Question

write the orbital diagram for the valence electrons of na. drag the appropriate labels to their respective targets. labels can be used once, more than once, or not at all. targets may be left blank, such as for unused orbitals.

Explanation:

Step1: Determine Valence Electron of Na

Sodium (Na) has an atomic number of 11. Its electron configuration is \(1s^2 2s^2 2p^6 3s^1\). So, the valence electron is in the \(3s\) orbital.

Step2: Orbital Diagram for \(3s\)

The \(s\) orbital can hold a maximum of 2 electrons, but Na has 1 valence electron. The left - most box (single \(s\) orbital) should have one electron (with spin - up or spin - down, but in the diagram, we place one electron in the \(3s\) orbital). The \(p\) orbitals (the three - box group) are for the \(2p\) subshell, which is filled in Na (valence electrons are only in \(3s\)), so the \(p\) orbitals are not part of the valence electron orbital diagram for the valence electron of Na (the valence electron is in \(3s\)). So, we place one electron (using the appropriate label, likely the single - electron label) in the single \(s\) orbital (the left - most box with one orbital) and leave the \(p\) orbitals (the three - box group) as they are (or with no additional valence electrons).

Answer:

The single \(s\) orbital (left - most box) gets one electron (e.g., the label for one electron, like the '1' or the single - spin label) and the \(p\) orbitals (three - box group) have no additional valence electrons (since valence electron of Na is in \(3s\)). So, the orbital diagram for the valence electron of Na has one electron in the \(3s\) orbital (the single orbital box) and the \(3p\) orbitals (three - box group) are empty for valence electrons.