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)

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

Identify the correct statement(s) with respect to the following reaction :
Zn + 2HCl \(\longrightarrow\) ZnCl₂ + H₂
(i) Zinc is acting as an oxidant
(ii) Chlorine is acting as a reductant
(iii) Hydrogen is not acting as an oxidant
(iv) Zn is acting as a reductant

(a)

only (ii)

(b)

only (iv)

(c)

both (ii) and (iii)

(d)

both (ii) and (i)

Which one of the following is the standard for atomic mass?

(a)

₁H¹

(b)

₆C¹²

(c)

₆C¹⁴

(d)

₈O¹⁶

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

(a)

13g

(b)

1 g

(c)

23 g

(d)

1/23g

When methane is burnt in oxygen to produce CO₂ and H₂O, the oxidation number of carbon changes by ____________.

(a)

-8

(b)

+4

(c)

Zero

(d)

+8

For d-electron, the orbital angular momentum is ___________

(a)

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

(b)

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

(c)

\(\frac { \sqrt { 2\times 4 } h }{ 2\pi } \)

(d)

\(\frac { \sqrt { 6 } h }{ 2\pi } \)

Time independent Schnodinger wave equation is ______________

(a)

\(\overset { \wedge }{ H } \psi =E\psi \)

(b)

\({ \triangledown }^{ 2 }\psi +\frac { 8{ \pi }^{ 2 }m }{ { h }^{ 2 } } (E+V)\psi =0\)

(c)

\(\frac { { \partial }^{ 2 }\psi }{ { \partial x }^{ 2 } } +\frac { { \partial }^{ 2 }\psi }{ { \partial y }^{ 2 } } +\frac { { \partial }^{ 2 }\psi }{ { \partial z }^{ 2 } } +\frac { { 2m } }{ { h }^{ 2 } } (E-V)\Psi =0\)

(d)

All of these

Consider the following statements regarding Rutherford's \(\alpha\)-ray scattering experiment.
i. Most of the \(\alpha\)-particles were deflected through a small angle.
ii. Some of \(\alpha\)-particles passed through the foil.
iii. Very few \(\alpha\)-particles were reflected back by 180^o.
Which of the above statements is/are not correct.

(a)

i and ii

(b)

ii and iii

(c)

i and iii

(d)

i, ii and iii

Which of the following is the actual configuration of Cr (Z = 24)?

(a)

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁴ 4s²

(b)

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s¹

(c)

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶

(d)

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s³

Assertion(A): Cr with electronic configuration [Ar] 3d⁵ 4s¹ is more stable than [Ar] 3d⁴ 4s².
Reason(R): Half filled orbitals have been found to have extra stability than partially filled orbitals.
Codes:
(a) A and R are correct and R is the correct explanation of A.
(b) A and R are correct but R is not the correct explanation of A.
(c) A is correct but R is wrong.
(d) A is wrong but R is correct.

(a)

A and R are correct but R is not the correct the explanation of A.

(b)

A is correct but R is wrong.

(c)

A is wrong but R is correct.

(d)

A is wrong but R is correct.

Across the period, Ionisation energy _______

(a)

increases

(b)

decreases

(c)

does not vary

(d)

first decreases and then increases

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)

Ionisation enthalpy is an _____ process.

(a)

exothermic

(b)

endothermic

(c)

reversible

(d)

both (a) and (b)

Among the elements Ca, Mg, P and CI the order of increasing atomic radii is ___________

(a)

Mg < Ca < Cl < P

(b)

Cl < P < Mg < Ca

(c)

p < Cl < Ca < Mg

(d)

Ca < mg < P < Cl

The chemical symbol of carbon and cobalt are______

(a)

Ca and CO

(b)

Ca and Cl

(c)

C and CO

(d)

Cr and Cb

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.

Which one of the following is a universal solvent?

(a)

Alcohol

(b)

Ether

(c)

CCl₄

(d)

Water

Why Cs and K are used as electrodes in photoelectric cells ___________

(a)

Due to their less ionisation energy

(b)

Due to high ionisation energy

(c)

Due to diagonal relationship

(d)

None of these

Consider the reaction where K_P = 0.5 at a particular temperature
PCl₅(g) ⇌ PCl₃ (g) + Cl₂ (g)
if the three gases are mixed in a container so that the partial pressure of each gas is initially 1 atm, then which one of the following is true ____________

(a)

more PCl₃ will be produced

(b)

more Cl₂ will be produced

(c)

more PCl₅ will be produced

(d)

none of these

The Henry's law constant for the solubility of Nitrogen gas in water at 350 K is 8 x 10⁴ atm. The mole fraction of nitrogen in air is 0.5. The number of moles of Nitrogen from air dissolved in 10 moles of water at 350K and 4 atm pressure is ____________

(a)

4 x 10^-4

(b)

4 x 10⁴

(c)

2 x 10^-2

(d)

2.5 x 10^-4

Equimolal aqueous solutions of NaCl and KCl are prepared. If the freezing point of NaCl is –2^oC, the freezing point of KCl solution is expected to be ____________

(a)

-2^oC

(b)

-4^oC

(c)

-1^oC

(d)

0^oC

The ratio of number of sigma (σ) and pi (л) bonds in 2- butynal is __________

(a)

8/3

(b)

5/3

(c)

8/2

(d)

9/2

Hybridisation of central atom in PCl₅ involves the mixing of orbitals __________

(a)

s, p_x, p_y, d_x2 , d_x²-y²

(b)

s, p_x . p_y, p_xy . d_x²-y²

(c)

s, p_x, p_y, p_z, d_x²-y²

(d)

s, p_x, p_y, d_xy, d_x²-y²

Structure of the compound whose IUPAC name is 5,6 - dimethylhept - 2 - ene is ___________

(a)

(b)

(c)

(d)

None of these

C -X bond is strongest in __________

(a)

Chloromethane

(b)

Iodomethane

(c)

Bromomethane

(d)

Fluoromethane