Question

1. the ionization energies of a given atom are ie₁ = 5.139 kj/mol, ie₂ = 47.286 kj/mol., ie3 = 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 ionization energy indicates that a core (non - valence) electron is being removed. Here, \(IE_1 = 5.139\ kJ/mol\) and \(IE_2=47.286\ kJ/mol\). The large increase from \(IE_1\) to \(IE_2\) suggests that after removing the first electron (which is a valence electron), the second electron is a core electron. So, the atom has 1 valence electron. The general valence electron configuration for an atom with 1 valence electron is \(ns^1\).

Answer:

The valence electron configuration is \(ns^1\). The large increase in ionization energy from \(IE_1\) to \(IE_2\) implies that the first electron removed is a valence electron and the second electron removed is a core electron. Since only one valence electron is easily removed (low \(IE_1\) compared to \(IE_2\)), the valence electron configuration is \(ns^1\).