Question

HELP PLZZZ Write the full electron configuration for phosphorus, atomic symbol P, then draw an orbital box diagram that accounts for all of the electrons in phosphorus. You don’t need to include the orbital box diagram as part of your answer. Based on your drawing, explain why phosphorus is either paramagnetic or diamagnetic.

Answer 1

a. 1s2, 2s2, 2p6, 3s2, 3p3

b. see attached - the arrow to the left should be facing up, and the arrow to the right should be facing down. I did it backwards - sorry!

c. Phosphorus has three unpaired electrons and therefore is paramagnetic.

Step-by-step explanation:

If the element or substance has unpaired electrons, then it is paramagnetic. If it is all paired up, then it is diamagnetic. This is only for it's grounded state - if it is an ion, then it behaves differently.

Answer 2

The correct configuration is -
`1s^2s^22p^63s^23p^3`

Step-by-step explanation:

Diamagnetism is an extremely week type of attraction that is incited by an adjustment in the orbital movement of electrons because of an applied attractive field. This attraction is nonpermanent and continues due to the presence of an external field.

The magnetic properties of a substance can be controlled by analyzing its electron configuration. If it has unpaired electrons in its outer orbital, at that point the substance is paramagnetic, and in the event that all electrons are found paired, the substance is then diamagnetic.

The electron configuration of the phosphorus is -

`1s^2s^22p^63s^23p^3`. As it is clear that the outer shell of P has 3 unpaired electron it is paramagnetic.