Z effective 2.37

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Z effective 2.37

Postby CaminaB_1D » Sun Oct 28, 2018 6:40 pm

can someone please explain to me how effective nuclear charge works in terms of 2.37. Thanks!

"Which of the following statements are true for many- electron atoms? If false, explain why. (a) The effective nuclear charge Zeff 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 for an electron in a p-orbital is lower than for an electron in an s-orbital in the same shell."

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Re: Z effective 2.37

Postby jessicahe4Elavelle » Sun Oct 28, 2018 7:00 pm

The Zeff is the net positive charge that valence electrons experience from the protons in the nucleus.
(a) is false because Zeff is largely dependent on the number of electrons in the atom. This is because the electrons in lower energy levels can shield electrons in higher energy orbitals thus decreasing the effective nuclear charge.
(b) this is true because the electrons in the s orbital are the nearest to the nucleus and can, therefore, shield the other electrons.
(c) This is false because electrons in the l2 subshell are farther away from the electrons in the l1 subshell.
(d) this is true because the electrons in the p orbital are shielded by the ones in the s orbital thus they experience a lower effective nuclear charge.

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