Amongst the following,the number of oxide(s) | vedclass

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(C) To determine the paramagnetism,we check for the presence of unpaired electrons:$Na_2O$: Diamagnetic (all electrons paired).$KO_2$: Paramagnetic (c

Vedclass · Accepted Answer

$4$

Vedclass · Answer

(C) To determine the paramagnetism,we check for the presence of unpaired electrons:$Na_2O$: Diamagnetic (all electrons paired).$KO_2$: Paramagnetic (contains $O_2^-$ ion with one unpaired electron).$NO_2$: Paramagnetic (odd number of valence electrons,$17$ valence electrons).$N_2O$: Diamagnetic (all electrons paired).$ClO_2$: Paramagnetic (odd number of valence electrons,$19$ valence electrons).$NO$: Paramagnetic (odd number of valence electrons,$11$ valence electrons).$SO_2$: Diamagnetic (all electrons paired).$Cl_2O$: Diamagnetic (all electrons paired).The paramagnetic oxides are $KO_2$,$NO_2$,$ClO_2$,and $NO$.Therefore,the total number of paramagnetic oxides is $4$.

Amongst the following,the number of oxide$(s)$ which are paramagnetic in nature is $Na_2O$,$KO_2$,$NO_2$,$N_2O$,$ClO_2$,$NO$,$SO_2$,$Cl_2O$.

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