The electron gain enthalpy values for O → O^– and O → O^2– are –141 and 702 kJ  mol^-1 , respectively. The correct statement about the formation of oxides is-

1.	Higher the electron gain enthalpy lower is the lattice energy.
2.	Higher the electron gain enthalpy higher is the lattice energy.
3.	Higher the electron gain enthalpy higher is the stability of oxide.
4.	O- is more stable than O2-

\(\mathrm{Xe}+\mathrm{PtF}_6 \rightarrow \text { ? }\)

The product of the above reaction is:

In which compound does phosphorous have the lowest oxidation state?

1. H₃PO₃ 

2. PCl₃ 

3. Ca₃P₂ 

4. POF₃

 A xenon fluoride that does not exist is:

1. XeF₄
2. XeF₂
3. XeF₃
4. XeF₆

(a) XeF₆ + 3H₂O →

(b) XeF₆ + H₂O $\to$

The products formed in the above reactions, respectively, are:

1. XeO₃ , XeOF₄
2. XeO₆ , XeOF₄
3. XeO₃, XeOF₆
4. XeO₆ , XeOF₆

XeF₄ is isostructural with :

1. ${\mathrm{ICl}}_4^{-}$       

2. ${\mathrm{IBr}}_2^{-}$                   

3. ${\mathrm{BrO}}_3^{-}$

4. ${\mathrm{ICl}}_3^{-}$

Which of the following is incorrect regarding noble gases?

1. The atomic radii corresponds to van der Waal’s radii.

2. They have the largest size in a period.

3. They are also called inert gases.

4. They combine to form molecules.

In solid-state, PCl₅ exists as: 

Match the items in Columns I and II and mark the correct option.

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