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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

Expert verified
a) AVEEs decrease as one moves down a group because the addition of new electron shells increases the atomic radius and the distance between the nucleus and the valence electrons, weakening their attraction and lowering the AVEEs. b) The atomic radius or atomic volume is another periodic property that follows the same trend as AVEEs.

Step by step solution

01

Understanding the Atomic Structures

In a group of the Periodic Table, the number of electron shells increases as you move down. An additional shell means greater distance between the nucleus and the valence electrons, which results in a larger atomic radius. Each new shell is further from the nucleus so the attraction between the nucleus and the valence electron(s) becomes weaker. Atomic Volume Electron Energies (AVEEs) decrease as this distance increases. The weaker the nuclear pull on an electron, the lower the AVEE.
02

Correlating Periodic Properties

Atomic radii and atomic volume - both exhibit a similar trend as AVEEs in the Periodic Table. As you move down a group or column in the Periodic Table, atomic radius generally increases. This is due to the addition of new energy levels or shells, which increase the size of the atomic volume. This additional distance between the nucleus and the valence (outermost) electrons weakens the nuclear attraction towards the electrons, which then decreases the AVEES. Hence, atomic radius or atomic volume is another periodic property that shows the same trend as AVEEs.

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Most popular questions from this chapter

a) Why do AVEEs increase as one goes from left to right across a period? b) What other periodic property has this same trend?

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