Plus One Public Exam March 2019 One Mark Question Paper

Download Tamil Nadu 11th 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

98 x 1 = 98

Which of the following pairs of elements exhibit diagonal relationship?

(a)

Be and Mg

(b)

Li and Mg

(c)

Be and B

(d)

Be and Al

Which of the following orders of ionic radii is correct?

(a)

H^- > H⁺ > H

(b)

Na⁺ > F^- > O^2-

(c)

F > O^2- > Na⁺

(d)

None of these

The element with positive electron gain enthalpy is _________

(a)

Hydrogen

(b)

Sodium

(c)

Argon

(d)

Fluorine

Identify the wrong statement.

(a)

Amongst the isoelectronic species, smaller the positive charge on cation, smaller is the ionic radius

(b)

Amongst isoelectric species greater the negative charge on the anion, larger is the ionic radius

(c)

Atomic radius of the elements increases as one moves down the first group of the periodic table

(d)

Atomic radius of the elements decreases as one moves across from left to right in the 2^nd period of the periodic table.

Various successive ionisation enthalpies (in kJ mol^-1) of an element are given below.

IE₁	IE₂	IE₃	IE₄	IE₅
577.5	1,810	2,750	11,580	14,820

The element is

(a)

phosphorus

(b)

Sodium

(c)

Aluminium

(d)

Silicon

Assertion: Permanent hardness of water is removed by treatment with washing soda.
Reason: Washing soda reacts with soluble calcium and magnesium chlorides and sulphates in hard water to form insoluble carbonates

(a)

Both assertion and reason are true and reason is the correct explanation of assertion.

(b)

Both assertion and reason are true but reason is not the correct explanation of assertion.

(c)

Assertion is true but reason is false

(d)

Both assertion and reason are false

Which one of the following is not a path function?

(a)

Work

(b)

Heat

(c)

Pressure

(d)

Either (a) or (b)

Hot water in a thermos flask is an example of ______

(a)

closed system

(b)

open system

(c)

isolated system

(d)

isochoric system

On moving from left to right across a period in the periodic table, the metallic character__________.

(a)

increases

(b)

decreases

(c)

remains constant

(d)

first increases and then decreases

10.

Which of the following is used in photoelectric cells?

(a)

(b)

(c)

(d)

11.

Which alkaline earth metal do not import colour to a non-Iuminous flame?

(a)

Beryllium

(b)

Calcium

(c)

Magnesium

(d)

Barium

12.

Which one of the following metal act as co-factor in phosphate transfer of ATP by enzymes?

(a)

Calcium

(b)

Beryllium

(c)

Magnesium

(d)

Sodium

13.

How many grams are contained in 1 gram atom of Na?

(a)

13g

(b)

1 g

(c)

23 g

(d)

1/23g

14.

Which one of the following is absolute zero?

(a)

293 K

(b)

273 K

(c)

-273.15^o C

(d)

0^o C

15.

The instrument used for measuring the atmospheric pressure is ___________.

(a)

lactometer

(b)

barometer

(c)

electrometer

(d)

ammeter

16.

Which of the following is the correct electronic configuration of noble gases?

(a)

ns² np⁶ nd¹⁰

(b)

ns² np⁵

(c)

ns² np⁶

(d)

ns² np³

17.

Hydrogen resembles halogens in many respects for which several factors are responsible. Of the following factors which one is most important in this respect?

(a)

Its tendency to lose an electron to form a cation

(b)

Its tendency to gain an electron to attain stable electronic configuration.

(c)

Its low negative electron gain enthalpy value

(d)

Its small size

18.

Which of the following statements is correct for an electron that has the quantum numbers n = 4 and in = -2.

(a)

The electron may be in 2p orbital

(b)

The electron may be in 4d orbital

(c)

The electron is in the second main shell

(d)

The electron must have spin quantum number as \(+\frac{1}{2}\)

19.

The idea of stationary orbits was first given by_________.

(a)

Rutherford

(b)

J.J. Thomson

(c)

Niels Bohr

(d)

Max Planck

20.

de Broglie equation is_________

(a)

E = \(h \ \gamma\)

(b)

E = mc²

(c)

\(\gamma ={E_2-E_1 \over h}\)

(d)

\(\lambda ={h\over mv}\)

21.

Which of the following experiment proves the presence of an electron in an atom?

(a)

Rutherford's \(\alpha\)-ray scattering experiment

(b)

Davisson and Germer experiment

(c)

J. J. Thomson cathode ray experiment

(d)

G.P. Thomson gold foil experiment

22.

Consider the following statements.
(i) Silver, Gold, Mercury and Platinum do not have any effect on water.
(ii) Carbon, Sulphur and Phosphorous do not react with water.
(iii) Beryllium reacts with water less violently.
Which of the following statements is/are not correct?

(a)

(i) only

(b)

(ii) and (iii)

(c)

(iii) only

(d)

(ii) only

23.

Which set of the metals do not have any effect on water?

(a)

Ag, Au, Pt

(b)

Na, Mg, Al

(c)

Fe, Ca, Zn

(d)

Fe, Pb, Na

24.

For the reaction, X₂ O₄(l) \(\rightarrow\) 2 XO₂ (g), \(\Delta\)U=2.1 Kcal, \(\Delta\)S = 20 cal K^-1 at 300 K. Hence,\(\Delta\)G is:

(a)

2.7 Kcal

(b)

-2.7 Kcal

(c)

9.3 K.=cal

(d)

-9.3 Kcal

25.

Gadolinium belong to 4f series. Its atomic number is 64. Which of the following is the correct electronic configuration of gadolinium?

(a)

[Xe]4f⁹5s¹

(b)

[Xe]4f⁷5d¹6s²

(c)

[Xe]4f⁶5d²6s²

(d)

[Xe]4f⁸d²

26.

The enthalpy of vapourisation of a liquid is 30 kJ mol^-1 and the entropy of vapourisation is 75 JK^-1 mol^-1. The boiling point of the liquid at 1 atm is __________

(a)

250K

(b)

400K

(c)

450K

(d)

600K

27.

Which of the following is a state function?

(a)

(b)

\(\Delta\)q

(c)

(d)

\(\Delta\)S

28.

Electronic configuration of species M²⁺ is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ and its atomic weight is 56. The number of neutrons in the nucleus of species M is ________

(a)

(b)

(c)

(d)

29.

Which of the following diagram directly describes the behaviour of a fixed mass of an ideal gas?

(a)

(b)

(c)

(d)

30.

Quick lime is ________

(a)

CaCO₃

(b)

CaO

(c)

CaSO₄.2H₂O

(d)

Ca(OH)₂

31.

Which of the following is electron precise hydride?

(a)

B₂H₆

(b)

NH₃

(c)

H₂0

(d)

CH₄

32.

Choose the incorrect statement:

(a)

The boiling points of both deuterium and tritium are higher than that of protium.

(b)

The inter nuclear distances between the two bonded atoms are different in all the isotopes.

(c)

Enthalpy of dissociation is high in tritium

(d)

both (b) and (c)

33.

Solve: ΔH=10 k cal mol^-1, ΔS=20 cal deg^-1 mol^-1 and T=300k. Then ΔG=?

(a)

-18,000 cals mol^-1

(b)

18,000 cals mol^-1

(c)

-16,000 cals mol^-1

(d)

4000 cals mol^-1

34.

What is correct about ΔG __________

(a)

It is zero for reversible reaction

(b)

It is positive for spontaneous reactions

(c)

It is negative for non-spontaneous reaction

(d)

It is zero for non-spontaneous reaction

35.

When water freezes in a glass beaker, ΔS of the system _____

(a)

ΔS>0

(b)

ΔS<0

(c)

ΔS=0

(d)

ΔS≥0

36.

Several blocks of magnesium are fixed to the bottom of a ship to ___________

(a)

Keep away the sharks

(b)

prevent of rusting of iron ships

(c)

make the ship lighter

(d)

prevent puncturing by under sea rocks

37.

Dead burnt plaster is ________

(a)

CaSO₄

(b)

CaSO₄·1/2H₂0

(c)

CaSO₄.H₂O

(d)

CaSO₄.2H₂O

38.

Which among the following is not a state function?

(a)

Pressure

(b)

Volume

(c)

Temperature

(d)

Work

39.

For an isothermal process _____

(a)

q = 0

(b)

dV = 0

(c)

dT = 0

(d)

dP = 0

40.

Which orbital diagram gives an insight to the highest ionization energy?

(a)

(b)

(c)

(d)

41.

"The relative tendency of a bonded atom in a molecule to attract the shared pair of electrons towards itself" is termed as_____

(a)

electron gain enthalpy

(b)

electronegativity

(c)

electron affinity

(d)

ionisation energy

42.

In a closed room of 1000 m³ a perfume bottle is opened up. The room develops smell. This is due to which property of gases _____________

(a)

Viscosity

(b)

Density

(c)

Diffusion

(d)

None

43.

What will be the basicity of H₃BO₃, which is not a protic acid?

(a)

One

(b)

Two

(c)

Three

(d)

Four

44.

Which pair of elements has the same characteristic chemical properties?

(a)

Z = 13, Z = 22

(b)

Z = 2, Z =4

(c)

Z = 4, Z = 24

(d)

Z = 3, Z = 11

45.

A gas such as carbon monoxide would be most likely to obey the ideal gas law at ___________

(a)

High temperature and high pressure

(b)

High temperature and low pressure

(c)

Low temperature and high pressure

(d)

Low temperature and high pressure

46.

Match the list - I with List - II and select the correct answer using the code given below the lists.

List-I	List-II
A. \(\frac { { r }_{ 1 } }{ { r }_{ 2 } } =\sqrt { \frac { { M }_{ 2 } }{ { M }_{ 1 } } } \)	1. Boyle's law
B. PV = constant	2. Graham's law
C. \(\frac { V }{ T } =constant\)	3. Ideal gas
D. PV=nRt	4. Charles' law

(a)

A	B	C	D
1	2	3	4

(b)

A	B	C	D
4	3	2	1

(c)

A	B	C	D
2	1	4	3

(d)

A	B	C	D
1	3	4	2

47.

Match the list I with List II and select the correct answer using. the code given below the lists.

List I		List II
A	H₂O₂	1	SiH₄
B	D₂O	2	PdH
C	Metallic hydride	3	Bleach
D	Molecular hydride	4	Study of reaction mechanism

(a)

A	B	C	D
1	3	2	4

(b)

A	B	C	D
4	3	1	2

(c)

A	B	C	D
3	4	2	1

(d)

A	B	C	D
2	1	4	3

48.

Match the list I with List II and select the correct answer using. the code given below the lists.

List I		List II
A	Metalloid	1	Cerium
B	Noble gas	2	Nobelium
C	Trans uranium element	3	Arsenic
D	Lanthanide	4	Argon

(a)

A	B	C	D
1	3	2	4

(b)

A	B	C	D
4	2	1	3

(c)

A	B	C	D
3	4	2	1

(d)

A	B	C	D
2	1	4	3

49.

Spodumene is the silicate mineral of _____

(a)

lithium

(b)

sodium

(c)

cesium

(d)

francium

50.

If the volume of a fixed mass of a gas is reduced to half at constant temperature, the gas pressure _____________

(a)

remains constant

(b)

doubles

(c)

reduces to half

(d)

becomes zero

51.

The atomic weight of Au is ______

(a)

195

(b)

197

(c)

198

(d)

196

52.

The values of ΔH and ΔS for a reaction are respectively 30 kJ mol^-1 and 100 JK^-1 mol^-1. Then the temperature above which the reaction will become spontaneous is ______________

(a)

300 K

(b)

30 K

(c)

100 K

(d)

200 C

53.

In an isothermal reversible compression of an ideal gas the sign of q, ΔS and w are respectively _______________

(a)

+, -, -

(b)

-, +, -

(c)

+, -, +

(d)

-, -, +

54.

Period of an element is represented by _____ quantum number

(a)

Principal

(b)

Azimuthal

(c)

Magnetic

(d)

Spin

55.

Given that C_(g)+ O_2(g)⟶ CO_2(g)ΔH^o =-akJ; 2CO_(g)+O_2(g) ⟶ 2CO_2(g)ΔH^o= -bkJ; Calculate the AHo for the reaction C_(g)+ 1/2O_2(g)⟶ CO_(g) ______________

(a)

\(\frac{b+2a}{2}\)

(b)

2a-b

(c)

\(\frac{2a-b}{2}\)

(d)

\(\frac{b-2a}{2}\)

56.

The heat of formation of CO and CO₂ are - 26.4 kcal and - 94 kcal, respectively. Heat of combustion of carbon monoxide will be ____________

(a)

+ 26.4 kcal

(b)

- 67.6 kcal

(c)

- 120.6 kcal

(d)

+ 52.8 kcal

57.

An ideal gas expands from the volume of 1 x 10^-3 m³to 1 x 10^-2m³ at 300 K against a constant pressure at 1 x 10⁵ Nm^-2. The work done is ______________

(a)

- 900 J

(b)

900 kJ

(c)

270 kJ

(d)

-900 kJ

58.

In an adiabatic process, which of the following is true ?

(a)

q = w

(b)

q = 0

(c)

ΔE = q

(d)

PΔV= 0

59.

Maximum oxidation state is present in the central metal atom of which compound

(a)

CrO₂Cl₂

(b)

MnO₂

(c)

[Fe(CN)₆]^3-

(d)

MnO

60.

Among the following the least thermally stable is ___________

(a)

K₂CO₃

(b)

Na₂CO₃

(c)

BaCO₃

(d)

Li₂CO₃

61.

When CaC₂ is heated in atmospheric nitrogen in an electric furnace the compound formed is ___________

(a)

Ca(CN)₂

(b)

CaNCN

(c)

CaC₂N₂

(d)

CaNC₂

62.

Which of the following does not represent the mathematical expression for the Heisenberg uncertainty principle?

(a)

\(\triangle x.\triangle p\ge \frac { h }{ 4\pi } \)

(b)

\(\triangle x.\triangle v\ge \frac { h }{ 4\pi m } \)

(c)

\(\triangle E.\triangle t\ge \frac { h }{ 4\pi } \)

(d)

\(\triangle E.\triangle x\ge \frac { h }{ 4\pi } \)

63.

A macroscopic particle of mass 100 g and moving at a velocity of 100 cm S^-1will have a de Broglie wavelength of ___________

(a)

6.6 x 10^-29 cm

(b)

6.6 x 10^-30 cm

(c)

6.6 x 10^-31 cm

(d)

6.6 x 10^-32 cm

64.

The compound (X) on heating gives a colourless gas and a residue that is dissolved in water to obtain (B). Excess of CO₂ is bubbled through aqueous solution of B, C is formed. Solid (C) on heating gives back X.(B) is ____________

(a)

CaCO₃

(b)

Ca(OH)₂

(c)

Na₂CO₃

(d)

NaHCO₃

65.

RbO₂ is _____________

(a)

superoxide and paramagnetic

(b)

peroxide and diamagnetic

(c)

superoxide and diamagnetic

(d)

peroxide and paramagnetic

66.

Which of the following compounds will not evolve H₂ gas on reaction with alkali metals ?

(a)

ethanoic acid

(b)

ethanol

(c)

phenol

(d)

none of these

67.

Equal moles of hydrogen and oxygen gases are placed in a container, with a pin-hole through which both can escape what fraction of oxygen escapes in the time required for one-half of the hydrogen to escape.

(a)

\(\frac { 3 }{ 8 } \)

(b)

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

(c)

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

(d)

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

68.

If temperature and volume of an ideal gas is increased to twice its values, the initial pressure P becomes _________

(a)

(b)

(c)

(d)

69.

The table indicates the value of van der Waals constant 'a' in (dm³)² atm. mol^-2.

Gas	O₂	N₂	NH₃	CH₄
a	1.360	1.390	4.170	2.253

The gas which can be most easily liquefied is ______________

(a)

O₂

(b)

N₂

(c)

NH₃

(d)

CH₄

70.

Which one of the following is used as a standard for atomic mass?

(a)

₆C¹²

(b)

₇C¹²

(c)

₆C¹³

(d)

₆C¹⁴

71.

Which of the following contain same number of carbon atoms as in 6 g of carbon-12 ?

(a)

7.5 g ethane

(b)

8 g methane

(c)

both (a) and (b)

(d)

none of these

72.

The mass of a gas that occupies a volume of 612.5 ml at room temperature and pressure (25⁰ c and 1 atm pressure) is 1.1g. The molar mass of the gas is _______.

(a)

66.25 g mol^-1

(b)

44 g mol^-1

(c)

24.5 g mol^-1

(d)

662.5 g mol^-1

73.

What is the mass of precipitate formed when 50 ml of 8.5 % solution of AgNO₃ is mixed with 100 ml of 1.865 % potassium chloride solution ?

(a)

3.59 g

(b)

(c)

14 g

(d)

28 g

74.

Two 22.4 litre containers A and B contains 8 g of O₂ and 8 g of SO₂ respectively at 273 K and 1 atm pressure, then ______.

(a)

Number of molecules in A and B are same

(b)

Number of molecules in B is more than that in A.

(c)

The ratio between the number of molecules in A= to number of molecules in B is 2:1

(d)

Number of molecules in B is three times greater than the number of molecules in A

75.

If uncertainty in position and momentum are equal, then minimum uncertainty in velocity is _________

(a)

\(\frac { 1 }{ m } \sqrt { \frac { h }{ \pi } } \)

(b)

\( \sqrt { \frac { h }{ \pi } } \)

(c)

\(\frac { 1 }{ 2m } \sqrt { \frac { h }{ \pi } } \)

(d)

\( { \frac { h }{4\pi } } \)

76.

Electron density in the yz plane of 3d_xy orbital is ___________

(a)

zero

(b)

0.50

(c)

0.75

(d)

0.90

77.

How many electrons in an atom with atomic number 105 can have (n + 1) = 8 ?

(a)

(b)

(c)

(d)

unpredictable

78.

The total number of orbitals associated with the principal quantum number n = 3 is _________

(a)

(b)

(c)

(d)

79.

What is the maximum numbers of electrons that can be associated with the following set of quantum numbers? n = 3, I = 1 and m =-1

(a)

(b)

(c)

(d)

= 10

80.

Which of the following statement(s) is/are not true about the following decomposition reaction.
2KClO₃ \(\longrightarrow\) 2KCl + 3O₂
(i) Potassium is undergoing oxidation
(ii) Chlorine is undergoing oxidation
(iii) Oxygen is reduced
(iv) None of the species are undergoing oxidation and reduction.

(a)

only (iv)

(b)

(i) and (iv)

(c)

(iv) and (iii)

(d)

All of these

81.

Identify disproportionation reaction

(a)

CH₄ + 2O₂ \(\longrightarrow\) CO₂+ 2H₂O

(b)

CH₄ + 4Cl₂ \(\longrightarrow\) CCl₄ + 4HCI

(c)

2F₂+ 2OH \(\longrightarrow\) 2F^-+ OF₂+ H₂O

(d)

2NO₂ + 2OH^- \(\longrightarrow\) NO^-₂ + NO^-₃ + H₂O

82.

The value of universal gas constant depends upon __________

(a)

Temperature of the gas

(b)

Volume of the gas

(c)

Number of moles of the gas

(d)

units of Pressure and volume.

83.

A bottle of ammonia and a bottle of HCI connected through a long tube are opened simultaneously at both ends. The white ammonium chloride ring first formed will be ___________

(a)

At the center of the tube

(b)

Near the hydrogen chloride bottle

(c)

Near the ammonia bottle

(d)

Throughout the length of the tube

84.

The temperatures at which real gases obey the ideal gas laws over a wide range of pressure is called ____________-

(a)

Critical temperature

(b)

Boyle temperature

(c)

Inversion temperature

(d)

Reduced temperature

85.

Total number of electrons present in 1.7 g of ammonia is _____.

(a)

6.022\(\times\)10²³

(b)

\(\frac { 6.022\times { 10 }^{ 22 } }{ 1.7 } \quad \)

(c)

\(\frac { 6.022\times { 10 }^{ 24 } }{ 1.7 } \)

(d)

\(\frac { 6.022\times { 10 }^{ 23 } }{ 1.7 } \)

86.

Shape of an orbital is given by ____________

(a)

Principal quantum number

(b)

Spin quantum number

(c)

Azimuthal quantum number

(d)

Magnetic quantum number

87.

Two electrons occupying the same orbital are distinguished by ___________

(a)

azimuthal quantum number

(b)

spin quantum number

(c)

magnetic quantum number

(d)

orbital quantum number

88.

Based on equation E = \(-2.178\times { 10 }^{ -18 }J\left( \frac { { Z }^{ 2 } }{ { n }^{ 2 } } \right) \)certain conclusions are written. Which of them is not correct?

(a)

Equation can be used to calculate the change in energy when the electron changes orbit

(b)

For n = 1, the electron has a more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit

(c)

The negative sign in equation simply means that the energy of electron bound to the nucleus is lower than it would be if the electrons were at the infinite distance from the nucleus.

(d)

Larger the value of n, the larger is the orbit radius.

89.

Water is a ___________

(a)

basic oxide

(b)

acidic oxide

(c)

amphoteric oxide

(d)

none of these

90.

The reaction H₃PO₂ + D₂O ➝ H₂DPO₂ + HDO indicates that hypo-phosphorus acid is _____________

(a)

tribasic acid

(b)

dibasic acid

(c)

mono basic acid

(d)

none of these

91.

The cause of permanent hardness of water is due to _____________

(a)

Ca(HCO₃)₂

(b)

Mg(HCO₃)₂

(c)

CaCl₂

(d)

MgCO₃

92.

The hardness of water can be determined by volumetrically using the reagent _____________

(a)

sodium thio sulphate

(b)

potassium permanganate

(c)

hydrogen peroxide

(d)

EDTA

93.

Non-stoichiometric hydrides are formed by _____________

(a)

palladium, vanadium

(b)

carbon, nickel

(c)

manganese, lithium

(d)

nitrogen, chlorine

94.

Tritium nucleus contains _____________

(a)

1 p+0 n

(b)

2 p+1 n

(c)

1 p + 2 n

(d)

none of these

95.

Which one of the following statements is incorrect with regard to ortho and para dihydrogen ?

(a)

They are nuclear spin isomers

(b)

Ortho isomer has zero nuclear spin whereas the para isomer has one nuclear spin

(c)

The para isomer is favoured at low temperatures

(d)

The thermal conductivity of the para isomer is 50% greater than that of the ortho isomer

96.

Water gas is _____.

(a)

H₂O_(g)

(b)

CO + H₂O

(c)

CO + H₂

(d)

CO + N₂

97.

The equivalent mass of a trivalent metal element is 9 g eq^-1 the molar mass of its anhydrous oxide is _____.

(a)

102 g

(b)

27 g

(c)

270 g

(d)

78 g

98.

An element X has the following isotopic Composition ²⁰⁰X = 90%, ¹⁹⁹X = 8% and ²⁰²X=2%.The Weighted average atomic mass of the element X is closest to _________.

(a)

201 u

(b)

202 u

(c)

199 u

(d)

200 u

Assertion and reason

2 x 2 = 4

99.

Assertion: The ash produced by burning paper in air is lighter than the original mass of paper.
Reason: he residue left after combustion of a chemical entity is always lighter
Codes:
(a) Both assertion and reason are correct and reason is the correct explanation for assertion.
(b) Both assertion and reason are correct but reason is not the correct explanation for assertion
(c) Assertion is true but reason is false.
(d) Both assertion and reason is false.

(a)

Both assertion and reason are correct and reason is the correct explanation for assertion.

(b)

Both assertion and reason are correct but reason is not the correct explanation for assertion

(c)

Assertion is true but reason are false

(d)

Both assertion and reason are false

100.

Assertion : BeSO₄ is soluble in water while BaSO₄ is not
Reason : Hydration energy decreases down the group from Be to Ba and lattice energy remains almost constant.
(a) both assertion and reason are true and reason is the correct explanation of assertion
(b) both assertion and reason are true but reason is not the correct explanation of assertion
(c) both assertion and reason are false.
(d) Both assertion and reason are false

(a)

both assertion and reason are true and reason is the correct explanation of assertion

(b)

both assertion and reason are true but reason is not the correct explanation of assertion

(c)

assertion is true but reason is false

(d)

both assertion and reason are false.

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Answers Key:

Multiple Choice Question

98 x 1 = 98

(d)
Be and Al

(d)
None of these

(a)
Amongst the isoelectronic species, smaller the positive charge on cation, smaller is the ionic radius

(a)
Both assertion and reason are true and reason is the correct explanation of assertion.

(b)
decreases

10.

(d)
Cs

11.

(a)
Beryllium

12.

13.

14.

15.

(b)
barometer

16.

17.

(b)
Its tendency to gain an electron to attain stable electronic configuration.

18.

(b)
The electron may be in 4d orbital

19.

20.

(d)
\(\lambda ={h\over mv}\)

21.

22.

23.

(a)
Ag, Au, Pt

24.

(b)
-2.7 Kcal

25.

(b)
[Xe]4f⁷5d¹6s²

26.

(b)
400K

27.

(d)
\(\Delta\)S

28.

29.

30.

(b)
CaO

31.

(d)
CH₄

32.

(b)
The inter nuclear distances between the two bonded atoms are different in all the isotopes.

33.

34.

(a)
It is zero for reversible reaction

35.

(b)
ΔS<0

36.

(b)
prevent of rusting of iron ships

37.

(a)
CaSO₄

38.

(d)
Work

39.

40.

41.

(b)
electronegativity

42.

43.

(a)
One

44.

(d)
Z = 3, Z = 11

45.

(b)
High temperature and low pressure

46.

47.

48.

49.

(a)
lithium

50.

(b)
doubles

51.

(b)
197

52.

(a)
300 K

53.

(d)
-, -, +

54.

(a)
Principal

55.

(d)
\(\frac{b-2a}{2}\)

56.

(b)
- 67.6 kcal

57.

(a)
- 900 J

58.

(b)
q = 0

59.

(a)
CrO₂Cl₂

60.

(d)
Li₂CO₃

61.

(b)
CaNCN

62.

(d)
\(\triangle E.\triangle x\ge \frac { h }{ 4\pi } \)

63.

64.

(b)
Ca(OH)₂

65.

(a)
superoxide and paramagnetic

66.

(d)
none of these

67.

68.

69.

70.

(a)
₆C¹²

71.

72.

(b)
44 g mol^-1

73.

(a)
3.59 g

74.

75.

76.

(a)
zero

77.

(b)
17

78.

(a)
9

79.

80.

(b)
(i) and (iv)

81.

(d)
2NO₂ + 2OH^- \(\longrightarrow\) NO^-₂ + NO^-₃ + H₂O

82.

(d)
units of Pressure and volume.

83.

(b)
Near the hydrogen chloride bottle

84.

(b)
Boyle temperature

85.

(a)
6.022\(\times\)10²³

86.

87.

(b)
spin quantum number

88.

(b)
For n = 1, the electron has a more negative energy than it does for n = 6 which means that the electron is more loosely bound in the smallest allowed orbit

89.

90.

91.

92.