Match the interhalogen compounds in Column-I with the geometry in Column-II and assign the correct code: 

	Column-I		Column-II
(A)	XX’	(i)	T-shape
(B)	XX’3	(ii)	Pentagonal bipyramidal
(C)	XX’5	(iii)	Linear
(D)	XX’7	(iv)	Square Pyramidal

 

	(A)	(B)	(C)	(D)
1.	(iii)	(i)	(iv)	(ii)
2.	(i)	(iv)	(iii)	(ii)
3.	(iv)	(iii)	(ii)	(i)
4.	(iii)	(iv)	(i)	(ii)

Choose the pairs of isoelectronic compounds which are isostructural:

1. TeF₂, XeF₂

2. IBr₂^-, XeF₂

3. IF₃, XeF₂

4. BeCl₂, XeF₂

In which pair of ions both the species contain S-S bond?

Which of the following reactions does not exhibit the oxidising behaviour of H₂SO₄?

1. Cu + 2H₂SO₄ → CuSO₄ + SO₂ + 2H₂O

2. 3S + 2H₂SO₄ → 3SO₂ + 2H₂O

3. C + 2H₂SO₄ → CO₂ + 2SO₂ + 2H₂O

4. CaF₂ + H₂SO₄ → CaSO₄ + 2HF

In the structure of ClF₃, the number of lone pairs of electrons on central atom 'Cl' is:

1. 1

2. 2

3. 3

4. 4

Which of the statements given below is incorrect?

1. \(\mathrm{C l_{2} O_{7  }}\)${}_{}$is an anhydride of perchloric acid
2. \(\mathrm{O_{3}}\)${\mathrm{}}_{}$ molecule is bent
3. ONF is isoelectronic with \(\mathrm{N O_{2}^{-}}\)${}_{}^{}$ 
4. \(\mathrm{O F_{2}}\) is an oxide of fluorine

The variation of the boiling point of the hydrogen halides is in the order HF > HI > HBr > HCl. 
The higher boiling point of hydrogen fluoride is explained as:

The strong reducing behaviour of H₃PO₂ is due to:

1. Presence of one -OH group and two P-H bonds.

2. High electron gain enthalpy of phosphorus.

3. High oxidation state of phosphorus.

4. Presence of two -OH groups and one P-H bond.