Question
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)ResponsesBromine 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.Chlorine atoms are larger than bromine atoms.Chlorine atoms form a double bond, and bromine atoms form a single bond.
Answers
GPT-4o mini
The correct statement that best explains the difference in bond energies between Cl–Cl and Br–Br bonds is:
**Bromine has more electron levels than chlorine.**
This is because bromine, being located below chlorine in the same group (Group 17 of the periodic table), has more electron shells. As the number of electron shells increases, the outer electrons are further from the nucleus, leading to increased electron shielding and reduced effective nuclear charge experienced by the bonding electrons. This results in a weaker bond for bromine compared to chlorine, which explains the lower bond energy of the Br–Br bond (190 kJ/mol) compared to the Cl–Cl bond (240 kJ/mol).
**Bromine has more electron levels than chlorine.**
This is because bromine, being located below chlorine in the same group (Group 17 of the periodic table), has more electron shells. As the number of electron shells increases, the outer electrons are further from the nucleus, leading to increased electron shielding and reduced effective nuclear charge experienced by the bonding electrons. This results in a weaker bond for bromine compared to chlorine, which explains the lower bond energy of the Br–Br bond (190 kJ/mol) compared to the Cl–Cl bond (240 kJ/mol).