Chlorine and bromine are in the same group in the periodic table. The bond energy of a Cl–Cl bond is 240 kJ/mol. The bond energy of a Br–Br bond is 190 kJ/mol. Which statement best explains this difference?(1 point)

Question

Responses

Chlorine atoms form a double bond, and bromine atoms form a single bond.
Chlorine atoms form a double bond, and bromine atoms form a single bond.

Bromine has more electron levels than chlorine.
Bromine has more electron levels than chlorine.

Bromine atoms are more likely than chlorine atoms to interact with other atoms.
Bromine atoms are more likely than chlorine atoms to interact with other atoms.

Chlorine atoms are larger than bromine atoms.

Answer 1

The statement that best explains the difference in bond energy between Cl–Cl and Br–Br bonds is:

Bromine has more electron levels than chlorine.

This statement is accurate because bromine has an additional electron shell compared to chlorine, which leads to increased electron-electron repulsions in the bromine molecule. As a result, the Br–Br bond is weaker (lower bond energy) compared to the Cl–Cl bond. The larger atomic radius of bromine compared to chlorine also contributes to this effect, as it can lead to a longer bond length and weaker bond strength.