Which of the following species contain unpair | vedclass

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(C) To determine the presence of unpaired electrons,we analyze the electronic structure of each species:$1$. $KO_2$: This contains the superoxide ion,

Vedclass · Accepted Answer

Only $KO_2$

Vedclass · Answer

(C) To determine the presence of unpaired electrons,we analyze the electronic structure of each species:$1$. $KO_2$: This contains the superoxide ion,$O_2^-$. The molecular orbital configuration of $O_2^-$ is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^2 = \pi^* 2p_y^1$. It has one unpaired electron.$2$. $AlO_2^-$: The aluminate ion has a closed-shell structure with no unpaired electrons.$3$. $BaO_2$: This contains the peroxide ion,$O_2^{2-}$. The configuration is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^2 = \pi^* 2p_y^2$. All electrons are paired.$4$. $NO_2^+$: The nitronium ion has $16$ valence electrons $(5 + 6 	imes 2 - 1 = 16)$. It is isoelectronic with $CO_2$ and has no unpaired electrons.Therefore,only $KO_2$ contains an unpaired electron.

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 species contain unpaired electrons: $KO_2, AlO_2^-, BaO_2$,and $NO_2^+$?

Similar Questions

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

List-$I$ List-$II$

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

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

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

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

Which of the following is correctly matched?

In which of the following molecules do the $\pi 2p_x$ and $\pi 2p_y$ orbitals fill after the $\sigma 2p_z$ molecular orbital?

The correct stability order for $N_2$ and its given ions is :-

Paramagnetism is exhibited by molecules:

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