Oxidation number of P in pyrophosphoric acid is:

1.  +5
2.  +2
3.  +3
4.  +4

A compound having two direct bonds between P and H atoms is:

1. $H_{3}P{O}_2$

2. $H_{3}P{O}_3$

3. $H_{3}P{O}_4$

4. $H_4{P}_2{O}_7$

General behavior of $O_3$ is: 

1. To give electrons
2. To Give $O_2$
3. Reaction with $H_2$
4. To accept electrons

 Wrong statement among the following is:

1. Bond energy of F₂ > Cl₂

2. Electronegativity of F > Cl

3. F is more oxidizing than Cl

4. Electron affinity of Cl > F

From the given options, the compound that has a planar structure is:
1. XeF₄
2. XeOF₂
3. XeO₂F₂
4. XeO₄

In X- H ----- Y, X, and Y both are electronegative elements. The correct statement among the following is:

Nitrogen form $N_2$, but phosphorous  form $P_2$, it's at a time convert in $P_4$, reason is:

1. Triple bond present between phosphorous atoms. 
2. $\mathrm{p}\mathrm{\pi }-p\mathrm{\pi }$ bonding is weak in phosphorous.
3. $\mathrm{p}\mathrm{\pi }-p\mathrm{\pi }$ bonding is strong in phosphorous.
4. Multiple bonds easily form phosphorous.

The correct statement among the following is:

Incorrect statement among the following is:

The correct order of acid strength is -

1. ${\mathrm{HClO}}_4<{\mathrm{HClO}}_3<{\mathrm{HClO}}_2<\mathrm{HClO}$

2. ${\mathrm{HClO}}_2<{\mathrm{HClO}}_3<{\mathrm{HClO}}_4<\mathrm{HClO}$

3. ${\mathrm{HClO}}_4<\mathrm{HClO}<{\mathrm{HClO}}_2<{\mathrm{HClO}}_3$

4. $\mathrm{HClO}<{\mathrm{HClO}}_2<{\mathrm{HClO}}_3<{\mathrm{HClO}}_4$