In bisulphate ion, HSO₄^-, the formal charge on S atom is

1. +6

2. +4

3. +1

4. +2

Which molecules/ions are most paramagnetic?

1. B₂

2. C₂

3. $O_2^{+}$

4. $O_2^{-}$

Favourable conditions for electrovalency are:

A molecule that has a complete octet is:

 1. BeCl₂(dimer)       

 2. BeH₂(dimer)

 3. BeH₂(s)               

 4. BeCl₂(s)

On the left are given decreasing orders of elements for a certain property and on the right side is given the property. The incorrect order for the given properties is:

1. ${\mathrm{AlF}}_3>\mathrm{MgO}>{\mathrm{MgF}}_2$    : Lattice energy

2. $\mathrm{Li}>\mathrm{Na}>\mathrm{Al}>\mathrm{Mg}$       : Electron affinity

3. ${\mathrm{PF}}_5>$ ${\mathrm{SF}}_6$ $>$ ${\mathrm{SiF}}_4$      : Lewis acidic character

4. ${\mathrm{SiCl}}_4>{\mathrm{SiBr}}_4$ $>{\mathrm{SiI}}_4$   : Decreasing ionic character

Among the following, the molecule expected to be stabilized by anion formation is : C₂, O₂, NO, F₂

1. NO
2. O₂
3. C₂
4. F₂

Overlap of which of the following atomic orbitals would be maximum to form the strongest covalent bond.

1. 1s-2s (σ)

2. 1s-2p (σ)

3. 2p-2p (π)

4. 2p-2p (σ)

Case Study Question:
The relative location of the bond pair and the lone pair is decided by Bent's rule. The rule states that the more electronegative atom prefers to stay in the orbital having less s character while the lone pair prefers to stay in the orbital having more s character. In molecules with trigonal bipyramidal (TBP) geometry, the more electronegative atom prefers the axial position while the lone pair prefers the equatorial position. 

Which molecule, among the following, has non-zero dipole moment? 

1. PCl₃F₂ 

2. PCl₃Br₂ 

3. PCl₃(CH₃)₂ 

4. Both (2) and (3) 

Which of the following correctly represents the decreasing order of bond angles for NH₃, PH₃, NF₃, and PF₃?

1. NH₃ > PH₃ > NF₃  > PF₃   

2. NH₃ > NF₃ >  PH₃  > PF₃  

3. NH₃ > NF₃ >  PF₃  > PH₃   

4. NH₃ > PF₃ > NF₃  > PH₃