Question

The electron configuration of an atom determines the number of electrons available to participate in bonding with another atom. One method of depicting the valence electrons that an atom has is through the Lewis structure. To begin this discussion, pick an element from the periodic table of elements. Identify the valence electrons and the orbitals in which they reside. You can use the textbook and lecture. Note: The goal of this exercise is to become familiar with the concepts. This discussion will also explore how this impacts the ability of atoms to bond and the 3D structure of the molecule.

Answer 1

Try the Chlorate ion: (ClO₃^-)

SOLUTION

First, lets find the how many valence electrons chlorate has:

ClO₃^- : 7 e^-(from Cl) + 3(6) e^-(from 3 O atoms) + 1 (from the total charge of -1) = 26

There are 26 valence electrons.

Next lets draw the basic framework of the molecule:

The molecule uses covalent bonds to hold together the atoms to the central Chlorine. The remaining electrons become non-bonding electrons. Since 6 electrons were used for the bonds, the 20 others become those un-bonding electrons to complete the octet:

The oxygen atom's shells fill up with 18 electrons, and the other 2 complete Chlorine's octet.