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:

1.	The electronegativity of flourine is much higher than other elements in group
2.	There is strong hydrogen bonding between HF molecules
3.	The bond energy of HF molecules is greater than in other hydrogen halides
4.	The effect of nuclear shielding is much reduced in flourine which polarizes the HF molecule

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.

The acidity of diprotic acids in aqueous solution increases in the order:

1. H₂S < H₂Se < H₂Te

2. H₂Se < H₂S < H₂Te

3. H₂Te < H₂S < H₂Se

4. H₂Se < H₂Te < H₂S

Which of the following compounds does not release oxygen when heated?

1. Zn(ClO₃)₂
2. K₂Cr₂O₇
3. (NH₄)₂Cr₂O₇
4. KClO₃

The incorrect statement regarding oxoacids of phosphorus is:

Oxidation states of P in H₄P₂O₅, H₄P₂O₆, H₄P₂O₇, are respectively:

Among the following which is the strongest oxidising agent?

1. $F_2$

2. $B{r}_2$

3. $l_2$

4. $C{l}_2$

The correct thermal stability order for \(\mathrm{{H}_2 {E}},\)  \(\mathrm{{ E}= {O}, {S}, {Se}, {Te}} \text { and } \mathrm{Po}\)  among the following is:
1. \(\mathrm{{H}_2 {Se}<{H}_2 {Te}<{H}_2 {Po}<{H}_2 {O}<{H}_2 S}\)
2. \(\mathrm{{H}_2 {~S}<{H}_2 {O}<{H}_2 {Se}<{H}_2 {Te}<{H}_2 {Po}}\)
3. \(\mathrm{{H}_2 {O}<{H}_2 {~S}<{H}_2 {Se}<{H}_2 {Te}<{H}_2 {PO}}\)
4. \(\mathrm{{H}_2 {Po}<{H}_2 {Te}<{H}_2 {Se}<{H}_2 {~S}<{H}_2 {O}}\)

Match the Xenon compounds in Column I with their structure in Column II and assign the correct code:

Code:

Match the name of process given in Column I with the name of compound given in Column II and mark the correct option.