Question

1. the ionization energies of a given atom are $ie_1 = 5.139 kj/mol$, $ie_2 = 47.286 kj/mol$, $ie_3 = 71.64 kj/mol$. predict the valence electron configuration for the atom, and explain your reasoning.

Explanation:

Ionization energy (IE) is the energy required to remove an electron from an atom. A large jump in IE occurs when removing an electron from a noble - gas - like (stable) electron configuration. Here, there is a large jump between \(IE_1\) and \(IE_2\). This indicates that after removing the first electron, the atom attains a stable (noble - gas - like) configuration. Elements that lose one electron to attain a noble - gas configuration are in Group 1 of the periodic table. The valence electron configuration of Group 1 elements is \(ns^1\).

Answer:

The valence electron configuration is \(ns^1\). The large jump between \(IE_1\) and \(IE_2\) implies that the first electron is relatively easy to remove (low \(IE_1\)), and after its removal, the atom has a stable electron configuration (high \(IE_2\) as removing the second electron disrupts this stability), which is characteristic of elements with a single valence electron (\(ns^1\) configuration).