Periodic Trends: Ionization Energy

Multiple Select

Which factors influence the ionization energy of an atom?

• Distance between valence electron and nucleus

• Effective nuclear charge (# of protons)

• Number of neutrons

• Type of chemical bond

Multiple Choice

Which of the following best describes ionization energy?

• The energy required to remove an electron from a gaseous atom

• The energy released when an electron is added to an atom

• The energy required to split a nucleus

• The energy released during chemical bonding

Open Ended

Explain how the distance between the valence electron and the nucleus affects ionization energy.

Multiple Choice

Which of the following best describes the trend in ionization energy as more electrons are removed from an atom?

• Ionization energy decreases with each electron removed.

• Ionization energy remains the same for each electron removed.

• Ionization energy increases with each electron removed.

• Ionization energy fluctuates randomly.

Open Ended

Why does it require more energy to remove a 2nd or 3rd electron compared to the first electron from an atom?

Multiple Choice

Which of the following statements about ionization energy trends across the periodic table is correct?

• Ionization energy increases down a group and decreases across a period.

• Ionization energy decreases down a group and increases across a period.

• Ionization energy increases both down a group and across a period.

• Ionization energy decreases both down a group and across a period.