Question

use the periodic table and your knowledge of properties and periodic trends to answer the following questions.

1. ionization energy

a) define ionization energy.
b) what is the trend as you move down a group (column)?
c) what is the trend as you move across a period (row)?
d) which family of elements has the highest ionization energies?
e) which family of elements has the lowest ionization energies?

Explanation:

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. As you move down a group (column) in the periodic table, ionization energy generally decreases. This is because the outermost electrons are further from the nucleus and are shielded by more inner - shell electrons. As you move across a period (row), ionization energy generally increases. This is due to the increasing nuclear charge (number of protons) which attracts the electrons more strongly. The noble gas family has the highest ionization energies because they have a full valence shell and are very stable. The alkali metal family has the lowest ionization energies as they have one valence electron that is relatively easy to remove.

Answer:

a) Ionization energy is the energy required to remove an electron from a gaseous atom or ion.
b) Ionization energy generally decreases as you move down a group (column).
c) Ionization energy generally increases as you move across a period (row).
d) The noble gas family has the highest ionization energies.
e) The alkali metal family has the lowest ionization energies.