Which of the following pairs of species are p | vedclass

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(C) To determine paramagnetism,we look for the presence of unpaired electrons.$1$. $O_2$: According to Molecular Orbital Theory,the electronic configu

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$O_2$ and $KO_3$

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(C) To determine paramagnetism,we look for the presence of unpaired electrons.$1$. $O_2$: According to Molecular Orbital Theory,the electronic configuration is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1 = \pi^* 2p_y^1$. It has $2$ unpaired electrons,so it is paramagnetic.$2$. $Na_2O_2$: Contains the peroxide ion $O_2^{2-}$. The configuration is $\sigma^* 2p_x^2 = \sigma^* 2p_y^2$. All electrons are paired,so it is diamagnetic.$3$. $BaO_2$: Contains the peroxide ion $O_2^{2-}$,which is diamagnetic.$4$. $KO_3$: Contains the ozonide ion $O_3^-$. The $O_3^-$ ion has $19$ valence electrons. Molecular orbital calculations show it has an unpaired electron in the antibonding $\pi^*$ orbital,making it paramagnetic.Therefore,$O_2$ and $KO_3$ are both paramagnetic.

List-$I$	List-$II$
$(1)$ ${\rm{NO}}$	$(A)$ $1.5$
$(2)$ ${\rm{CO}}$	$(B)$ $2.0$
$(3)$ ${\rm{O}}_2^-$	$(C)$ $2.5$
$(4)$ ${\rm{O}}_2$	$(D)$ $3.0$

Which of the following pairs of species are paramagnetic?

Similar Questions

Which of the following molecular orbitals has two nodal planes?

Match the species given in List-$I$ with their bond orders given in List-$II$.

List-$I$ List-$II$

$(1)$ ${\rm{NO}}$ $(A)$ $1.5$

$(2)$ ${\rm{CO}}$ $(B)$ $2.0$

$(3)$ ${\rm{O}}_2^-$ $(C)$ $2.5$

$(4)$ ${\rm{O}}_2$ $(D)$ $3.0$

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Four diatomic species are listed below. Identify the correct order in which the bond order is increasing in them.

Which of the following molecules does not exist according to molecular orbital theory?

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