Ionization Energy and Atomic Structure

The video tutorial covers periodic trends, focusing on effective nuclear charge, shielding effect, atomic and ionic radii, ionization energy, electron affinity, and electronegativity. It explains how these factors influence atomic structure and behavior, using examples like lithium and beryllium. The tutorial also discusses Coulomb's Law and its application in atomic interactions, highlighting exceptions in ionization energy trends and the concept of successive ionization energies.

What is the effective nuclear charge for lithium?

• 0

• +2

• +1

• +3

How does the atomic radius change as you move across a period?

• Fluctuates

• Remains the same

• Decreases

• Increases

Why do metals become smaller when they form ions?

• They lose protons

• They gain protons

• They lose an energy level

• They gain electrons

What happens to ionization energy as you move down a group?

• Decreases

• Fluctuates

• Increases

• Remains constant

What does a negative electron affinity indicate?

• Atom loses electrons

• Energy is absorbed

• Atom is unstable

• Energy is released

Which element is likely to have a higher electronegativity?

• Metal

• Noble gas

• Alkali metal

• Nonmetal

According to Coulomb's law, what increases the force of attraction between two charged species?

• Decreasing charge

• Increasing distance

• Increasing charge

• Decreasing mass

Why is the ionization energy of nitrogen higher than that of oxygen?

• Oxygen is more stable

• Nitrogen has more protons

• Oxygen has paired electrons

• Nitrogen has fewer electrons

What happens to successive ionization energies as more electrons are removed?

• They fluctuate

• They decrease

• They increase

• They remain constant

Why does sodium have a much larger second ionization energy compared to the first?

• It becomes a noble gas

• It has a full energy level

• It loses a valence electron

• It gains an energy level