In which species would 2 unpaired electrons be present in the ground state: $a. sodium atom;$ $"a. sodium atom;"$ $b. cobalt atom;$ $"b. cobalt atom;"$ $c. iron dication,$ $"c. iron dication,"$ $F e^{2 +}$ $Fe^(2+)$ ; $d. iron atom?$ $"d. iron atom?"$

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In which species would 2 unpaired electrons be present in the ground state: $a. sodium atom;$ $"a. sodium atom;"$ $b. cobalt atom;$ $"b. cobalt atom;"$ $c. iron dication,$ $"c. iron dication,"$ $F e^{2 +}$ $Fe^(2+)$ ; $d. iron atom?$ $"d. iron atom?"$

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Answer 1 · 2017-08-16T08:29:55

$Option (d)$ $"Option (d)"$ .

Explanation:

We can immediately eliminate $N a$ $Na$ , $Z = 11$ $Z=11$ , and $C o$ $Co$ , $Z = 27$ $Z=27$ , because these give rise to an odd number of electrons in the ground state, the which must necessarily be UNPAIRED.

As regards, $b .$ $b.$ , i.e. $F e$ $Fe$ , we have $Z = 26$ $Z=26$ , however, Hunds' rule dictates a configuration of $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{6}$ $1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)3d^6$ . In the isolated ATOM, we must fit 6 electrons into the 5 valence $d-orbitals$ $"d-orbitals"$ . At least 2 of the electrons must be unpaired.

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In which species would 2 unpaired electrons be present in the ground state: $a. sodium atom;$ $"a. sodium atom;"$ $b. cobalt atom;$ $"b. cobalt atom;"$ $c. iron dication,$ $"c. iron dication,"$ $F e^{2 +}$ $Fe^(2+)$ ; $d. iron atom?$ $"d. iron atom?"$

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In which species would 2 unpaired electrons be present in the ground state: a. sodium atom;"a. sodium atom;" b. cobalt atom;"b. cobalt atom;" c. iron dication,"c. iron dication," Fe2+Fe^(2+); d. iron atom?"d. iron atom?"

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In which species would 2 unpaired electrons be present in the ground state: $a. sodium atom;$ $"a. sodium atom;"$ $b. cobalt atom;$ $"b. cobalt atom;"$ $c. iron dication,$ $"c. iron dication,"$ $F e^{2 +}$ $Fe^(2+)$ ; $d. iron atom?$ $"d. iron atom?"$