Question

1. justify why the number of valence electrons stays the same within a group using electron configurations. i need a hint groups or families have similar properties and a play b additional electrons are placed in a higher energy level. score: 0/1

Explanation:

Answer:

In a group of the periodic - table, elements have the same outer - shell electron configuration. The principal quantum number \(n\) of the outermost shell (valence shell) increases as we move down the group, but the number of electrons in the outermost orbital set (which defines the valence electrons) remains the same. For example, all elements in Group 1 have an outer - shell electron configuration of \(ns^1\), where \(n = 1,2,3,\cdots\). As we move from hydrogen (\(1s^1\)) to lithium (\(2s^1\)) to sodium (\(3s^1\)) and so on, the number of valence electrons is always 1. This is because the additional electrons as we move down the group are added to higher energy levels while the number of electrons in the outermost orbital set (the valence electrons) is determined by the group number and remains constant within a group.