Chemistry, 19.01.2020 23:31 alexandraparava

Which of the following diatomic species are paramagnetic and which are diamagnetic? a blank molecular orbital diagram (part b 1 figure) has been provided to you.
drag the formulas to the appropriate magnetic bin : c2^2+,li2-,b2^2-

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Answer : For a species to be diamagnetic it needs to have no unpaired electrons and for paramagnetic the species needs t have unpaired electrons.

Answer 1) : $C_{2} ^{+2}$

Electronic configuration of carbon is $1s^{2}2s^{2} 2p^{2}$

So, electronic configuration of $C_{2} ^{+2}$ will be $1s^{2} 2s^{2}$ , as it has given its two electrons present in the outermost valence shell.

This molecule of $C_{2} ^{+2}$ will behave as diamagnetic species as there are no unpaired electrons in the orbital.

Answer 2) $Li^{-2}$

Explanation : The electronic configuration of Lithium is $1s^{2} 2s^{1}$

When lithium is in $Li^{-2}$ state it will have electronic configuration as $1s^{2} 2s^{2} 2p^{1}$

This shows that Lithium has one electron which is available in 2p orbital, and it is also unpaired.

Therefore, the $Li^{-2}$ species will behave like a paramagnetic substance.

Answer 3) $B_{2}^{-2}$

Boron has electronic configuration as $1s^{2} 2s^{2} 2p^{1}$ ,

So, the excited state of $B_{2}^{-2}$ will be $1s^{2} 2s^{2} 2p^{3}$ ,

Here, Boron in excited state has one unpaired electron in 2p orbital rest 2 electrons are paired in the 2p orbital.

This will make $B_{2}^{-2}$ as a paramagnetic substance.

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Which of the following diatomic species are paramagnetic and which are diamagnetic? a blank molecul...

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