Question

The first ionization energy (kJ/mol) for each group 1 element are shown.

3
Li
520
11
Na
496
19
K
419
37
Rb
403
55
Cs
376
Which statement explains the trend in first ionization energy of group 1 elements?
A. As the number of valence electrons increases, the amount of energy required to add an electron to the atom decreases.
B. As the number of valence electrons increases, the amount of energy required to remove an electron from the atom decreases.
c. As the distance between the nucleus and the outermost electrons increases, the amount of energy required to add an electron to
the atom decreases.
D. As the distance between the nucleus and the outermost electrons increases, the amount of energy required to remove an electron
from the atom decreases.

Answer 1

[AI-generated answer — Bot GPT 3.5]

B. As the number of valence electrons increases, the amount of energy required to remove an electron from the atom decreases.

This statement explains the trend in first ionization energy of group 1 elements. As you move down the group, the number of valence electrons increases, making it easier to remove an electron, resulting in a decrease in ionization energy.