Solution Found!
The electron affinities, in kJ>mol, for the group 1B and
Chapter , Problem 7.98(choose chapter or problem)
The electron affinities, in kJ>mol, for the group 1B and group 2B metals are as follows: Hg > 0 Au 223 Cd > 0 Ag 126 Zn > 0 Cu 119 (a) Why are the electron affinities of the group 2B elements greater than zero? (b) Why do the electron affinities of the group 1B elements become more negative as we move down the group? [Hint: Examine the trends in the electron affinities of other groups as we proceed down the periodic table.]
Questions & Answers
QUESTION:
The electron affinities, in kJ>mol, for the group 1B and group 2B metals are as follows: Hg > 0 Au 223 Cd > 0 Ag 126 Zn > 0 Cu 119 (a) Why are the electron affinities of the group 2B elements greater than zero? (b) Why do the electron affinities of the group 1B elements become more negative as we move down the group? [Hint: Examine the trends in the electron affinities of other groups as we proceed down the periodic table.]
ANSWER:Step 1 of 2
(a)
The general configuration of group 2B metals is . Their outer electronic configuration is fully paired that means they don’t want electrons. Due to this, they have low ability to accept the electron and large amount of energy is required for the addition of the electron. Thus, they have electron affinities greater than zero.