Problem: In the molecule ClF3, chlorine makes three covalent bonds. Therefore, three of its seven valence electrons need to be unpaired. The orbitals with the same energy are known as degenerate orbitals. For example, the p subshell has three degenerate orbital, namely, px, py, and pz. How many degenerate orbitals are needed to contain seven electrons with three of them unpaired?Express your answer numerically.Carbon has four valence electrons in a configuration of 2s22p2 as shown in the diagram. For carbon to form four covalent bonds it must have four unpaired electrons. For carbon to have four unpaired electrons, hybridization must occur. If the s orbital and the three p orbitals were to combine, or hybridize, carbon could have four degenerate orbitals at an energy midway between the s and the p orbitals. The resulting orbitals are called sp3 because they are the combination of one s and three p orbitals.

FREE Expert Solution
Problem Details

In the molecule ClF3, chlorine makes three covalent bonds. Therefore, three of its seven valence electrons need to be unpaired. The orbitals with the same energy are known as degenerate orbitals. For example, the p subshell has three degenerate orbital, namely, px, py, and pz. How many degenerate orbitals are needed to contain seven electrons with three of them unpaired?

Express your answer numerically.


Carbon has four valence electrons in a configuration of 2s22p2 as shown in the diagram. For carbon to form four covalent bonds it must have four unpaired electrons. For carbon to have four unpaired electrons, hybridization must occur. If the s orbital and the three p orbitals were to combine, or hybridize, carbon could have four degenerate orbitals at an energy midway between the s and the p orbitals. The resulting orbitals are called sp3 because they are the combination of one s and three p orbitals.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Hybridization concept. You can view video lessons to learn Hybridization. Or if you need more Hybridization practice, you can also practice Hybridization practice problems.