1E.5

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Aashka Popat 1A
Posts: 50
Joined: Sat Sep 07, 2019 12:16 am

1E.5

Postby Aashka Popat 1A » Sun Oct 13, 2019 11:49 pm

The question is: Which of the following statements are true for many-elec- tron atoms? If false, explain why. (a) The effective nuclear charge Zeffe is independent of the number of electrons present in an atom. (b) Electrons in an s-orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge because an electron in an s-orbital can penetrate to the nucleus of the atom. (c) Electrons having l = 2 are better at shielding than electrons having l = 1. (d) Zeff e for an electron in a p-orbital is lower than for an electron in an s-orbital in the same shell.

I'm having trouble understanding why part c is false and part d is true, could anyone explain it to me? Thanks

DMuth_1J
Posts: 63
Joined: Thu Jul 11, 2019 12:15 am

Re: 1E.5

Postby DMuth_1J » Mon Oct 14, 2019 2:54 pm

For part C, the orbitals are the same energy level and same mathematical shape. They are identical, only differing in the directions they face. If you think of an atom like a circle, the direction they face doesn't change the electron's ability to inhibit interaction with another atom. Basically, it is false because the two orbitals mentioned are pretty much the same.

For part D, it would require more energy to be in an orbital that is not spherical (the s orbital "fills" before any of the others). If it has more energy and is further away from the nucleus of the atom, the Zeff is smaller.

DMuth_1J
Posts: 63
Joined: Thu Jul 11, 2019 12:15 am

Re: 1E.5

Postby DMuth_1J » Mon Oct 14, 2019 2:54 pm

For part C, the orbitals are the same energy level and same mathematical shape. They are identical, only differing in the directions they face. If you think of an atom like a circle, the direction they face doesn't change the electron's ability to inhibit interaction with another atom. Basically, it is false because the two orbitals mentioned are pretty much the same.

For part D, it would require more energy to be in an orbital that is not spherical (the s orbital "fills" before any of the others). If it has more energy and is further away from the nucleus of the atom, the Zeff is smaller.


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