Question

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the following lewis diagram represents the valence electron configuration of a main - group element.
(enter the answer using superscript.)
if this element is in period 5, its valence electron configuration is
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Explanation:

Step1: Determine valence electrons from Lewis diagram

The Lewis diagram shows 5 valence electrons (the dots around X). So the valence electron configuration for a main - group element in period 5 will have the outermost electrons in the \(n = 5\) shell. For a main - group element with 5 valence electrons, the valence electron configuration is \(5s^{2}5p^{3}\) (since \(s\) orbital can hold 2 electrons and \(p\) orbital can hold up to 6, and we have 5 valence electrons: \(2+3 = 5\)).

Step2: Confirm the period and valence electrons

The element is in period 5, so the principal quantum number \(n = 5\). The number of valence electrons is 5 (from the Lewis dot structure: count the number of dots, which is 5). The electron configuration for the valence shell ( \(n = 5\)) with 5 electrons is \(5s^{2}5p^{3}\).

Answer:

\(5s^{2}5p^{3}\)