Question

What is the trend for ionization energy across a period and down a group? Explain this trend in terms of attraction and repulsion.

a) Ionization energy increases across a period and decreases down a group due to increasing atomic size.
b) Ionization energy decreases across a period and increases down a group due to decreasing atomic size.
c) Ionization energy increases across a period and down a group due to decreasing atomic size.
d) Ionization energy decreases across a period and down a group due to increasing atomic size.

Answer 1

Ionization energy increases across a period and decreases down a group due to decreasing atomic size.

Step-by-step explanation:

The trend for ionization energy across a period is that it generally increases from left to right. This is because as you move across a period, the atomic size decreases and the electrostatic interactions between the nucleus and valence electrons increase. As a result, it becomes more difficult to remove electrons from the atoms, leading to an increase in ionization energy.

The trend for ionization energy down a group is that it decreases from top to bottom. This is because as you move down a group, the valence electrons are located in higher energy orbitals that are farther away from the nucleus. These electrons experience less pull from the nucleus, making it easier to remove them and resulting in a decrease in ionization energy.