Electronic configuration of H⁺ is

• 1s⁰

• 1s¹

• 1s²

• 1s¹, 2s¹

2.

From the given sets of quantum numbers, the one that is inconsistent with the theory is

• n =3; l =2; m = -3; s = +$\frac{1}{2}$

• n = 4; l = 3; m = 3; s = +$\frac{1}{2}$

• n = 2; l = 1; m = 0; s = -$\frac{1}{2}$

• n = 4; l = 3; m = 2; s = +$\frac{1}{2}$

Pick out the isoelectronic structures from the following

$\underset{\mathrm{I}}{{\mathrm{CH}}_3^{+}} \underset{\mathrm{II}}{{\mathrm{H}}_3{\mathrm{O}}^{+}} \underset{\mathrm{III}}{{\mathrm{NH}}_3} \underset{\mathrm{IV}}{{\mathrm{CH}}_3^{-}}$

• I and II

• I and IV

• I and III

• II, III and IV

Which of the following species is paramagnetic?

• CN^-

• NO

• O${}_2^{2-}$

• CO

XeF₄ has a shape of

• spherical

• trigonal bipyramidal

• square planar

• tetrahedral

1f 20 mL of 0.4 N NaOH solution completely neutralises 40 mL of a dibasic acid, the molarity of the acid solution is

• 0.1 M

• 0.2 M

• 0.3 M

• 0.4 M

Molality of a solution is equal to

• $\frac{\mathrm{number} \mathrm{of} \mathrm{moles} \mathrm{of} \mathrm{solute}}{\mathrm{number} \mathrm{of} \mathrm{litres} \mathrm{of} \mathrm{solution}}$

• $\frac{\mathrm{number} \mathrm{of} \mathrm{g}-\mathrm{equivalents} \mathrm{of} \mathrm{solute}}{\mathrm{number} \mathrm{of} \mathrm{litres} \mathrm{of} \mathrm{solution}}$

• $\frac{\mathrm{number} \mathrm{of} \mathrm{moles} \mathrm{of} \mathrm{solute}}{\mathrm{number} \mathrm{of} \mathrm{kilogram} \mathrm{of} \mathrm{solvent}}$

• $\frac{\mathrm{number} \mathrm{of} \mathrm{moles} \mathrm{of} \mathrm{a} \mathrm{component}}{\mathrm{total} \mathrm{number} \mathrm{of} \mathrm{moles} \mathrm{of} \mathrm{all} \mathrm{components}}$

In the following particle

₃Li⁶ + ? → ₂He⁴ + ₁H³

the missing particle is

• electron

• neutron

• proton

• deuteron

Consider the two gaseous equilibria involving SO₂ and the corresponding equilibrium constants at 298 K

SO₂ (g) + $\frac{1}{2}$O₂ (g) $\rightleftharpoons$ SO₃ (g); K₁

2SO₃ (g) $\rightleftharpoons$ 2SO₂ (g) + O₂ (g); K₂

The values of the equilibrium constants are related by

• K₂ = K₁

• K₂ = K${}_1^2$

• K₂ = $\frac{1}{{\mathrm{K}}_1^2}$

• K₂ = $\frac{1}{{\mathrm{K}}_1}$

For the reaction,

A + B $\rightleftharpoons$ C + D,

the initial concentrations of A and B are equal. The equilibrium concentration of C is two times the equilibrium concentration of A. The equilibrium constant is

• 4

• $\frac{1}{4}$

• 9

• $\frac{1}{9}$