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sslc_science-chemistry_em

Total questions: 93

Worksheet time: 47mins

Name
Class
Date
1.

which of the following has the smallest mass

a)

6.023x1023

b)

1 atom of He

c)

2 g of He

d)

1 mole atoms of He

2.

Which of the following is a triatomic molecule?

a)

glucose

b)

helium

c)

carbon di oxide

d)

hydrogen

3.

Th e volume occupied by 4.4 g of CO2 at

S.T.P

a)

22.4 litre

b)

2.24 litre

c)

0.24 litre

d)

0.1 litre

4.

Mass of 1 mole of Nitrogen atom is

a)

28 amu

b)

14 amu

c)

28 g

d)

14 g

5.

Which of the following represents 1 amu?

a)

Mass of a C – 12 atom

b)

Mass of a hydrogen atom

c)

1/12th of the mass of a C – 12 atom

d)

Mass of O – 16 atom

6.

Which of the following statement is incorrect?

a)

One gram of C – 12 contains Avogadro’s number of atoms.

b)

One mole of oxygen gas contains Avogadro’s number of molecules.

c)

One mole of hydrogen gas contains Avogadro’s number of atoms

d)

One mole of electrons stands for 6.023 × 1023 electrons.

7.

The volume occupied by 1 mole of a diatomic gas at S.T.P is

a)

11.2 litre

b)

5.6 litre

c)

22.4 litre

d)

44.8 litr

8.

In the nucleus of 20Ca40, there are

a)

20 protons and 40 neutrons

b)

20 protons and 20 neutrons

c)

20 protons and 40 electrons

d)

40 protons and 20 electrons

9.

The gram molecular mass of oxygen molecule is

a)

16 g

b)

18 g

c)

32 g

d)

17 g

10.

1 mole of any substance contains ____ molecules.

a)

6.023 × 1023

b)

6.023 × 10-23

c)

3.0115× 1023

d)

12.046 × 1023

11.

The number of periods and groups in the periodic table are______.

a)

6,16

b)

7,17

c)

8,18

d)

7,18

12.

Atoms of different elements having _______ mass number, but ________ atomic numbers are called isobars.

a)

same , different

b)

different , same

c)

one , two

d)

two , one

13.

Atoms of different elements having same number of ___________ are called isotones.

a)

electrons

b)

neutrons

c)

protons

d)

positrons

14.

Atoms of one element can be transmuted into atoms of other element by ________.

a)

natural method

b)

by some plant juices

c)

artificial transmutaion

d)

magic

15.

The sum of the numbers of protons and neutrons of an atom is called its __________

a)

atomic number

b)

neutron number

c)

proton number

d)

mass number

16.

Relative atomic mass is otherwise known as __________

a)

standard atomic weight

b)

mass number

c)

atomic number

d)

proton number

17.

The average atomic mass of hydrogen is ___________ amu

a)

1008

b)

1.008

c)

1

d)

8

18.

If a molecule is made of similar kind of atoms, then it is called ____________ atomic molecule

a)

hetero

b)

homo

c)

multi

d)

none of these

19.

The number of atoms present in a molecule is called its ____________

a)

atomicity

b)

atomic number

c)

mass number

d)

neutron number

20.

One mole of any gas occupies ________ ml at S.T.P

a)

22.4

b)

2.24

c)

22400

d)

224

21.

Atomicity of phosphorous is ___________

a)

1

b)

2

c)

4

d)

3

22.

The basis of modern periodic law is ...

a)

atomic number

b)

atomic mass

c)

isotopic mass

d)

number of neutrons

23.

..... group contains the menger of halogen family

a)

17th

b)

15th

c)

18th

d)

16th

24.

.... is a relative periodic property.

a)

Atomic radii

b)

ionic radii

c)

electron affinity

d)

electronegativity

25.

Chemical formula if rust is .....

a)

FeO.xH2O

b)

FeO4.xH2O

c)

Fe2O3.xH2O

d)

FeO

26.

In the alumino thermic process the role of Al is

a)

Oxidizing agent

b)

reducung agent

c)

hydrogenating agent

d)

sulphurising agent

27.

The process of coating the surface of metal with a thin layer of zinc is called .....

a)

painting

b)

thinning

c)

galvanization

d)

electroplating

28.

Which of the following have inert gases 2 electrons in the outermost shell

a)

He

b)

Ne

c)

Ar

d)

Kr

29.

Neon shows zero electron affinity due to

a)

stable arreangement of neutrons

b)

stable configuration of electrons

c)

reduced size

d)

increased density

30.

........ is an important metal to form amalgam.

a)

Ag

b)

Hg

c)

Mg

d)

Al

31.

If the electronegativity difference between two bonded atoms in a molecule is greater than 1.7, the nature of bonding is ______

a)

ionic

b)

covalent

c)

nuclear

d)

none of these

32.

________ is the longest period in the periodical table

a)

seventh period

b)

sixth period

c)

fifth period

d)

fourth period

33.

________ forms the basis of modern periodic table

a)

atomic number

b)

mass number

c)

proton number

d)

neutron number

34.

If the distance between two Cl atoms in Cl 2 molecule is 1.98Å, then the radius of Cl atom is ________

a)

99Ao

b)

9.9Ao

c)

0.99Ao

d)

990Ao

35.

Among the given species A–,A+, and A, the smallest one in size is ________

a)

A+

b)

A-

c)

A

d)

A and A+

36.

The scientist who propounded the modern periodic law is ________.

a)

Henry Moseley

b)

charles

c)

Boyle

d)

curie

37.

Across the period, ionic radii ________

a)

decreases

b)

increases

c)

connstant

d)

no change

38.

________ and ________ are called inner transition elements

a)

Lanthanides,Actinides

b)

He, H

c)

Alkaline,Alkaline earth

d)

He,Ne

39.

The chief ore of Aluminium is ......

a)

Bauxite

b)

Cryolite

c)

Corundum

d)

None of these

40.

The chemical name of rust is .....

a)

hydrated ferric oxide

b)

freeic oxide

c)

ferrous oxide

d)

hydrated ferrous oxide

41.

A solution is a .......... mixture

a)

homogenous

b)

heterogeneous

c)

homogeneous and heterogeneous

d)

non homogeneous

42.

The number of componenets in a binary solution is .........

a)

2

b)

3

c)

4

d)

5

43.

Which of the following is the universal solvent

a)

Acetone

b)

Benzene

c)

Water

d)

Alcohol

44.

A solution in which no more solute can be dissolved in a definite amount of solvent at a given temperature is called _______

a)

Saturated solution

b)

un saturated solution

c)

Super saturated solution

d)

Dilute solution

45.

Identify the non aqueous solution

a)

sodium chloride in water

b)

glucose in water

c)

copper sulphate in water

d)

sulphur in carbon di sulphide

46.

When pressure is increased at constant temperature the solubility of gases in liquid ___________.

a)

no change

b)

increases

c)

decreases

d)

no reaction

47.

Solubility of NaCl in 100 ml water is 36 g. If 25 g of salt is dissolved in 100 ml of water how much more salt is required for saturation _____________

a)

12 g

b)

11 g

c)

16 g

d)

20 g

48.

A 25% alcohol means

a)

25 ml alcohol in 100 ml of water

b)

25 ml alcohol in 25 ml of water

c)

25 ml alcohol in 75 ml of water

d)

75 ml alcohol in 25 ml of water

49.

Deliquescence is due to __________

a)

strong affinity to water

b)

less affinity to water

c)

strong hatred to water

d)

inertness to water

50.

Which of the following is hygroscopic in nature?

a)

ferric chloride

b)

copper sulphate penta hydrate

c)

silica gel

d)

none of the above

51.

The component present in lesser amount, in a solution is called _______

a)

solute

b)

amalgam

c)

solvent

d)

salt

52.

Example for liquid in solid type solution is ....

a)

amalgam

b)

polar

c)

solute

d)

solvent

53.

solubility is the amount of solute dissolved in ....g of solvent.

a)

50

b)

100

c)

200

d)

75

54.

polar compounds are soluble in ............ solvents.

a)

non polar

b)

amalgam

c)

polar

d)

none of these

55.

volume percentage decreases with increase in temperature because .....

a)

contraction of the liquid

b)

no change in liquid

c)

expansion of liquid

d)

none of these

56.

H2(g) + Cl2(g) -> 2HCl(g) is a

a)

Decomposition reaction

b)

combination reaction

c)

Single displacement reaction

d)

Double displacement reaction

57.

Photolysis is a decomposition reaction caused by

a)

heat

b)

electricity

c)

light

d)

mechanical energy

58.

A reaction between carbon and oxygen is represented by C(s) + O2(g) -->CO2(g) + Heat. In which of the type(s), the above reaction can be classified?

i)combination reaction

ii)Combustion reaction

iii)Decomposition reaction

iv)Irreversible reaction

a)

i and ii

b)

i and iv

c)

i , ii and iii

d)

i,ii and iv

59.

The chemical equation

Na2SO4(aq) +BaCl2(aq) -->BaSO4(s)+2NaCl(aq)

a)

Neutralisation

b)

Combustion

c)

Precipitation

d)

Single displacement

60.

Which of the following statements are correct about a equilibrium?

i) It is dynamic in nature

ii) The rate of the forward and backward reactions are equal at equilibrium

iii)Irreversible reactions do not attain chemical equilibrium

iv)The concentration of reactants and products may be different

a)

i,ii and iii

b)

i,ii and iv

c)

ii,iiii and iv

d)

iii and iv

61.

A single displacement reaction is represented by X(s) + 2HCl(aq) -->XCl2(aq) + H2(g). Which of the following could be X?

i) Zn

ii) Ag

iii)Cu

iv)Mg

a)

i and ii

b)

ii and iii

c)

iii and iv

d)

i and iv

62.

Which of the following is not an "element + element ->compound" reaction

a)

C(s) + O2(g) ---> CO2(g)

b)

2K(s) + Br2(l) ---> 2KBr(s)

c)

2CO(g) + O2(g) ---> 2CO2(g)

d)

4Fe(s) + 3O2(g) ---> 2Fe2O3(s)

63.

Which of the following represents a precipitation reaction?

a)

A(s) + B(s) --> C(s) + D(s)

b)

A(s) + B(aq) --> C(aq) + D(l)

c)

A(aq) + B(aq) --> C(s) + D(aq)

d)

A(aq) + B(s) --> C(s) + D(aq)

64.

The pH of a solution is 3. its [OH-] concentration is

a)

1 x 10-3 M

b)

3 M

c)

1 x 10-11 M

d)

11 M

65.

powdered CaCO3 reacts more rapidly than flaky CaCO3 because of ...........

a)

large surface area

b)

high pressure

c)

high concentration

d)

high temperature

66.

A reaction between an acid and a base is called...

a)

neutralization

b)

single displacement

c)

double displacement

d)

ionic

67.

When lithium metal is placed in hydrochloric acid, ..... gas is evolved

a)

chlorine

b)

hydrogen

c)

helium

d)

oxygen

68.

The equilibrium attained during the melting of ice is known as .....

a)

chemical equilibrium

b)

crystallisation

c)

physical equilibrium

d)

evoporaisation

69.

The pH of a fruit juice is 5.6. if you add slaked lime to this juice its pH ........

a)

increases

b)

decreases

c)

no change

d)

doubled

70.

The value of ionic product of water at 250C is ....

a)

1.00 x 1014 mol2dm-6

b)

100 x 10-14 mol2dm-6

c)

10.0 x 10-14 mol2dm-6

d)

1.00 x 10-14 mol2dm-6

71.

The normal pH of human blood is .....

a)

7.4

b)

7.8

c)

6.4

d)

6.8

72.

Electrolysis is type of .............. reaction

a)

compound to element

b)

element decomposition

c)

ionic

d)

covalent

73.

The number of products formed in a synthesis reaction is ....

a)

1

b)

2

c)

3

d)

4

74.

chemical volcano is an example for .... type of reaction

a)

single displacement

b)

double displacement

c)

decomposition

d)

neutralization

75.

The ion formed by dissolution of H+ in water is called ....

a)

helium ion

b)

Hydronium ion

c)

oxygen ion

d)

chlorine ion

76.

The molecular formula of an open chain organic compound is C3H6. The class of the compound is

a)

alkane

b)

alkene

c)

alkyne

d)

alcohol

77.

The IUPAC name of an organic compound is 3-methyl butan-1-ol. What type of compound it is?

a)

Aldehyde

b)

Carboxylixc acid

c)

Ketone

d)

Alcohol

78.

The secondary suffix used in IUPAC nomenclature of an aldehyde is ........

a)

-ol

b)

-oic acid

c)

-al

d)

-one

79.

Which of the following pairs can be successive members of a homologous series?

a)

C3H8 and C4H10

b)

C2H2 and C2H4

c)

CH4 and C2H6

d)

C2H5 OH and C4H8 OH

80.

C2H5OH + 3O2 --> 2CO2 +3H2O is a

a)

Reduction of ethanol

b)

combustion of ethanol

c)

oxidation of ethanoic acid

d)

oxidation of ethnal

81.

Rectified spirit is an aqueous solution which contains about ....... of ethanol

a)

95.5%

b)

75.5%

c)

55.5%

d)

45.5%

82.

Which of the following are used as anaesthetics?

a)

carboxylic acids

b)

ethers

c)

esters

d)

aldehydes

83.

TFM is soaps represents ..... content in soap

a)

meneral

b)

vitamin

c)

fatty acid

d)

carbohydrate

84.

Which of the following statements is wrong about detergents?

a)

it is sodium salt of long chain fatty acids

b)

it is sodium salts of sulphonic acids

c)

The ionic part in a detergent is -SO3- Na+

85.

An atom or a group of atoms which is responsible for chemical characteristics of an organic compound is called .....

a)

functional group

b)

root word

c)

Furan

d)

None of these

86.

The general molecular formula of alkynes is _____________

a)

CnH2n

b)

CnH2n-2

c)

CnH2n+2

d)

CnH2n-2 OH

87.

In IUPAC name, the carbon skeleton of a compound is represented by _________

a)

root word

b)

prefix

c)

suffix

d)

all of these

88.

___________ compounds decolourize bromine water.

a)

saturated

b)

unsaturated

c)

organic

d)

inorganic

89.

Dehydration of ethanol by conc. Sulphuric acid forms _______

a)

ethane

b)

ethene

c)

methane

d)

propane

90.

100% pure ethanol is called ......

a)

alcohol

b)

pure alcohol

c)

absolute alcohol

d)

propanol

91.

Ethanoic acid turns _______ litmus to _________

a)

blue , red

b)

red , blue

c)

colorless , pink

d)

pink , colorless

92.

The alkaline hydrolysis of fatty acids is termed as _____________

a)

saturated

b)

unsaturated

c)

saponification

d)

esterification

93.

Biodegradable detergents are made of _________ chain hydrocarbons

a)

straight

b)

branched

c)

carbon

d)

none of these

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