Question

select the diamagnetic species from the following: (a) hnc, (b) o₂²⁻, (c) oh, (d) hco, and (e) h₂. their lewis structures are described below. check all that apply. (a) h—n⁺≡c⁻ (b) :o⁻—:o⁻ (c) :o⁻—h (d) h—c·=o· (e) h—h

Explanation:

Step1: Recall the definition of diamagnetic species

Diamagnetic species have all electrons paired.

Step2: Analyze each species

• (a) HNC:

The Lewis structure is \(H - \overset{+}{N}\equiv\overset{-}{C}\). All electrons are paired.

• (b) \(O_{2}^{2 - }\):

The Lewis structure is \(\overset{-}{\underset{\cdot\cdot}{O}}-\overset{\cdot\cdot}{O}\overset{-}{\underset{\cdot\cdot}{}}\). All electrons are paired.

• (c) \(OH\):

The Lewis structure is \(\overset{\cdot\cdot}{O}-H\). There is an unpaired electron on oxygen.

• (d) \(HCO\):

The Lewis structure is \(H-\overset{\cdot}{C}=\overset{\cdot\cdot}{O}\). There is an unpaired electron on carbon.

• (e) \(H_{2}\):

The Lewis structure is \(H - H\). All electrons are paired.

Answer:

(a) HNC, (b) \(O_{2}^{2 - }\), (e) \(H_{2}\)