I was going through an article given to me by my teacher which gave info about the influence of the positive nucleus on the electrons in the 's orbital', 'p orbital' and 'd orbital' respectively. Here I am quoting the part of the article which I didn't understand.
Despite the shielding of the outer electrons from the nucleus by the inner shell electrons, the attractive force experienced by the outer shell electrons increases with increase of nuclear charge. In other words, the energy of interaction between, the nucleus and electron (that is orbital energy) decreases (that is more negative) with the increase of the atomic number (Z).
Now after reading the article further I came across this paragraph..
The energy of electrons in s orbital will be lower (more negative) than that of p orbital electron which will have less energy than that of d orbital electron and so on.
Aren't both the above paras contradicting?
First, it says that as the electron is away from nucleus, the nucleus's influence decreases. (like it should) Then why is electron more negative? (see brackets in first para above). Does it mean that as the electron moves away then it has less positive charge and the negative charge dominates?
But in the second para it says that the electron in s orbital (which is near nucleus) is more negative? I mean what's going on in both of these paras?
All in all I want to know,
- Is electron near nucleus more negative/less negative and has lower energy/higher energy?
- Is electron away from nucleus more negative/less negative and has lower energy/higher energy?
Please help me. I did genuine efforts to understand all this and surfed internet for many hours but couldn't get it.