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-

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) :

Electronic configuration of carbon is

So, electronic configuration of will be , as it has given its two electrons present in the outermost valence shell.

This molecule of will behave as diamagnetic species as there are no unpaired electrons in the orbital.

Answer 2)

Explanation : The electronic configuration of Lithium is

When lithium is in state it will have electronic configuration as

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

Therefore, the species will behave like a paramagnetic substance.

Answer 3)

Boron has electronic configuration as ,

So, the excited state of will be ,

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

This will make as a paramagnetic substance.

you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6

d.) the average kinetic energy of the gas particles is greater in container b because its particles move faster.