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.

(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 _________.

(C_nH_2n-2, C_nH_2n, C_nH_2n+2, C_nH_2n+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 _________.

(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)

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 _________.

(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 _________.

(alkane, alkene, alkyne)

58.        Sui gas and kerosene oil both have the general formula _________.

(C_nH_2n+2, C_nH_2n+1, C_nH_2n-2, C_nH_2n-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^-, O^2-)

69.        Present standard for determining relative atomic mass

(Hydrogen, chlorine, carbon ¹²)

70.        I calorie is equal to _________ joules.

(4.0, 2.2, 0.5, 4.18)

71.        Atomic mass unit is _________.

(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 _________

(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)

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)

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)

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)

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)

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)