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Download Tamil Nadu 12th Standard Chemistry question papers, model tests, one-mark questions, important questions, and public exam papers in PDF format. Free study materials and answer keys for TN State Board students.

Questions:

Multiple Choice Question

99 x 1 = 99

The half-life period of a first order reaction is 69.3 seconds. Its rate constant is ________.

(a)

10^-2 s^-1

(b)

10^-4 s^-1

(c)

10 s^-1

(d)

10² s^-1

Activation energy is equal to _______.

(a)

Threshold energy + Energy of colliding molecules

(b)

Threshold energy

(c)

Threshold energy x Energy of colliding molecules

(d)

Threshold energy - Energy of colliding molecules

Energy of activation of a reactant is reduced by ________.

(a)

reduced pressure

(b)

increased pressure

(c)

reduced temperature

(d)

increased temperature

Rate law cannot be determined from balanced chemical equation if ______.

(a)

Reverse reactions is not involved

(b)

It is an elementary reaction

(c)

It is a sequence of elementary reactions

(d)

All of the reactants is in excess. Rate law can be determined from balanced chemical equation if it is an elementary reaction.

In the graph showing Maxwell, Boltzmann distribution of energy _____.

(a)

area under the curve must not change with increase in temperature.

(b)

area under the curve increases in temperature.

(c)

area under the curve decreases with increase in temperature.

(d)

None of these above

Which one of the following is an example of pseudo first order reaction?

(a)

Acid hydrolysis of ester

(b)

Decomposition of HI

(c)

Synthesis of NH₃

(d)

All radioactive transformations

If the initial concentration of the reactants is doubled, then rate _____.

(a)

remains constant

(b)

doubled

(c)

is reduced to half of its value

(d)

is increased by four times of initial rate

Compound A reacts by first order kineties. At 25^oC, the rate constant of the reaction is 0.60 sec. What is the half life of A?

(a)

1.15 sec

(b)

0.4158 sec

(c)

0.093 sec

(d)

1.29 sec

For a reaction: aA ⟶ bB, the rate of reaction is doubled when the concentration of A is increased by four times. The rate of reaction is equal to _____.

(a)

k[A]^a

(b)

\(k{ \left[ A \right] }^{ \frac { 1 }{ 2 } }\)

(c)

\(k{ \left[ A \right] }^{ \frac { 1 }{ a } }\)

(d)

K[A]

10.

The term A in Arrhenius equation is called as _____.

(a)

Probability factor

(b)

Activation energy

(c)

Collision factor

(d)

Frequency factor

11.

During decomposition of an activated complex.

(a)

energy is always released

(b)

energy is always absorbed

(c)

energy does not change

(d)

products may be formed.

12.

For the following reaction, identify the order of reaction and dimension of the rate constant.
H₂O₂_(aq) +3I^-_(aq)+ 2H⁺ ⟶ 2H₂O₍₁₎ + I₃^- ; Rate = k[H₂O₂] [I]^-

(a)

2, L mol^-1 s^-1

(b)

1. s^-1

(c)

\(\frac { 3 }{ 2 } \), L^1/2 mol^-1/2 s^-1

(d)

None of these

13.

2A ⟶ B + C. It would be a zero order reaction when ______.

(a)

The rate of reaction is proportional to square of conc. of A

(b)

The rate of reaction remains same at any conc. of A.

(c)

The rate of remains unchanged at any conc. of B and C

(d)

The rate of reaction doubles if conc. of B is increased to double.

14.

Which of the following does not affect the rate of reaction?

(a)

Amount of the reactant taken

(b)

Physical state of the reactant

(c)

∆H of reaction

(d)

Size of vessel

15.

What would be the activation energy of a reaction when the temperature is increased from 27^oC to 37^oC?

(a)

534 kJ mol^-1

(b)

53.4 kJ mol^-1

(c)

5.34 kJ mol^-1

(d)

None of these

16.

The high reactivity of fluorine is due to________.

(a)

high ionisation energy

(b)

low bond dissociation energy

(c)

low electron affinity

(d)

high electro negativity

17.

Oxidation states of P in H₄P₂O₅, H₄P₂O₆, H₄P₂O₇ are respectively _______.

(a)

+3, +4, +5

(b)

+3, +5, +4

(c)

+5, +3, +4

(d)

+5, +4, +3

18.

Repeated use of which one of the following fertilizers would increase the activity of the soil_______.

(a)

Ammonium sulphate

(b)

Superphosphate of lime

(c)

Urea

(d)

Potassium nitrate

19.

The incorrect statement regarding structure of ozone is______.

(a)

Bond angle is less than 120°

(b)

It is linear

(c)

The two oxygen-oxygen bond length in ozone are identical

(d)

Both (b) and (c).

20.

Orthophosphorus acid on heating gives______.

(a)

Hypophosphorous

(b)

Orthophosphoric acid

(c)

Phosphine gas

(d)

both (b) and (c)

21.

Least volatile hydrogen halide is ______.

(a)

(b)

HCI

(c)

HBr

(d)

22.

When Copper is heated with cone HNO₃ it produces

(a)

Cu (NO₃)₂ and N₂O

(b)

Cu (NO₃)₂ and NO₂

(c)

Cu (NO₃)₂ and NO

(d)

Cu (NO₃)₂ NO and N₂O

23.

Which is dibasic?

(a)

Orthophosphoric acid

(b)

Pyrophosphoric acid

(c)

Orthophosphorus acid

(d)

Hypophosphorous acid

24.

Catenation property of group 15 elements, follow the order _______.

(a)

N < P < As < Sb < Bi

(b)

P >> N > As > Sb > Bi

(c)

P < N < As < Sb < Bi

(d)

N>> P > As > Sb > Bi

25.

Which of the following is correct?

(a)

H₃PO₃ is dibasic and reducing

(b)

H₃PO₃ is dibasic and non-reducing

(c)

H₃PO₄ is tribasic and reducing

(d)

H₃PO₃ is tribasic and non-reducing

26.

Crystals of NaCI has yellow colour due the presence of_________.

(a)

cation vacancy

(b)

F centres

(c)

both (a) and (b)

(d)

neither (a) nor (b)

27.

If electrical conductivity is found to be same in all directions through a solid the substance is ________ solid and the property is called _________.

(a)

crystalline, isotropy

(b)

amorphous, isotropy

(c)

crystalline, anisotropy

(d)

amorphous, isotropy

28.

The seven primitive crystal systems differ in the _______ arrangement.

(a)

crystallographic axes

(b)

angles

(c)

both (a) and (b)

(d)

Neither (a) or (b )

29.

A crystal which has the same unit cell and contains the same lattice points throughout the crystal is_________.

(a)

perfect

(b)

imperfect

(c)

distorted

(d)

both (b) and (c)

30.

An example of covalent crystal is _________.

(a)

CsCl

(b)

NaCl

(c)

ice

(d)

diamond

31.

The number of cesium ion per unit cell in CsCI crystal system is________.

(a)

(b)

(c)

(d)

32.

In a face centred cubic cell, an atom at the face contributes to the unit cell_______.

(a)

\(\frac{1}{4}\)Part

(b)

1Part

(c)

\(\frac{1}{2}\)Part

(d)

\(\frac{1}{8}\)Part

33.

The number of chloride ions present per unit of CsCI are _______.

(a)

(b)

(c)

(d)

34.

In an hexagonal crystal _______.

(a)

a=b=c,∝ =β=૪=90°

(b)

a=b=c,∝ =β=૪≠90°

(c)

a=b≠c,∝ =β=૪=90°

(d)

a=b≠c,∝ =β=90°૪=120°

35.

Which one of the following statements is wrong about Frenkel defect?

(a)

An ion occupies an interstitial position

(b)

Anion is much larger in size than the cation

(c)

The crystal remains neutral

(d)

Non-stoichiometric compound is formed

36.

Which type of defect is found in transition metals that have variable valency?

(a)

Frenkel defect

(b)

Schottky defect

(c)

Line defect

(d)

Metal deficiency defect

37.

The defect arising due to an ion occupying interstitial position is called _______.

(a)

Schottky defect

(b)

Metal excess defect

(c)

Frenkel defect

(d)

Metal deficiency defect

38.

Which one of the following statements is not true?

(a)

The heat of vaporisation of ionic crystals are high

(b)

Ionic crystals are soluble in non-polar solvent

(c)

Ionic crystals are hard and brittle

(d)

Ionic crystals are conductors in solution state

39.

The wavelength of X-ray is in the order of _______.

(a)

10^-8cm

(b)

10^-10c

(c)

10^-8 m

(d)

10^-10 nm

40.

Pick out the example for covalent and molecular crystal.

(a)

Ice, Diamond

(b)

Diamond, Ice

(c)

NaCl, FeS

(d)

FeS, Ice

41.

In the Bragg's equation for diffraction of X-rays, 'n' represents _______.

(a)

The number of moles

(b)

Avogadro number

(c)

A quantum number

(d)

Order of reflection

42.

Three atoms P, Q and R crystallize in a cubic solid lattice having P atom at corners Q atom at body centre and R atom at the face centres. Identify formula of the compound _______.

(a)

PQR

(b)

PQR₂

(c)

PQR₃

(d)

P₃QR

43.

Borax is _______.

(a)

Na₂[B₄O₅(OH)₄).8H₂O

(b)

Na₂[B₄O₅(OH)₆).7H₂O

(c)

Na₂[B₄O₃(OH)₈].6H₂O

(d)

Na₂[B₄O₂(OH)₁₀).5H₂O

44.

Silicones are ______.

(a)

ortho silicates

(b)

water repellent thermal insulators

(c)

both (a) and (b)

(d)

None of these

45.

The silicates which contain discrete tetrahedral units are _______.

(a)

ortho silicates

(b)

sheet silicates

(c)

pyrosilicates

(d)

three dimensional silicates

46.

Allotropy is due to ______.

(a)

difference in chemical properties

(b)

difference in the number of atoms in the molecules

(c)

difference in the arrangement of atoms in the molecules in the crystal

(d)

None of these

47.

If 'a' is the length of unit cell, then which one is correct relationship?

(a)

For simple cubic lattice, radius of metal atom =\(\frac{a}{2}\)

(b)

For bee lattice, radius of metal atom \(=\frac { \sqrt { 3a } }{ 4 } \)

(c)

For fcc lattice, radius of metal atom \(=\frac { a }{ 2\sqrt { 2 } } \)

(d)

All of these

48.

A solid with formula ABC₃ would probably have, _______.

(a)

A at body centre, B at face centres and C at corners of the cube

(b)

A at corners of cube, B at body centre, C at face centre

(c)

A at corners of hexagon, B at centres of the hexagon and C inside the hexagonal unit cell

(d)

A at corner, B at face centre, C at body centre

49.

Group 14 elements have general electronic configuration _______.

(a)

ns²

(b)

ns²np⁴

(c)

ns²np⁶

(d)

ns²np²

50.

All elements except carbon have the tendency to show maximum covalency of six ______

(a)

due to presence of vacant d-orbitals

(b)

due to absence of vacant d-orbitals

(c)

due to presence of partially filled d-orbitals

(d)

due to presence of completely filled d-orbitals

51.

Boron compounds behave as Lewis acid, because of their _______.

(a)

ionisation property

(b)

acidic nature

(c)

covalent nature

(d)

electron deficient nature

52.

Which one is correct statement for zeolite?

(a)

Zeolites are aluminosilicates having three dimensional framework

(b)

Hydrate zeolites are used as ion exchangers in hardening of soft water

(c)

Zeolites are alumino silicates

(d)

all the above

53.

Chemical formula of phosgene is_______.

(a)

COCl₂

(b)

CaOCl₂

(c)

CaCO₃

(d)

COCI

54.

Which one of the following compounds has similar structure to that of graphite?

(a)

Boron nitride

(b)

Boron Carbide

(c)

Aluminium Carbide

(d)

Aluminium Oxide

55.

A mixture of TiCl₄ and trialkyl aluminium is _________

(a)

hydroformylation of obfine

(b)

Zeigler - Natta Catalyst

(c)

interstitial compounds

(d)

ferromagnetic

56.

The general electronic configuration of 4f series of elements can be written as ________.

(a)

[Xe]4f^2-14 5d^0-46s²

(b)

[Xe]4f^2-145d^0-46s¹

(c)

[Xe] 4f^1-145⁰6s¹

(d)

[Xe]4f^2-145d^0-46s¹

57.

Equivalent weight of KMnO₄ in acidic medium is _______.

(a)

3.16

(b)

31.6

(c)

158

(d)

52.67

58.

The electronic configuration of Sc is ______.

(a)

[Ar] 3d¹ 4s²

(b)

[Ar] 3d² 4S¹

(c)

[Ar] 3d⁵ 4S¹

(d)

[Ar] 3d³ 4S¹

59.

In black and white photography, the developed film is fixed by washing with ______.

(a)

Hypo solution

(b)

AgBr solution

(c)

Na₂S₄O₆ solution

(d)

FeC₂O₄ solution

60.

On oxidation with KMnO₄ in acidic medium, SO₂ is oxidised to _______.

(a)

SO₂

(b)

H₂SO₄

(c)

SO₃^2-

(d)

H₂S

61.

Which of the following ions will exhibit colour in aqueous solutions?

(a)

SC³⁺(Z=21)

(b)

Ti³⁺(Z =22)

(c)

La³⁺(Z=57)

(d)

Lu³⁺(Z=71)

62.

Identify the correct reason for lanthanide contraction.

(a)

Decreasing nuclear charge

(b)

Decreasing screening effect

(c)

Increasing nuclear charge

(d)

Negligible screening effect

63.

The reaction of aqueous KMnO₄ with H₂O₂ in acidic condition gives_______.

(a)

Mn⁴⁺ and MnO₂

(b)

Mn⁴⁺ and O₂

(c)

Mn²⁺ and O₂

(d)

Mn²⁺ and O₃

64.

Which of the following statement is correct for 3d-transition element?

(a)

All metals except Zn and Sc form 'MO' Oxide

(b)

All metals except Sc forms 'MO' Oxide

(c)

All metals except Zn forms 'MO' Oxide

(d)

All metals except Mn forms 'MO' Oxide

65.

What are the species X and Y in the following?

(a)

CrO₃, CrO₄^2-

(b)

CrO₃, Cr₂O₃

(c)

CrO₄^-2, Cr₂O₇^2-

(d)

H₂CrO₄, H₂Cr₂O₇

66.

The lanthanide contraction is responsible for the fact that _______.

(a)

Zr and Zn have the same oxidation state

(b)

Zr and Hf have almost the same radius

(c)

Zr and Nb have similar oxidation state

(d)

Zr and Y have similar radius

67.

The trend in ionisation enthalpy of a transition element is not regular because,_______.

(a)

removal of one electron alters the relative energies of 4s and 3d orbitals

(b)

due to different electronic configuration (stability)

(c)

Poor screening of 3p-orbital

(d)

due to decrease in effective nuclear charge

68.

The highest possible oxidation state shown by osmium in its compound is_______.

(a)

(b)

(c)

(d)

+10

69.

Most of the transition metal ions are coloured, because of the ________.

(a)

presence of unpaired electrons

(b)

energy gap between two energy levels is very small

(c)

both (a) and (b)

(d)

neither (a) nor (b)

70.

Galena is_______.

(a)

PbS

(b)

ZnS

(c)

Ag₂S

(d)

FeS₂

71.

The percentage of carbon in high carbon steel is_________.

(a)

0.5 - 1%

(b)

0.15 - 1.5%

(c)

0.15 - 1.5%

(d)

0.15 - 0.3%

72.

\({ Zn }_{ (s) }+2\left[ Au(CN)_{ 2 } \right] ^{ - }_{ (aq) }\longrightarrow \left[ Zn(CN)_{ 4 } \right] ^{ 2- }_{ (aq) }+2A{ { u }_{ (s) } }\) In the above equation the oxidation state of metallic gold is_______

(a)

(b)

(c)

(d)

-2

73.

Na[Ag(CN)₂] is _________.

(a)

Sodium aurocyanide

(b)

Sodium meta aluminate

(c)

Aluminosilicate

(d)

Sodium dicyanoargentate

74.

Malachite has______ composition.

(a)

2CuCO₃.Cu(OH)₂

(b)

CuCO₃.Cu(OH)₂

(c)

Cu₂O

(d)

Cu₂S

75.

Pick out the alloy that contains a non-metal as a constituent in it ________.

(a)

Brass

(b)

Bronze

(c)

Steel

(d)

Invar

76.

\(\Delta { G }^{ o }\) vs T plot in the Ellingham's diagram slopes downward the reaction ________.

(a)

\(Mg+\frac { 1 }{ 2 } { O }_{ 2 }\longrightarrow MgO\)

(b)

\(C+\frac { 1 }{ 2 } { O }_{ 2 }\longrightarrow CO\)

(c)

\(2Ag+\frac { 1 }{ 2 } { O }_{ 2 }\longrightarrow { Ag }_{ 2 }O\)

(d)

\(2Ag+\frac { 1 }{ 2 } { O }_{ 2 }\longrightarrow { Ag }_{ 2 }O\)

77.

The blistered appearance of Cu obtained from the reverberatory furnace is due to evolution of________.

(a)

CO₂ gas

(b)

SO₂gas

(c)

NO₂

(d)

Due to evaporation of volatile materials

78.

Sodium magnesium and aluminum can be obtained from their ore by________.

(a)

electro metallurgy

(b)

pyro metallurgy

(c)

hydro metallurgy

(d)

smelting

79.

Identify the decreasing order of carbon content in different forms of iron________.

(a)

Wrought iron > Pig iron > cast iron

(b)

Cast iron > Pig iron > Wrought iron

(c)

Pig iron > Cast iron > Wrought iron

(d)

Cast iron > Wrought iron > Pig iron

80.

The structure of hexaaquatitanium (III) ion is _______.

(a)

[Ti(H₂O)₆]³⁺

(b)

[Ti(H₂O)₆]^3-

(c)

[Ti(H₂O)₅]H₂O

(d)

[Ti(H₂O)₆]

81.

Magnetic moment is given by the formula _______.

(a)

\(\sqrt { n(n+1) } \)

(b)

\(\sqrt { n(n+2) } \)

(c)

\(\sqrt { (n+2) } \)

(d)

\(\sqrt { { n }^{ 2 }+(n+2) } \)

82.

The chemical formula for diammine silver (I) chloride is _______.

(a)

[Ag(NH₃)₂] Cl

(b)

[Ag(NH₃)]Cl

(c)

[Ag(NH₂)₂]Cl

(d)

[Ag(NH₄)₂]Cl

83.

In co-ordination complexes, ligand ammonia is written as _______.

(a)

ammine

(b)

amine

(c)

ammonal

(d)

none of these

84.

Crystal field stabilization energy for high spin d⁴ octahedral complex is ______.

(a)

- 0. 6 \({ \triangle }_{ 0 }\)

(b)

- 1. 8 \({ \triangle }_{ 0 }\)

(c)

- 1. 6 \({ \triangle }_{ 0 }\)

(d)

- 1. 4 \({ \triangle }_{ 0 }\)

85.

An example of ambidentate ligand is _________.

(a)

cyano

(b)

nitro

(c)

chloro

(d)

triphenylphosphine

86.

The ligand capable of coordinating in two or more ways with the central metal ion are called _______ ligands.

(a)

didentate

(b)

tridentate

(c)

ambidentate

(d)

none of the above

87.

The coordination polyhedron of the complex [Cr(H₂O)₆]CI₃ is________.

(a)

square planar

(b)

tetrahedral

(c)

trigonal

(d)

octahedral

88.

The ionisation isomer of [Cr(H₂O)₄CI(NO₂)]Cl is _________.

(a)

[Cr(H₂O)₄Cl₂(NO)₂]

(b)

[Cr(H₂O)₄Cl₂]NO₂

(c)

[Cr(H₂O)₄Cl(ONO)]

(d)

both (a) and (b)

89.

A 'd' block metal ion has a magnetic moment of 1.732 BM. The number of unpaired electrons are _______.

(a)

(b)

(c)

(d)

90.

The coordination number of Ni(II) in [Ni(CN)₄]^2-is _______.

(a)

(b)

(c)

(d)

91.

The geometry of [Cu(NH₃)₄]²⁺ complex ion _______.

(a)

Linear

(b)

Tetrahedral

(c)

Square planar

(d)

Angular

92.

An example of a complex compound having coordination number 4 _______.

(a)

K₄[Fe(CN)₆]

(b)

[Co(en)₃]Cl

(c)

[Fe(H₂O)₆]Cl₃

(d)

[Cu(NH₃)₄]Cl₂

93.

Which is a double salt?

(a)

K₂SO₄AI₂(SO₄)₃24H₂O

(b)

NaCI

(c)

K₄[Fe(CN)₆]

(d)

KCl

94.

Which of the following will exhibit linkage isomerism?

(a)

[Co(NH₃)₅ (NO₂)]²⁺

(b)

[Co(H₂O)₅CO)]³⁺

(c)

[Fe(en)₂CI₂]⁺

(d)

all the above

95.

Coordination compounds are stabilised by Chelate effect. Which among the following is the most stable complex?

(a)

[Fe(CN)₆]^3-

(b)

[Fe(Co)₅]

(c)

[Fe(NH₃)₆]³⁺

(d)

[Fe(C₂O₄)₃]^3-

96.

Predict the geometry and hybridisation of Fe(Co)₅ _______.

(a)

Trigonal planar, dsp³

(b)

Trigonal bipyramidal, dsp³

(c)

Square planar dsp²

(d)

Octahedral d²sp³

97.

The hypothetical complex triamminediaqua chloridocobalt (III)chloride can be represented as _______.

(a)

[Co(NH₃)₃(H₂O)₂Cl]Cl₂

(b)

[Co(NH)₃(H₂O)Cl₃]

(c)

[Co(NH₂)₃(H₂O)₂Cl]

(d)

[Co(NH₃)₃(H₂O)₃]Cl₃

98.

Among the following complexes the one which shows zero crystal field stabilisation energy is _______.

(a)

[Mn(H₂O)₆]³⁺

(b)

[Fe(H₂O)₆]³⁺

(c)

[CO(H₂O)₆]²⁺

(d)

[CO(H₂O)₆]³⁺

99.

The total number of electrons donated by ligands to platinum ion in [Pt(en)₂CI₂] is _______.

(a)

(b)

(c)

(d)

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Answers Key:

Multiple Choice Question

99 x 1 = 99

(a)
10^-2 s^-1

(a)
Threshold energy + Energy of colliding molecules

(d)
increased temperature

(a)
area under the curve must not change with increase in temperature.

(a)
Acid hydrolysis of ester

(d)
is increased by four times of initial rate

(a)
1.15 sec

(b)
\(k{ \left[ A \right] }^{ \frac { 1 }{ 2 } }\)

10.

(d)
Frequency factor

11.

(a)
energy is always released

12.

(a)
2, L mol^-1 s^-1

13.

(b)
The rate of reaction remains same at any conc. of A.

14.

15.

(d)
None of these

16.

(b)
low bond dissociation energy

17.

(a)
+3, +4, +5

18.

(a)
Ammonium sulphate

19.

(b)
It is linear

20.

(d)
both (b) and (c)

21.

(a)
HF

22.

(b)
Cu (NO₃)₂ and NO₂

23.

24.

(b)
P >> N > As > Sb > Bi

25.

(a)
H₃PO₃ is dibasic and reducing

26.

(b)
F centres

27.

(b)
amorphous, isotropy

28.

29.

(a)
perfect

30.

(d)
diamond

31.

(d)
1

32.

33.

34.

(d)
a=b≠c,∝ =β=90°૪=120°

35.

(d)
Non-stoichiometric compound is formed

36.

(d)
Metal deficiency defect

37.

38.

(b)
Ionic crystals are soluble in non-polar solvent

39.

(a)
10^-8cm

40.

(b)
Diamond, Ice

41.

(d)
Order of reflection

42.

43.

(a)
Na₂[B₄O₅(OH)₄).8H₂O

44.

45.

(b)
sheet silicates

46.

47.

(d)
All of these

48.

(b)
A at corners of cube, B at body centre, C at face centre

49.

(d)
ns²np²

50.

(a)
due to presence of vacant d-orbitals

51.

(d)
electron deficient nature

52.

(d)
all the above

53.

(a)
COCl₂

54.

(a)
Boron nitride

55.

(b)
Zeigler - Natta Catalyst

56.

(a)
[Xe]4f^2-14 5d^0-46s²

57.

(b)
31.6

58.

(a)
[Ar] 3d¹ 4s²

59.

(a)
Hypo solution

60.

(b)
H₂SO₄

61.

(b)
Ti³⁺(Z =22)

62.

(d)
Negligible screening effect

63.

64.

(b)
All metals except Sc forms 'MO' Oxide

65.

(a)
CrO₃, CrO₄^2-

66.

(b)
Zr and Hf have almost the same radius

67.

(a)
removal of one electron alters the relative energies of 4s and 3d orbitals

68.

69.

70.

(a)
PbS

71.

(b)
0.15 - 1.5%

72.

(b)
0

73.

(d)
Sodium dicyanoargentate

74.

(b)
CuCO₃.Cu(OH)₂

75.

76.

(b)
\(C+\frac { 1 }{ 2 } { O }_{ 2 }\longrightarrow CO\)

77.

(b)
SO₂gas

78.

(a)
electro metallurgy

79.

80.

(a)
[Ti(H₂O)₆]³⁺

81.

(b)
\(\sqrt { n(n+2) } \)

82.

(a)
[Ag(NH₃)₂] Cl

83.

(a)
ammine

84.

(a)
- 0. 6 \({ \triangle }_{ 0 }\)

85.

(b)
nitro

86.

87.

(d)
octahedral

88.

(b)
[Cr(H₂O)₄Cl₂]NO₂

89.

(a)
1

90.

(b)
4

91.

92.

(d)
[Cu(NH₃)₄]Cl₂

93.

(a)
K₂SO₄AI₂(SO₄)₃24H₂O

94.

(a)
[Co(NH₃)₅ (NO₂)]²⁺

95.

(d)
[Fe(C₂O₄)₃]^3-

96.

(b)
Trigonal bipyramidal, dsp³

97.

(a)
[Co(NH₃)₃(H₂O)₂Cl]Cl₂

98.

(b)
[Fe(H₂O)₆]³⁺

99.

ONE MARK EXAM VOL I

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Std: 12th Standard - Chemistry

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