The oxidation state of a element in its uncombined state is

(a)

zero

(b)

+1

(c)

-1

(d)

none

Fe2 + \(\longrightarrow\) Fe³⁺ + e^- is a ________ reaction.

(a)

redox

(b)

reduction

(c)

oxidation

(d)

decomposition

The oxidation number of hydrogen in LiH is _________

(a)

+1

(b)

-1

(c)

+2

(d)

-2

The oxidation number of Cr in Cr₂O₇^2- _______ is

(a)

+6

(b)

-6

(c)

+7

(d)

-7

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

(a)

CrO₂Cl₂

(b)

MnO₂

(c)

[Fe(CN)₆]^3-

(d)

MnO

Identify the redox reaction taking place in a beaker.

(a)

Zn_(s)+ Cu²⁺_(aq) \(\longrightarrow\) Zn²⁺_(aq) + Cu_(s)

(b)

Cu_(s) + 2Ag⁺_(aq) \(\longrightarrow\) Cu²⁺_(aq) + 2Ag_(s)

(c)

Cu_(s) + Zn²⁺_(aq) \(\longrightarrow\) Zn_(s) + cu²⁺ _(aq)

(d)

2Ag_(s) + cu²⁺_(aq) \(\longrightarrow\) 2Ag⁺_aq + Cu_(s)

The characteristic feature of orderly arrangement of molecules belongs to ______________.

(a)

Solids

(b)

Liquid

(c)

Gases

(d)

None of these

12 g of carbon-12 contains_____carbon atoms

(a)

6.022\(\times\)10²³

(b)

6

(c)

12

(d)

12.022\(\times\)10^-23 kg

One mole of Sulphuric acid contains _______oxygen atoms

(a)

4 x 10²³

(b)

4 x 6.023 x 10^-23

(c)

4 x 6.023 x 10²³

(d)

4 x 6.023 x 10³²

The empirical formula and molecular mass of a compound are CH₂O and 180g respectively. What will be the molecular formula of the compound?

(a)

C₉H₁₉0

(b)

CH₂O

(c)

C₆H₁₂O₆

(d)

C₂H₄O₂

Give an example of molecule in which the ratio of the molecular formula is six times the empirical formula.

(a)

C₆H₁₂O₆

(b)

CH₂O

(c)

CH₄

(d)

NA₂CO₃

10g of hydrogen and 64g of oxygen were filled in a steel vessel and exploded. The amount of water produced in this reaction will be ________

(a)

3mol

(b)

4mol

(c)

1mol

(d)

2mol

The value of Avogadro Number N is equal to ___________.

(a)

2.24 x 10^-2L

(b)

22400 cm^-3

(c)

6.023 x 10^-23

(d)

6.023 x 10²³

Identify the compound formed during the rusting of iron

(a)

Fe₂O₃

(b)

Fe₂O₃.xH₂O

(c)

FeO.xH₂O

(d)

FeO

The molar mass of Na₂SO₄ is ___________.

(a)

129

(b)

142

(c)

110

(d)

70

Shape of an orbital is given by ____________

(a)

Principal quantum number

(b)

Spin quantum number

(c)

Azimuthal quantum number

(d)

Magnetic quantum number

Which of the following has maximum number of unpaired d-electrons?

(a)

N³⁺

(b)

Fe²⁺

(c)

Zn⁺

(d)

Cu⁺

In Rutherford's gold foil experiment, a thin gold foil was bombarded with a stream of fast moving ___________

(a)

B particles

(b)

\(\alpha\)-particles

(c)

\(\gamma\) particles

(d)

\(\delta\) particles

How many neutrons and protons respectively are present  in the ₆C¹³ nuclei?

(a)

6, 13

(b)

6, 7

(c)

13,6

(d)

7,6

Name the element whose isotope has mass number 14 and 8 neutrons.

(a)

Carbon

(b)

Nitrogen

(c)

Oxygen

(d)

Fluorine

Neutrons was discovered by ________

(a)

Rutherford

(b)

Chadwick

(c)

Bohr

(d)

Thomson

If E_n = -313.6/n2,If the value of E_i = -34.84 to which value 'n' corresponds __________

(a)

4

(b)

3

(c)

2

(d)

1

The energy of electron in an atom is given by En =

(a)

\(\frac { 4{ \pi }^{ 2 }{ me }^{ 4 } }{ { n }^{ 2 }h^{ 2 } } \)

(b)

\(\frac { 2{ \pi }^{ 2 }{ me }^{ 4 } }{ { n }^{ 2 }h^{ 2 } } \)

(c)

\(\frac { 2{ \pi }^{ 2 }{ me }^{ 4 } }{ { n }^{ 2 }h^{ 2 } } \)

(d)

\(\frac { 2{ \pi }{ me }^{ 4 } }{ { n }^{ 2 }h^{ 2 } } \)

Maximum number of electrons in a subshell of an atom is determined by the following

(a)

2l + 1

(b)

4l - 2

(c)

2n²

(d)

4l + 2

What will be the wavelength of a ball of mass 0.1 kg moving with a velocity of 10ms^-1?

(a)

6.62 \(\times\) 10^-34m

(b)

6.626 \(\times\) 10³⁴m

(c)

6.626 \(\times\) 10^-34m

(d)

6.626 \(\times\) 10³⁴m

The velocity of light is 3 x 10⁸ ms^-1. The wave length of violet radiation is 400 nm. The wavelength in frequency (Hz) is:

(a)

7.5 x 10¹⁴ Hz

(b)

7.5 x 10¹⁵ Hz

(c)

7.5 x 10¹³ Hz

(d)

7.5 x 10¹⁶ Hz

For a principle quantum number n = 4, the total number of orbitals having l = 3 is:

(a)

3

(b)

7

(c)

5

(d)

9

The orbital diagram in which both the Pauli's exclusion principle and Hund's rule are violated is __________

(a)

(b)

(c)

(d)

Which of the following has the largest wavelength, provided all have equal velocity?

(a)

carbon di oxide molecule

(b)

electron

(c)

ammonia molecule

(d)

proton

Identify the quantum number for 4d_x²-y².electron ____________

(a)

\(4,2,-2,+\frac{1}{2}\)

(b)

\(4,0,0,+\frac{1}{2}\)

(c)

\(4,3,2,+\frac{1}{2}\)

(d)

\(4,3,2,-\frac{1}{2}\)

The value of n, I, m and s of 8^th electron in an oxygen atom are respectively____________.

(a)

\(1,0,0,+\frac{1}{2}\)

(b)

\(2,1,+1,-\frac{1}{2}\)

(c)

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

(d)

\(2,1,0,+\frac{1}{2}\)

The Bohr's radius of Li²⁺ of 2^nd orbit is ________________

(a)

0.529 \(\mathring{A}\)

(b)

0.0753\(\mathring{A}\)

(c)

0.7053\(\mathring{A}\)

(d)

0.0529\(\mathring{A}\)

What are the values of n, I, m and s for 3p_x electron?

(a)

3,2,1,0

(b)

3,1,-1,+1/2

(c)

3,2,+1,-1/2

(d)

3,0,0,+1/2

The first list of 23 chemical elements was published by _____ in the year 1789.

(a)

Berzelius

(b)

Dobereiner

(c)

Lavoisier

(d)

John Dalton

Which of the following is Dobereiner's triad?

(a)

Ne,Ca,Na

(b)

H₂, N₂, O₂

(c)

Li, Na, K

(d)

Na, Br, K

The atomic weight of Au is ______

(a)

195

(b)

197

(c)

198

(d)

196

Find the incorrect statement.

(a)

Smallest atom of periodic table is He

(b)

p-block elements are metals, nonmetals and metalloids

(c)

Noble gases have 8 valence electrons except He

(d)

Valence electron and valency is same for group I

The general electronic configuration of d-block element is _____

(a)

ns²np⁶

(b)

(n-1) d^1-10 ns^0-2

(c)

(n-1) d¹ ns^0-2

(d)

(n-1) d^0-10 ns²

With respect to chlorine, hydrogen will be __________

(a)

Electropositive

(b)

Electronegative

(c)

Neutral

(d)

None of these

Which of the following processes involves absorption of energy?

(a)

Cl_(g) +e^- ⟶ Cl^-

(b)

O^-_(g) +e^- ⟶ O^2-

(c)

O_(g) +e^- ⟶ O_(g)^-

(d)

S_(g)+e^- ⟶ S^-_(g)

The increasing order of the first ionisation enthalpy of the elements B, P, Sand F (lowest first) is __________

(a)

B

(b)

B < S < P < F

(c)

F < S < P < B

(d)

P< S

Which period contain 32 elements?

(a)

Period 1

(b)

Period 4

(c)

Period 5

(d)

Period 6

Which one of the following is not an isoelectronic ion?

(a)

Al³⁺

(b)

N^3-

(c)

Mg²⁺

(d)

K⁺

Which of the following pair is not diagonally related?

(a)

Li, Mg

(b)

Li, Na

(c)

Be, Al

(d)

B, Si

The order of screening effect of electron of s, p, d and f orbits of a given shell of an atom on its outershell electrons is ___________

(a)

s > p > d> f

(b)

f>d>p>s

(c)

P>d>s>f

(d)

f>p>s>d

The number of neutrons in  hydrogen atom is ___________.

(a)

three

(b)

two

(c)

one

(d)

zero

The half life period of Tritium is ___________

(a)

12.33 secs

(b)

12.33 mins

(c)

12.33 hrs

(d)

12.33 years

Ortho and para hydrogen differ in _____________

(a)

proton spin

(b)

electron spin

(c)

nuclear charge

(d)

both b and c

FeSO₄ contains _________ molecules of water of hydration.

(a)

5

(b)

7

(c)

10

(d)

12

H₂O₂ is a ________ acid.

(a)

mono basic

(b)

di basic

(c)

tri basic

(d)

none

The element which does not contain a neutron is _____________

(a)

hydrogen

(b)

helium

(c)

chlorine

(d)

none of the above

Which of the following is used in illumination of wrist watches?

(a)

Phosphorous

(b)

Radon

(c)

Tritium

(d)

Deuterium

Which of the following can effectively remove all types of hardness of water?

(a)

Soap

(b)

Slaked lime

(c)

Washing soda

(d)

Zeolite

The elements that belong to group 1 of the periodic table are called as _________

(a)

alkali metals

(b)

alkaline earth metals

(c)

chalcogens

(d)

rare gases

Which of the following is used in photoelectric cells?

(a)

Na

(b)

K

(c)

Li

(d)

Cs

Which of the following metals is most commonly used in photochemical cells?

(a)

Lithium

(b)

Calcium

(c)

Caesium

(d)

Francium

Identify the most stable hydride among the following ____________

(a)

NaH

(b)

LiH

(c)

KH

(d)

CsH

Alkaline earth metals exhibit ______ oxidation state in their compounds

(a)

+1

(b)

+2

(c)

+4

(d)

+6

The element that does not answer the flame test is _________

(a)

Ba

(b)

Mg

(c)

Ca

(d)

Sr

Plaster of Paris is______

(a)

CaSO₄.H₂O

(b)

CaSO₄.1/2H₂O

(c)

CaSO₄.1/4H₂O

(d)

CaSO₄.2H₂O

Dead burnt plaster is ________

(a)

CaSO₄

(b)

CaSO₄·1/2H₂0

(c)

CaSO₄.H₂O

(d)

CaSO₄.2H₂0

Which is insoluble in water?

(a)

CaF₂

(b)

CaCI

(c)

HgCl₂

(d)

Ca(NO₃)₂

Quick lime is ________

(a)

CaCO₃

(b)

CaO

(c)

CaSO₄.2H₂O

(d)

Ca(OH)₂

The general electronic configuration of alkali metals is ____________

(a)

[noble gas] ns²

(b)

[noble gas] ns¹

(c)

ns² np⁶

(d)

ns² (n-1)d^1-10

The second ionization enthalpy of alkali metals is ________

(a)

Zero

(b)

low

(c)

high

(d)

very low

Which of the following ions are more responsible for transmission of nerve signal?

(a)

Li⁺

(b)

RB⁺

(c)

Cs⁺

(d)

K⁺

Which one of the following is used to build the beam pipe in accelerators?

(a)

Be

(b)

Ca

(c)

Mg

(d)

Sr

Which is used to treat upset stomach and eczema?

(a)

MgSO₄·7H₂O

(b)

FeSO₄·7H₂O

(c)

CaSO₄.2H₂O

(d)

2CaSO₄.H₂O

Which of the following is not a peroxide?

(a)

KO₂

(b)

CrO₅

(c)

Na₂O₂

(d)

BaO₂

Value of gas constant R is ____________

(a)

0.082dm³atm

(b)

0.987 cal mol^-1 K^-1

(c)

8.3 J mol^-1 K^-1

(d)

8 er mol^-1 K^-1

The absolute zero is _____________

(a)

-273^oC

(b)

273^oC

(c)

OK

(d)

both a and c

Compression factor Z is given by _____________

(a)

PV/nRT

(b)

P/nRT

(c)

PV/R

(d)

PV/T

What is the correct increasing order of liquefiability of the gas?

(a)

H₂ < CO₂ < CH₄ < N₂

(b)

H₂ < N₂ < CH₄ < CO₂

(c)

CO₂ < CH₄ < H₂ < N₂

(d)

CO₂ < CH₄ < N₂ < H₂

Maximum deviations from ideal gas is expected from ___________

(a)

H₂(g)

(b)

N₂(g)

(c)

CH₄(g)

(d)

NH₃(g)

A fundamental goal of thermodynamics is the prediction of __________ of the process.

(a)

reversibility

(b)

rate

(c)

spontaneity

(d)

none of these

Internal energy is denoted by the symbol_______

(a)

H

(b)

S

(c)

G

(d)

U

The SI unit of entropy is ______

(a)

JK

(b)

JK^-1

(c)

KJ K^-1

(d)

KJ / mole

Which of the following will have highest \(\Delta\)H_vap value?

(a)

Acetone

(b)

Ethanol

(c)

Carbon tetrachloride

(d)

Chloroform

Enthalpy change for the reaction, 4H (g) \(\rightarrow\) 2H₂ (g) is - 869.6 kJ. The dissociation energy of H - H bond is _________

(a)

-217.4 kJ

(b)

-434.8 kJ

(c)

- 896.6 kJ

(d)

+ 434.8 kJ

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

Mathematically, the third law of thermodynamics is expressed as _______

(a)

\(\overset{\lim}{T\rightarrow 0}{ S=0 } \)

(b)

\(\overset{\lim}{T\rightarrow \infty} {S=1 } \).

(c)

ΔU = q + w

(d)

G = H - TS

Le-Chatelier's principle is not applicable to _____________

(a)

\({ F }e_{ \left( g \right) }+{ S }_{ \left( s \right) }\rightleftharpoons { FeS }_{ \left( s \right) }\) 

(b)

\({ H }_{ 2\left( g \right) }+{ I }_{ 2\left( g \right) }\rightleftharpoons { 2HI }_{ \left( g \right) }\)

(c)

\(x = {-b \pm \sqrt{b^2-4ac} \over 2a}\)

(d)

\({ N }_{ 2\left( g \right) }+3H_{ 2\left( g \right) }\rightleftharpoons { 2NN }_{ 3\left( g \right) }\)

For the reaction,\(CaC{ O }_{ 3\left( s \right) }\rightleftharpoons { CaO }_{ \left( s \right) }+{ CO }_{ 2\left( g \right) }\) K_p is equal to __________

(a)

K_c

(b)

K_cRT

(c)

K_c(RT)²

(d)

K_c(RT)^-

For the system \(3A+2B\rightleftharpoons C\) , the expression for equilibrium constant K is __________

(a)

\(\cfrac { \left[ 3A \right] \times \left[ 2B \right] }{ \left[ C \right] } \)

(b)

\(\cfrac { { \left[ A \right] }^{ 3 }\times \left[ B \right] }{ \left[ C \right] } \)

(c)

\(\cfrac { \left[ C \right] }{ { \left[ A \right] }^{ 3 }\times { \left[ B \right] }^{ 2 } } \)

(d)

\(\cfrac { \left[ C \right] }{ { \left[ 3A \right] }\times { \left[ 2B \right] } } \)

For the homogeneous gas reaction at 600K \(4NH_{ 3\left( g \right) }+5{ O }_{ 2\left( g \right) }\rightleftharpoons 4NO_{ \left( g \right) }+6{ H }_{ 2 }{ O }_{ \left( g \right) }\) The unit of equilibrium constant K" is

(a)

(mol dm^-3)^-1

(b)

(mol dm^-3)

(c)

(mol dm^-3)¹⁰

(d)

(mol dm-³)⁹

In a binary solution __________

(a)

solvent may be liquid

(b)

solvent may be solid

(c)

solute may be gas

(d)

any of these

For associative solutes ____________

(a)

i < 1 and a < 1

(b)

i > 1 and a >. 1

(c)

i < 1 and a < 1

(d)

i > 1 and a < 1

Which of the following has maximum freezing point?

(a)

Pure H₂0

(b)

0.1 M NaCl (aq)

(c)

0.01 M NaCl (aq)

(d)

0.5 M NaCl (aq)

Two liquids having vapour pressures \({ p }_{ 1 }^{ 0 }\) and \({ p }_{ 2 }^{ 0 }\) in pure state in the ratio of 2 : 1 are mixed in the molar ratio of 1 : 2. The ratio of their moles in the vapour state would be __________

(a)

1: 1

(b)

1: 2

(c)

2: 1

(d)

3: 2

The relationship between the values of osmotic pressure of 0.1 M solutions. of KNO₃ (P₁) and CH₃COOH(P₂) is ___________

(a)

P₁ > P₂

(b)

P₂ > P₁

(c)

P₁ = P₂

(d)

\(\frac { { P }_{ 1 } }{ { P }_{ 1 }+{ P }_{ 2 } } =\frac { { P }_{ 2 } }{ { P }_{ 1 }+2{ P }_{ 2 } } \)

Which of the following molecule has no dative bond?

(a)

CO

(b)

\({ SO }_{ 4 }^{ 2- }\)

(c)

\({ CO }_{ 3 }^{ 2- }\)

(d)

None of these

Which among the following molecule obeys octet rule?

(a)

NO

(b)

NO₂

(c)

N₂O₃

(d)

ClO₂

The correct order of increasing bond angles in the following triatomic species is ____________

(a)

\({ NO }_{ 2 }^{ + }\)< NO₂ <\({ NO }_{ 2 }^{ - }\)

(b)

\({ NO }_{ 2 }^{ - }\)< NO₂ <\({ NO }_{ 2 }^{ + }\)

(c)

\({ NO }_{ 2 }^{ - }\)<\({ NO }_{ 2 }^{ + }\)< NO₂

(d)

\({ NO }_{ 2 }^{ + }\)< \({ NO }_{ 2 }^{ - }\)2

Identify the pair of species that possess same bond order.

(a)

\(O_{ 2 }^{ 2- }\), B₂

(b)

NO, CO

(c)

N₂,O₂

(d)

He₂, H₂

Which among the following cannot be formed?

(a)

H₂

(b)

He₂

(c)

N₂

(d)

O₂

In which of the following compound has only one type of hybridised carbon atom?

(a)

(b)

(c)

(d)

All of these

The most stable carbocation is ____________

(a)

\(C{ H }_{ 3 }-\overset { + }{ C } { H }_{ 2 }\)

(b)

\(C{ H }_{ 3 }-\overset { + }{ C } H-C{ H }_{ 3 }\)

(c)

\(C{ H }_{ 2 }=CH-\overset { + }{ C } { H }_{ 2 }\)

(d)

\(\overset { + }{ C } { H }_{ 3 }\)

Chloropicrin is prepared by adding nitric acid to______________,

(a)

CCl₄

(b)

CH₃CI

(c)

CH₃CI₃

(d)

None

Cause of eutrophication is ____________

(a)

Increase of oxygen in water bodies

(b)

Increase in number of aquatic organisms

(c)

Nutrient enrichment of water bodies

(d)

All ofthese