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What happens to the number of energy levels when an electron is removed to form a cation?

It decreases.

How does the size of the cation compare to the same, neutral atom?

Smaller than the neutral atom.

What happens to the number of energy levels when an electron is added to form an anion?

It increases.

How does the size of the anion compare to the same, neutral atom?

Larger than the neutral atom.

What is ionization energy?

Energy required to remove an electron from a gaseous atom.

Why do smaller atoms have larger ionization energies?

Electrons are closer to the nucleus, resulting in stronger attraction.

Why do larger atoms have smaller ionization energies?

Electrons are farther from the nucleus, resulting in weaker attraction.

What is electronegativity?

An atom's ability to attract electrons in a chemical bond.

Describe the electronegativity pattern on the periodic table.

Increases left to right and bottom to top.

What are the common ion charge patterns in Groups 1, 2, 15, 16, & 17?

Group 1: +1, Group 2: +2, Group 15: -3, Group 16: -2, Group 17: -1.

Why don't we normally see ions from group 14?

They typically share electrons instead of gaining or losing.

Would you expect ionization energy to increase or decrease from left to right across a period?

Increase due to more valence electrons.

What does it mean that fluorine is the most electronegative element?

It strongly attracts electrons from other atoms in a bond.