Question

which of the following matches the electronic configuration of a paramagnetic element?
a. (1s^{2}2s^{2}2p^{6}3s^{2}3p^{1})
b. (rn7s^{2}5f^{14}6d^{10})
c. (1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6})
d. (xe6s^{2}4f^{14}5d^{10}6p^{6})
e. (1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2})

Explanation:

Step1: Recall the concept of paramagnetism

Paramagnetic elements have unpaired electrons.

Step2: Analyze option A

For \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{1}\), in the \(3p\) sub - shell, according to Hund's rule, there is 1 unpaired electron.

Step3: Analyze option B

For \([Rn]7s^{2}5f^{14}6d^{10}\), all electrons in \(7s\), \(5f\) and \(6d\) sub - shells are paired (\(s\): \(n = 2\), \(f\): \(n=14\), \(d\): \(n = 10\)).

Step4: Analyze option C

For \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}\), all electrons in \(s\) (\(n = 2\)), \(p\) (\(n=6\)), \(d\) (\(n = 10\)) sub - shells are paired.

Step5: Analyze option D

For \([Xe]6s^{2}4f^{14}5d^{10}6p^{6}\), all electrons in \(s\) (\(n = 2\)), \(f\) (\(n=14\)), \(d\) (\(n = 10\)), \(p\) (\(n=6\)) sub - shells are paired.

Step6: Analyze option E

For \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}\), all electrons in \(s\) (\(n = 2\)), \(p\) (\(n=6\)), \(d\) (\(n = 10\)) sub - shells are paired.

Answer:

A. \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{1}\)