Consider the elements neon, bromine, and phosphorus. Which has five electrons in its 4p sublevel?
I got phosphorus wrong as my answer....
Phosphorus has three electrons in its 3p sublevel
so it would be Bromine?
Only bromine. You have to write electron configuration:
[Br]:1s^22s^22p^63s^23p^63d^{10}4s^24p^5
Thank you :)
To determine which element has five electrons in its 4p sublevel, we need to look at the electron configuration of each element.
The electron configuration of neon (Ne) is 1s² 2s² 2p⁶, meaning it has completely filled its 2p sublevel with six electrons.
The electron configuration of bromine (Br) is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁵. We can see that in the 4p sublevel, there are five electrons present in the case of bromine.
The electron configuration of phosphorus (P) is 1s² 2s² 2p⁶ 3s² 3p³, which also shows that in the 3p sublevel, there are three electrons present instead of five.
Therefore, the correct element with five electrons in its 4p sublevel is bromine (Br), not phosphorus (P).