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Indicate the number of unpaired electrons in: (a) P, (b) Si, (c) Cr, (d) Fe and (e) Kr.

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(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...
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(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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