Solution Found!
Use orbital notation to illustrate the bonding in each of
Chapter 6, Problem 6.1.34(choose chapter or problem)
Use orbital notation to illustrate the bonding in each of the following molecules:
a. chlorine, \(\mathrm{Cl}_{2}\)
b. oxygen, \(\mathrm{O}_{2}\)
c. hydrogen fluoride, HF
Questions & Answers
QUESTION:
Use orbital notation to illustrate the bonding in each of the following molecules:
a. chlorine, \(\mathrm{Cl}_{2}\)
b. oxygen, \(\mathrm{O}_{2}\)
c. hydrogen fluoride, HF
ANSWER:Step 1 of 3
To illustrate bonding between two atoms, we should first know their electronic configuration.
Chlorine with \(Z=17\) has the electronic configuration: \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}\)
Its orbital notation is shown below:
So in a chlorine molecule, we have two such Cl atoms, each having one unpaired electron in the p-orbital. These two unpaired electrons combine to form a sigma bond between the two Cl atoms, thus creating a \(\mathrm{Cl}_{2}\) molecule.