Ionization Energy and Atomic Structure

The video tutorial explains ionization energy, its trends across the periodic table, and the factors affecting it, such as atomic radius and force of attraction. It discusses the differences in ionization energies among elements like sodium, magnesium, and aluminum, highlighting the impact of noble gas configurations and the number of protons. The tutorial concludes with a review of key concepts, including ionic and atomic radii.

Why do noble gases have high ionization energy?

• They have a full valence shell.

• They are highly reactive.

• They have a low number of protons.

• They have a large atomic radius.

What happens to ionization energy as you move diagonally from bottom left to top right across the periodic table?

• It fluctuates randomly.

• It increases.

• It remains constant.

• It decreases.

How does the atomic radius affect the ionization energy of an element?

• Larger radius decreases ionization energy.

• Radius has no effect on ionization energy.

• Larger radius increases ionization energy.

• Smaller radius decreases ionization energy.

Why does sodium have a significant jump in ionization energy from the first to the second level?

• It achieves a noble gas configuration.

• Its atomic radius increases.

• It loses a proton.

• It gains an electron.

Why do alkaline earth metals have a higher ionization energy than alkali metals?

• They are more reactive.

• They have a smaller atomic radius.

• They have a larger atomic radius.

• They have more valence electrons.

Which element has a higher ionization energy due to a smaller ionic radius and more protons?

• Francium

• Lithium

• Magnesium

• Sodium

What is the relationship between the number of protons and ionization energy?

• Fewer protons increase ionization energy.

• Protons have no effect on ionization energy.

• More protons increase ionization energy.

• More protons decrease ionization energy.

Which factor contributes to the higher ionization energy of magnesium compared to sodium?

• More electron shielding

• Fewer protons

• Larger atomic radius

• Smaller ionic radius

What is the main reason for the large jump in ionization energy from the third to the fourth level in aluminum?

• Increase in atomic radius

• Decrease in proton count

• Achieving a noble gas configuration

• Increase in electron shielding

What happens to the radius of an anion when it gains electrons?

• The radius decreases.

• The radius remains the same.

• The radius increases.

• The radius fluctuates.