Chapter 20: Problem 2

a) Why do AVEEs decrease as one goes down a group? b) What other periodic property has this same trend?

Short Answer

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a) AVEEs decrease as one goes down a group because the atomic radius increases, weakening the electrostatic attraction between electrons and the nucleus, hence it is easier to remove an electron and so the AVEE is lower. b) The other periodic property that follows the same trend is ionization energy. It also decreases as you move down a group due to the same reason as AVEEs.

Step by step solution

Understand AVEEs trend down a group

As one moves down in a group (vertical column) on the Periodic Table, Atomic Volume Electron Energy (AVEEs) decrease. This is due to the increase in atomic radius (atom size). As atomic radius increases, electrons are located further from the nucleus and the electrostatic attraction between the electrons and the nucleus decreases. Hence, it is easier to remove electrons, leading to lower electron energy or what we call Atomic Volume Electron Energy.

Identifying other periodic property with similar trend

To find another periodic property that also decreases as you move down a group, it's necessary to look back on the principles of atomic structure. An obvious candidate would be ionization energy. Ionization energy is the energy required to remove an electron from an atom. As you move down a group, atomic size increases, and electrons are further from the nucleus. Consequently, they are held less tightly by the electrostatic attraction and can be removed more easily. Thus, ionization energy decreases down a group, similar to AVEEs.

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a) Why do AVEEs decrease as one goes down a group? b) What other periodic property has this same trend?

Short Answer

Step by step solution

Understand AVEEs trend down a group

Identifying other periodic property with similar trend

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