Chlorine and bromine are in the same group in the periodic table. The bond energy of a Cl–Cl bond is

Question

240 kJ/mol. The bond energy of a Br–Br bond is 190 kJ/mol. Which statement best explains this
difference?(1 point)
Chlorine atoms form a double bond, and bromine atoms form a single bond.
Bromine atoms are more likely than chlorine atoms to interact with other atoms.
Chlorine atoms are larger than bromine atoms.
Bromine has more electron levels than chlorine.

Answer 1

The best explanation for the difference in bond energies between Cl–Cl and Br–Br bonds is:

Bromine has more electron levels than chlorine.

This is because bromine is located lower in the periodic table than chlorine, which means it has more electron shells. This increased distance between the nucleus and the bonding electrons in bromine leads to a weaker bond compared to the Cl–Cl bond. Additionally, the larger size of bromine atoms contributes to a longer bond length, resulting in lower bond energy.