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Total questions: 121

Worksheet time: 1hrs 1mins

Name
Class
Date
1.

Molecular mass of CuSO4 x 5H2O is

a)

200 g/mole

b)

160 g/mole

c)

250 g/mole

d)

500 g/mole

e)

90 g/mole

2.

Find the correct name of PCl5

a)

nitrogen monooxide

b)

phosphorus trichloride

c)

dinitrogen tetraoxide

d)

boron trichloride

e)

phosphorus pentachloride

3.

Find the correct name of PCl3

a)

phosphorus pentachloride

b)

boron trichloride

c)

nitrogen monooxide

d)

dinitrogen tetraoxide

e)

phosphorus trichloride

4.

Find the correct name of BCl3

a)

phosphorus trichloride

b)

nitrogen monooxide

c)

boron trichloride

d)

phosphorus pentachloride

e)

dinitrogen tetraoxide

5.

Find the correct name of N2O4

a)

boron trichloride

b)

nitrogen monooxide

c)

dinitrogen tetraoxide

d)

phosphorus trichloride

e)

phosphorus pentachloride

6.

Find the correct name of LiCl

a)

boron trichloride

b)

sodium chloride

c)

calcium fluoride

d)

magnesium bromide

e)

lithium chloride

7.

Find the correct name of NaCl

a)

lithium chloride

b)

magnesium bromide

c)

boron trichloride

d)

calcium fluoride

e)

sodium chloride

8.

Find the correct name of MgBr2

a)

sodium chloride

b)

calcium fluoride

c)

lithium chloride

d)

boron trichloride

e)

magnesium bromide

9.

Find the correct name of CaF2

a)

magnesium bromide

b)

lithium chloride

c)

calcium fluoride

d)

sodium chloride

e)

boron trichloride

10.

In any chemical reaction, equilibrium is supposed to be establish when

a)

No correct answer

b)

Mutual opposite reactions undergo

c)

Velocity of mutual reactions become equal

d)

The temperature of mutual opposite reactions become equal

e)

Concentration of reactants and resulting products are equal

11.

Which of the following conditions represents an equilibrium

a)

No correct answer

b)

Freezing of ice in a open vessel, temperature of ice is constant

c)

Few drops of water is present along with air in a balloon, temperature of balloon is constant

d)

All the statements are correct for the equilibrium

e)

Water is boiling in an open vessel over stove, temperature of water is constant

12.

In chemical reaction A↔B, the system will be known in equilibrium when

a)

No correct answer

b)

Only 10% of A changes to B

c)

The rate of change of A to B and B to A on both the sides are same

d)

A completely changes to B

e)

50% of A changes to B

13.

When rate of forward reaction becomes equal to backward reaction, this state is termed as

a)

No correct answer

b)

Reversible state

c)

All of these

d)

Equilibrium

e)

Chemical equilibrium

14.

In chemical reaction A↔B, the system will be known in equilibrium when

a)

No correct answer

b)

A completely changes to B

c)

50% of A changes to B

d)

Only 10% of A changes to B

e)

The rate of change of A to B and B to A on both the sides are same

15.

For the reaction A+2B ↔ C, the expression for equilibrium constant is

a)

K=C/A•B^2

b)

K=C/A

c)

K=C/A-B

d)

K=C/A+B

e)

No correct answer

16.

Which of the following statement is correct with respect to the property of elements with an increase in atomic number in the carbon family (group 4)

a)

No correct answer

b)

Ionization energy increase

c)

Metallic character decrease

d)

Atomic size decrease

e)

Stability of +2 oxidation state increase

17.

The pair of amphoteric hydroxides is

a)

Be(OH)2,Zn(OH)2

b)

Fe(OH)2,Be(OH)2

c)

Be(OH)2,Mg(OH)2

d)

Al(OH)3,LiOH

e)

CO2

18.

Which of the following oxides is amphoteric in character

a)

BeO

b)

CO2

c)

SiO2

d)

CaO

e)

Fe(OH)2,Be(OH)2

19.

Which one of the following oxides is neutral

a)

CO

b)

ZnO

c)

SiO2

d)

SnO2

e)

CaO

20.

All elements in 3rd period have

a)

No correct answer

b)

3 complete sub-shells

c)

+3 valence electrons

d)

3 electrons less than the octet

e)

An atomic number 3

21.

Which shows variable valency

a)

No correct answer

b)

Radioactive elements

c)

d - block elements

d)

s - block elements

e)

p - block elements

22.

Most reducing agent is

a)

No correct answer

b)

Al

c)

K

d)

Mg

e)

Ba

23.

If the valency shell electronic structure for an element is ns2np5, this element will belong to the group of

a)

Radioactive elements

b)

Inert metals

c)

Halogens

d)

Alkali metals

e)

Noble gases

24.

If the valency shell electronic structure for an element is ns1, this element will belong to the group of

a)

Radioactive elements

b)

Inert metals

c)

Alkali metals

d)

Halogens

e)

Noble gases

25.

If the valency shell electronic structure for an element is ns2np6, this element will belong to the group of

a)

Radioactive elements

b)

Inert metals

c)

Noble gases

d)

Alkali metals

e)

Halogens

26.

Which will show maximum non-metallic character

a)

K

b)

Вe

c)

В

d)

Al

e)

Mg

27.

Which of the following halogen acids is least acidic

a)

HAc

b)

HBr

c)

HF

d)

HI

e)

HCl

28.

Variable valency in general, is exhibited by

a)

Radioactive elements

b)

s-block elements

c)

Transition elements

d)

Non-metals

e)

Gaseous elements

29.

An element of atomic weight 40 has 2, 8, 8, 2 as the electronic configuration. Which one of the following statements regarding this element is correct

a)

It belongs to V group of the periodic table

b)

It belongs to 5th period of the periodic table

c)

It belongs to III group of the periodic table

d)

It has 40 neutrons

e)

The formula of its oxide is MO

30.

Which of the following oxides is most basic

a)

Na2O

b)

SO2

c)

Al2O3

d)

SiO2

e)

Fe(OH)2,Be(OH)2

31.

Which of the following group of elements eliminates electron easily

a)

Fe, Cu, Zn

b)

N, P, As

c)

O, S, Se

d)

Cl, Ba, I

e)

Li, Na, K

32.

The maximum valency of an element with atomic number 7 is

a)

1

b)

2

c)

3

d)

5

e)

7

33.

Which of the following metals exhibits more than one oxidation state

a)

K

b)

Al

c)

Fe

d)

Na

e)

Mg

34.

Fluorine, chlorine, bromine and iodine are placed in the same group (17) of the periodic table, because

a)

They are electropositive

b)

They are electronegative

c)

They are non-metals

d)

Their atoms are generally univalent

e)

They have 7 electrons in the outermost shell of their atom

35.

Which of the following elements is found in native state

a)

Fr

b)

K

c)

Au

d)

Al

e)

Na

36.

Which is the weakest base

a)

Zn(OH)2

b)

KOH

c)

Ca(OH)2

d)

NaOH

e)

NaO2

37.

The valency shell of calcium contains

a)

8 electrons

b)

4 electrons

c)

6 electrons

d)

6 electrons

e)

2 electrons

38.

Which of the following halogens doesn't exhibit positive oxidation state in its compounds

a)

At

b)

Br

c)

F

d)

Cl

e)

J

39.

Which of the following gas does not have an octet or eight electrons in the outer shell

a)

O

b)

Rn

c)

He

d)

Ar

e)

Ne

40.

Between HF, HCl, HBr and HI, HF has the highest ionic character because

a)

It belongs to V group of the periodic table

b)

F has the highest electron affinity

c)

In HF, electronegativity difference is highest

d)

Atomic orbitals of H and F have almost similar energy

e)

Atomic orbitals of H and Cl have almost similar energy

41.

On going from right to left in a period in the periodic table the electronegativity of the elements

a)

Increases first then decreases

b)

Remain unchanged

c)

Decreases first then increases

d)

Increases

e)

Decreases

42.

Of the following elements, which one has highest electronegativity

a)

At

b)

Cl

c)

F

d)

J

e)

Br

43.

Going from fluorine to chlorine, bromine and iodine, the electronegativity

a)

Increases first then decreases

b)

Increases

c)

First decreases then increases

d)

Changes randomly

e)

Decreases

44.

The compound which could not act both as oxidising as well as reducing agent is

a)

Al2O3

b)

SO2

c)

MnO2

d)

CrO

e)

CaO

45.

Select the correct charge of nitrogen in HNO2

a)

+4

b)

-3

c)

+5

d)

+3

e)

+6

46.

Select the correct charge of nitrogen in NH3

a)

+6

b)

+5

c)

+4

d)

-3

e)

+3

47.

Select the correct charge of nitrogen in N2O5

a)

+3

b)

+4

c)

+6

d)

+5

e)

-3

48.

Select the correct charge of nitrogen in NO2

a)

-3

b)

+6

c)

+3

d)

+4

e)

+5

49.

M+3 ion loses 3e−. Its oxidation number will be

a)

0

b)

-3

c)

+3

d)

+6

e)

+5

50.

The oxidation number of sulphur in H2S2O7 and iron in K4Fe(CN)6 is respectively

a)

No correct answer

b)

+ 6 and + 4

c)

+ 6 and + 2

d)

+ 2 and + 2

e)

+ 8 and + 2

51.

Amongst the following identify the species with an atom in + 6 oxidation state

a)

CrO2Cl2

b)

MnO4

c)

NiF6

d)

Cr(CN)6

e)

No correct answer

52.

The oxidation number of sulphur in S8, S2F2, H2S respectively, are

a)

- 2, + 1 and - 2

b)

0, + 1 and + 2

c)

+ 2, +1 and - 2

d)

0, +1 and - 2

e)

No correct answer

53.

When MnO2 is fused with KOH, a coloured compound is formed, the product and its colour is

a)

No correct answer

b)

K2MnO4,purple green

c)

Mn2O3, brown

d)

KMnO4, purple

e)

Mn3O4, black

54.

In the equation H2S+2HNO3→2H2O+2NO2+S

The equivalent weight of hydrogen sulphide is

a)

No correct answer

b)

17

c)

68

d)

16

e)

34

55.

Which one of the following nitrates will leave behind a metal on strong heating

a)

Copper nitrate

b)

Ferric nitrate

c)

Manganese nitrate

d)

Silver nitrate

e)

No correct answer

56.

Prevention of corrosion of iron by zinc coating is called

a)

Electrolysis

b)

Cathodic protection

c)

Photo electrolysis

d)

Galvanization

e)

No correct answer

57.

The metal used in galvanizing of iron is

a)

Al

b)

Sn

c)

Pb

d)

Zn

e)

No correct answer

58.

In which of the following reactions there is no change in valency

a)

No correct answer

b)

BaO+H2CO4->BaSO4+H2O

c)

4KClO3->3KClO4+KCl

d)

2Ba+O2->2BaO

e)

2BaO+O2->2BaO2

59.

The free energy change for a reversible reaction at equilibrium is

a)

No correct answer

b)

Small positive

c)

Large positive

d)

Small negative

e)

0

60.

To prevent rancidification of food material, which of the following is added

a)

Reducing agent

b)

None of these

c)

Oxidising agent

d)

Anti-oxidant

e)

No correct answer

61.

25ml of 3.0M HNO3 are mixed with 75ml of 4.0M HNO3. If the volumes are additive, the molarity of the final mixture would be

a)

3.25M

b)

3.50M

c)

4.0M

d)

3.75M

e)

No correct answer

62.

The amount of anhydrous Na2CO3 present in 250 ml of 0.25 M solution is

a)

662.5 g

b)

66.25 g

c)

6.0 g

d)

6.625 g

e)

No correct answer

63.

Dilute one liter 1 molar H2SO4 solution by 5 liter water, the normality of that solution is

a)

10 N

b)

5 N

c)

0.2 N

d)

0.33 N

e)

No correct answer

64.

The molarity of 0.006 mole of NaCl in 100ml solution is

a)

0.6

b)

0.066

c)

0.006

d)

0.06

e)

No correct answer

65.

9.8g of H2SO4 is present in 2 liters of a solution. The molarity of the solution is

a)

0.2M

b)

0.1M

c)

0.005M

d)

0.05M

e)

No correct answer

66.

What will be the molarity of a solution containing 5g of sodium hydroxide in 250ml solution

a)

0.1

b)

1.0

c)

0.2

d)

0.5

e)

No correct answer

67.

Which of the following has maximum number of molecules

a)

No correct answer

b)

2g of H2

c)

16g of O2

d)

7g of N2

e)

16g of NO2

68.

Molarity is expressed as

a)

Gramm/liter

b)

Moles/1000 g

c)

Liter/mole

d)

Moles/liter

e)

No correct answer

69.

How much of NaOH is required to neutralize 1500 cm3 of 0.1 N HCl

a)

4 g

b)

60 g

c)

40 g

d)

6 g

e)

No correct answer

70.

If 5.85 g of NaCl (molecular weight 58.5) is dissolved in water and the solution is made up to 0.5 liter, the molarity of the solution will be

a)

0.4

b)

0.1

c)

1.0

d)

0.2

e)

No correct answer

71.

A mixture has 18g water and 414g ethanol. The mole fraction of water in mixture is (assume ideal behaviour of the mixture)

a)

0.9

b)

0.7

c)

0.4

d)

0.1

e)

No correct answer

72.

The number of molecules in 4.25 g of ammonia is approximately

a)

No correct answer

b)

1.5×10^23

c)

3.5×10^23

d)

0.5×10^23

e)

2.5×10^23

73.

The largest number of molecules is in

a)

No correct answer

b)

36g of H2O

c)

25g of CO2

d)

54g of N2O5

e)

46g of C2H5OH

74.

If 1 M and 2.5 liter NaOH solution is mixed with another 0.5 M and 3 liter NaOH solution, then molarity of the resultant solution will be

a)

0.50 M

b)

1.0 M

c)

0.80 M

d)

0.73 M

e)

No correct answer

75.

When the concentration is expressed as the number of moles of a solute per liter of solution it known as

a)

Mass percentage

b)

Mole fraction

c)

Normality

d)

Molarity

e)

No correct answer

76.

The normality of 2.3 M H2SO4 solution is

a)

0.23 N

b)

0.46 N

c)

2.3 N

d)

4.6 N

e)

No correct answer

77.

2.0 molar solution is obtained, when 0.5 mole solute is dissolved in

a)

250 ml solvent

b)

250 g solvent

c)

1000 ml solvent

d)

250 ml solution

e)

No correct answer

78.

How many gram of HCl will be present in 150ml of its 0.52 M solution

a)

5.70 g

b)

8.50 g

c)

3.65 g

d)

2.84 g

e)

No correct answer

79.

The molarity of 0.006 mole of NaCl in 100ml solution is

a)

0.006

b)

0.6

c)

0.066

d)

0.06

e)

No correct answer

80.

9.8g of H2SO4 is present in 2 liters of a solution. The molarity of the solution is

a)

0.2M

b)

0.1M

c)

0.01M

d)

0.05M

e)

No correct answer

81.

Determine the oxidation state of phosphorus in H3PO4:

a)

+1

b)

-3

c)

+3

d)

+5

e)

0

82.

Choose compound in which the oxidation state of nitrogen is equal to +3:

a)

No correct answer

b)

H2O3

c)

NaNO3

d)

NO2

e)

NH3

83.

Choose compound in which the oxidation state of nitrogen is equal to -3:

a)

No correct answer

b)

NH3

c)

NaNO3

d)

N2O3

e)

NO2

84.

Choose the minimal oxidation state for sulphur:

a)

No correct answer

b)

-2

c)

+6

d)

+4

e)

0

85.

Choose the maximal oxidation state for chlorine:

a)

+1

b)

-1

c)

+3

d)

+7

e)

No correct answer

86.

Which chemical element demonstrate a single possible oxidation state in compounds?

a)

Mn

b)

Cu

c)

O

d)

F

e)

No correct answer

87.

Choose basic oxide:

a)

No correct answer

b)

K2O

c)

Al2O3

d)

SO2

e)

SO3

88.

Choose acidic oxide:

a)

No correct answer

b)

SO2

c)

K2O

d)

Na2O

e)

Al2O3

89.

Choose amphoteric oxide:

a)

No correct answer

b)

Al2O3

c)

SO2

d)

K2O

e)

Na2O

90.

Choose insoluble (solubility < 0.1 g per 100 g of H2O) salt:

a)

No correct answer

b)

BaSo4

c)

NaNO3

d)

Na2SO4

e)

KCL

91.

For a spontaneous change, free energy change ΔG is

a)

No correct answer

b)

Positive

c)

Can be positive or negative

d)

Negative

e)

0

92.

The relation between ΔG and ΔH is

a)

TΔS−ΔG=ΔH

b)

ΔH=TΔG+ΔS

c)

ΔH=ΔG−TΔS

d)

ΔG=ΔH−TΔS

e)

No correct answer

93.

The relation ΔG=ΔH−TΔS was given by

a)

Faraday

b)

Boltzmann

c)

Thomson

d)

Gibbs-Helmholtz

e)

No correct answer

94.

Spontaneity of a chemical reaction is decided by the negative change in

a)

Enthalpy

b)

Internal energy

c)

Entropy

d)

Free energy

e)

No correct answer

95.

Gibb's free energy (G) is defined as

a)

ΔG=ΔH+TCp

b)

ΔH=ΔG−TΔS

c)

ΔG=ΔH+T/ΔS

d)

ΔG=ΔH−TΔS

e)

No correct answer

96.

__________ reactions release heat energy.

a)

Catalyzed

b)

Inhibited

c)

Endothermic

d)

Exothermic

e)

Neutralization

97.

__________ reactions absorb heat energy.

a)

Inhibited

b)

Catalyzed

c)

Exothermic

d)

Endothermic

e)

Neutralization

98.

Match a symbol of element antimony:

a)

F

b)

Hg

c)

Bi

d)

Sb

e)

Pb

99.

Match a symbol of element tungsten:

a)

F

b)

Hg

c)

Bi

d)

W

e)

Pb

100.

Match a symbol of element tin:

a)

F

b)

Hg

c)

Bi

d)

Sn

e)

Pb

101.

Find formulas of K3[FeF6] with its name

a)

tetrachloroplatinate(II) ion

b)

sodium dicyanocuprate(I)

c)

hexafluoroaluminate ion

d)

triamminetrihydroxochromium(III)

e)

potassium hexafluoroferrate(III)

102.

Find formulas of Na[Cu(CN)2] with its name

a)

potassium hexafluoroferrate (III)

b)

triamminetrihydroxochromium (III)

c)

tetrachloroplatinate (II) ion

d)

hexafluoroaluminate ion

e)

sodium dicyanocuprate (I)

103.

Find formulas of [Cr(NH3)3(OH)3] with its name

a)

sodium dicyanocuprate (I)

b)

hexafluoroaluminate ion

c)

triamminetrihydroxochromium (III)

d)

potassium hexafluoroferrate(III)

e)

tetrachloroplatinate(II) ion

104.

Find formulas of Na2[SnCl6] with its name

a)

potassium hexafluoroferrate(III)

b)

triamminetrihydroxochromium (III)

c)

tetrachloroplatinate(II) ion

d)

hexafluoroaluminate ion

e)

sodium hexachlorostannate(IV)

105.

Find formulas of [AlF6] with its name

a)

potassium hexafluoroferrate(III)

b)

sodium hexachlorostannate(IV)

c)

hexafluoroaluminate ion

d)

tetrachloroplatinate(II) ion

e)

triamminetrihydroxochromium (III)

106.

Find formulas of [PtCl4] with its name

a)

potassium hexafluoroferrate(III)

b)

sodium hexachlorostannate(IV)

c)

triamminetrihydroxochromium (III)

d)

hexafluoroaluminate ion

e)

tetrachloroplatinate(II) ion

107.

Find formulas of Mg[PdCl6] with its name

a)

triamminetrihydroxochromium (III)

b)

tetrachloroplatinate(II) ion

c)

sodium hexachlorostannate(IV)

d)

hexafluoroaluminate ion

e)

magnesium hexachloropalladate(IV)

108.

Find formulas of Ni[NH3)6] with its name

a)

triamminetrihydroxochromium (III)

b)

tetrachloroplatinate(II) ion

c)

sodium hexachlorostannate(IV)

d)

hexafluoroaluminate ion

e)

hexaamminenickel(II) ion

109.

Find formulas of [Co(NH3)3(H2O)2Cl]SO4 with its name

a)

sodium hexachlorostannate(IV)

b)

hexaamminenickel(II) ion

c)

hexafluoroaluminate ion

d)

tetrachloroplatinate(II) ion

e)

triamminediaquachlorocobalt(II) sulfate

110.

Find formulas of K2[Pt(NH3)Cl6] with its name

a)

sodium hexachlorostannate(IV)

b)

hexaamminenickel(II) ion

c)

hexafluoroaluminate ion

d)

tetrachloroplatinate(II) ion

e)

potassium amminehexachloroplatinate (IV)

111.

Choose s-element:

a)

Sr

b)

P

c)

Al

d)

Na

e)

Fe

112.

Choose p-element:

a)

Sb

b)

Cu

c)

He

d)

Cl

e)

Na

113.

Choose d-element:

a)

He

b)

Cl

c)

O

d)

Mn

e)

P

114.

What is the maximal number of electrons which can occupy all orbitals of the same s-sublevel?

a)

6

b)

10

c)

14

d)

2

e)

5

115.

What is the maximal number of electrons which can occupy all orbitals of the same p-sublevel?

a)

2

b)

10

c)

14

d)

6

e)

5

116.

What is the maximal number of electrons which can occupy all orbitals of the same d-sublevel?

a)

2

b)

6

c)

14

d)

10

e)

5

117.

What is the maximal number of electrons which can occupy all orbitals of the same f-sublevel?

a)

6

b)

2

c)

10

d)

14

e)

5

118.

How many unpaired electrons are there in the nitrogen atom (in its normal state)?

a)

5

b)

7

c)

2

d)

3

e)

1

119.

What is the number of electrons on the outer shell (level) of the chlorine atom:

a)

18

b)

10

c)

17

d)

7

e)

1

120.

Choose the electron configuration of the nitrogen atom (in its normal state):

a)

No correct answer

b)

1s°2,2s°2,2p°3

c)

1s°2,2s°3,2p°2

d)

1s°2,2s°3,2p°1

e)

1s°2,2s°1,2p°4

121.

Choose d-element:

a)

He

b)

Cl

c)

O

d)

Mn

e)

P

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