Oxygen molecule is paramagnetic because
- ABonding electrons are more than antibonding electrons
- BContains unpaired electrons
- CBonding electrons are less than antibonding electrons
- DBonding electrons are equal to antibonding electrons
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View SolutionMatch each of the diatomic molecules in Column $I$ with its property / properties in Column $II$.
Column $I$ Column $II$ $(A)$ $B_2$ $(p)$ Paramagnetic $(B)$ $N_2$ $(q)$ Undergoes oxidation $(C)$ $O_2^{-}$ $(r)$ Undergoes reduction $(D)$ $O_2$ $(s)$ Bond order $\geq 2$ $(t)$ Mixing of '$s$' and '$p$' orbitals
| Column $I$ | Column $II$ |
| $(A)$ $B_2$ | $(p)$ Paramagnetic |
| $(B)$ $N_2$ | $(q)$ Undergoes oxidation |
| $(C)$ $O_2^{-}$ | $(r)$ Undergoes reduction |
| $(D)$ $O_2$ | $(s)$ Bond order $\geq 2$ |
| $(t)$ Mixing of '$s$' and '$p$' orbitals |
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