Page 1 of 1

Effective Nuclear Charge

Posted: Sun Oct 27, 2019 4:27 pm
by Sean Sugai 4E
In multi-electron atoms, each electron is repelled by other present electrons. How do more electrons affect shielding and nuclear attraction?

Re: Effective Nuclear Charge

Posted: Sun Oct 27, 2019 4:38 pm
by katrinawong3d
The more electrons there are, the greater the shielding effect on the outermost electrons. So, since there are more electrons to repel each other, the attraction between an electron and the nucleus (nuclear attraction) decreases.

Re: Effective Nuclear Charge

Posted: Sun Oct 27, 2019 5:09 pm
by Siddiq 1E
What is the relationship between effective nuclear charge and ionization energy?

Re: Effective Nuclear Charge

Posted: Sun Oct 27, 2019 5:43 pm
by Elena Bell 1C
Effective nuclear charge affects ionization energy because more protons and pull the electrons closer to the nucleus and make it harder to remove electrons.

Re: Effective Nuclear Charge

Posted: Sun Oct 27, 2019 5:54 pm
by John Arambulo 1I
Yes, a higher number of electrons results in an increase in shielding and a decrease in effective nuclear charge. This is because an increased number of electrons between an atom's positive nucleus and the atom's valence electrons results in both increased attraction between the internal electrons and the nucleus as well as increased electron-electron repulsion (i.e. increased shielding). Because of this, it's almost like the nucleus has "less positive charge" that can effectively interact with the outer electrons... a decrease in effective nuclear charge due to an increase in shielding.