46.
PCl3 + H2O

47.
H2O2

48.
Al + Cl2

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49.
ZnO + HNO3

50.
AgNO3 + NaCl

51.
NaOH + H2SO4

52.
Pb(NO3)2 + H2SO4

53.
C + O2 (limited)

54.
CaCO3
Heat

55.
ZnCl2 + AgNO3

56.
FeCl2 + Cl2

57.
BaCl2 + H2SO4

58.
Fe + HCl (dil)

59.
CaO + CO2

60.
ZnCl2 + NaOH

61.
Na2CO3 + HClO3

62.
Ca(HCO3)2 + HCl

63.
BiCl3 + H2O

64.
NH3 + O2

65.
Cu2S + O2

66.
Na + ZnCl2

67.
CO + O2

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68.
NH4OH + H2SO4

69.
NH4Cl + H2O

70.
Fe + S
Heat

71.
Hg + I2
Heat

72.
NaHCO3 + HCl

73.
MgO + H2SO4

74.
Fe2O3 + HCl

75.
Cr2O3 + H2SO4

76.
Na2O + SiO2

77.
PbO + SO3

78.
CaO + CO2

79.
P2O5 + Ca(OH)2

80.
NaOH + SO2

81.
NO2 + H2O

82.
P2O5 + H2O

83.
P2O3 + H2O

84.
Al + HCl

85.
Al + Fe2O3

86.
Al + NaOH

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87.
Zn + O2

88.
Zn + Cl2

89.
Zn + HCl

90.
Zn + NaOH

91.
Zn + NH3

92.
Zn + CuSO4

93.
Pb + Cl2

94.
Pb + O2

95.
Pb + HCl

96.
Pb + Ag+

97.
HNO3 + Mg

98.
HNO3 + Cu

99.
HNO3 + S

100. HNO3 + S

101. HNO3 + Ag

102. CuO + C

103. SnO2 + C

104. H2SO4 + C

105. HNO3 + C

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106. C + CO2

107. Zn + CO2

108. Ca(OH)2 + CO2

109. CaCO3 + CO2

110. CaC2 + N2

111. H2 + N2

112. Ca + N2

113. B + N2

114. Mg + N2

115. CuO + HNO3

116. Zn + HNO3

117. H2S + HNO3

118. SO2 + HNO3

119. FeSO4 + HNO3

120. P + O2

121. Na + O2

122. K + O2

123. Mg + O2

124. S + Cu

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125. S + C

126. S + Fe

127. S + Cl2

128. SO2 + H2S

129. CO + SO2

130. FeCl3 + SO2

131. KMnO4 + SO2

132. K2Cr2O7 + SO2

133. Sb + Cl2

134. KI + Cl2

135. NaOH + Cl2

136. CH4 + Cl2

137. CO + Cl2

138. NH3 + Cl2

139. NaCl + MnO2 + H2SO4

140. Cl2 + H2O

141. Al2O3 + NaOH

142. CuS + O2

DETECTION OF GROUP AND PERIOD FROM ATOMIC NUMBER
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1.
The atomic number of an element is 11. Write its name. To which group of the Periodic table does it belong?
2.
The atomic number of an element is 17. Write its name. To which group of the periodic table does it belong?
3.
The atomic number of an element is 15. Give the name, the electronic distribution in the shells, the group in
the periodic table and the valency of the element.
4.
The atomic number of an element is 8 and its mass number is 16. Write its normal valency, its electronic
configuration, number of neutrons in its atom and group number of the element in the periodic table.
5.
An element has 11 electrons, 11 protons and 12 neutrons. What will be its mass number and valence
number?
6.
Atomic number of an element is 17. Give the distribution of electrons in its shells, the number of protons
and the valence number.
NAMES OF CHEMICAL COMPOUNDS
Write down the names of the following chemical compounds:
1.
C12H22O11
2.
CH3COOH
3.
C6H12O6
4.
(NH2)2CO
5.
Cu2O
6.
[CuCO3.Cu(OH)2]
7.
2CuCO3.Cu(OH)2]
8.
CuFeS2
9.
C6H8O7
10. C27H46O
11. NaHCO3
12. Fe2O3
13. Fe2O3. 3H2O
14. Fe3O4
15. Fe2S
16. Cu2S
17. CuS
18. ZnS
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19. ZnO
20. ZnCO3
21. PbS
22. PbCO3
23. PbSO4
24. HgS
25. MgSO4. 7H2O
26. CaSO4. 2H2O
27. BaSO4
28. (NH4)2 CO3
29. Fe2(SO4)3
30. MnCl2
31. Al(NO3)2
32. KHSO4
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