Given below are two statements :
Statement I: A hypothetical diatomic molecule with bond order zero is quite stable.
Statement II: As bond order increases, the bond length increases.
In the light of the above statements, choose the most appropriate answer from the options given below:
Match List-I with List-II
| List - I | List - II | ||
|---|---|---|---|
| A | $\mathrm{XeO}_3$ | I | $\mathrm{sp}^3 \mathrm{~d}$; linear |
| B | $\mathrm{XeF}_2$ | II | $\mathrm{sp}^3$; pyramidal |
| C | $\mathrm{XeOF}_4$ | III | $s p^3 d^3$; distorted octahedral |
| D | $\mathrm{XeF}_6$ | IV | $s p^3 d^2$; square pyramidal |
Choose the correct answer from the options given below :
Identify the correct orders against the property mentioned
A. $\mathrm{H}_2 \mathrm{O}>\mathrm{NH}_3>\mathrm{CHCl}_3$-dipole moment
B. $\mathrm{XeF}_4>\mathrm{XeO}_3>\mathrm{XeF}_2$ - number of lone pairs on central atom
C. $\mathrm{O}-\mathrm{H}>\mathrm{C}-\mathrm{H}>\mathrm{N}-\mathrm{O}-$ bond length
D. $\mathrm{N}_2>\mathrm{O}_2>\mathrm{H}_2-$ bond enthalpy
Choose the correct answer from the options given below:
Which of the following molecules has "NON ZERO" dipole moment value?