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Asked by Anish Last Modified
Answer (a) Phosphorus (P):
Atomic number = 15
The electronic configuration of P is:
1s2 2s2 2p6 3s2 3p3
The orbital picture of P can be represented as:
From the orbital picture, phosphorus has three unpaired electrons.
(b) Silicon (Si):
Atomic number = 14
The electronic configuration of Si is:
1s2 2s2 2p6 3s2 3p2
The orbital picture of Si can be represented as:
From the orbital picture, silicon has two unpaired electrons.
(c) Chromium (Cr):
Atomic number = 24
The electronic configuration of Cr is:
1s2 2s2 2p6 3s2 3p6 4s1 3d5
The orbital picture of chromium is:
From the orbital picture, chromium has six unpaired electrons.
(d) Iron (Fe):
Atomic number = 26
The electronic configuration is:
1s2 2s2 2p6 3s2 3p6 4s2 3d6
The orbital picture of chromium is:
From the orbital picture, iron has four unpaired electrons.
(e) Krypton (Kr):
Atomic number = 36
The electronic configuration is:
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
The orbital picture of krypton is:
Since all orbitals are fully occupied, there are no unpaired electrons in krypton.
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