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(a) What is meant by the term effective nuclear charge? (b) How does the effective nuclear charge experienced by the valence electrons of an atom vary going from left to right across a period of the periodic table?

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Jamar Ferry
Jamar FerryLv2
13 May 2020

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Related questions

How does the effective nuclear chargeexperienced by the valence electrons of an atom vary going fromleft to right across a period of the periodic table?


1. Going from left to right across a period, nuclear chargeincreases while the number of electrons in the core is constant.This results in a increase in Zeff.

2. Going from left to right across a period, nuclear chargeremains approximately the same while the number of electrons in thecore decreases. This results in a increase in Zeff.

3. Going from left to right across a period, nuclear chargedecreases while the number of electrons in the core is constant.This results in a decrease in Zeff.

4. Going from left to right across a period, nuclear chargeremains approximately the same while the number of electrons in thecore increases. This results in a decrease in Zeff.

Classify each statement about effective nuclear charge, Zeff, as true or false.

In a Be atom, a 1s electron has a greater Zeff than a 2s electron.

Across a period, as Zeff increases, atomic size decreases.

Electrons in a p orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge.

A 1s electron is a Be atom has a smaller Zeff than a 1s electron in a Li atom.

Effective nuclear charge decreases from left to right across a period on the periodic table.

Effective nuclear charge is dependent on the number of electrons present in an atom.

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