Question

Which of the following factors do not influence the length of a covalent bond?

A) the tendency of atoms to fill the outer electron shells
B) the attractive forces between negatively charged electrons and positively charged nuclei
C) the repulsive forces between the positively charged nuclei
D) the minimization of repulsive forces between the two nuclei by the cloud of shared electrons

Answer 1

The repulsive forces between the positively charged nuclei do not influence the length of a covalent bond. The length of a covalent bond is primarily influenced by the attractive forces between negatively charged electrons and positively charged nuclei, as well as the minimization of repulsive forces between the two nuclei by the cloud of shared electrons.

Step-by-step explanation:

The factor that does not influence the length of a covalent bond is the repulsive forces between the positively charged nuclei. In covalent bonding, atoms share electrons in a mutually stabilizing relationship. The length of a covalent bond is primarily influenced by the attractive forces between negatively charged electrons and positively charged nuclei, as well as the minimization of repulsive forces between the two nuclei by the cloud of shared electrons.

The tendency of atoms to fill the outer electron shells and the repulsive forces between the positively charged nuclei also play a role in determining the length of a covalent bond.