Dimagnetic species are those which contain no unpaired electrons. Which among the following are dimagnetic?

(i) N₂

(ii) N₂^2–

(iii) O₂

(iv) O₂^2-

<p>This is a Multiple Choice Questions as classified in NCERT Exemplar</p><p><strong>Ans:</strong> Option (i) and (iv)</p><p><strong> (i)</strong> N₂ will have 14 electrons in its structure. So, its electronic configuration will be:</p><p>σ1s² σ∗1s² σ2s² σ∗2s², π2p²_x, π2p²_y, s2p_z²</p><p>According to the molecular electronic configuration of N₂ it does not contain any unpaired electrons, it will be diamagnetic in nature.</p><p><strong> (ii)</strong> N₂^{2<strong>–</strong>} will have 16 electrons in its structure. So, its molecular electronic configuration will be:</p><p>σ1s² σ∗1s² σ2s² σ∗2s², π2p²_x, π2p²_y, s2p_z², , π*2p¹_y</p><p>According to the molecular electronic configuration of 2 N₂^-, it has two unpaired electrons in π*2p¹_x, &nbsp;&nbsp;π*2p¹_y&nbsp; sub- shell. Hence, it will be paramagnetic in nature.</p><p><strong> (iii)</strong> O₂ will have 16 electrons in its structure. So, its molecular electronic configuration will be:</p><p>σ1s² σ∗1s² σ2s² σ∗2s²s2p_z²π2p²_y π2p²_x π*2p¹_y π*2p¹_x</p><p>According to the molecular electronic configuration of O₂, it has two unpaired electrons in π2p¹_y π*2p¹_x&nbsp; sub-shell. Hence, it will be paramagnetic in nature.</p><p><strong> (iv)</strong> O₂^2- will have 18 electrons in its structure. So, its molecular electronic configuration will be:</p><p>σ1s² σ∗1s² σ2s² σ∗2s²s2p_z²π2p²_y π2p²_x π*2p²_y π*2p²_x</p><p>According to the molecular electronic configuration of O₂^2- it does not contain any unpaired electrons, it will be diamagnetic in nature.</p>

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