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Question 1

What happens to ionization energy across a period

Answer 1

It increases because effective nuclear charge (Z_eff) increases, pulling electrons closer.

Question 2

What is ionization energy (IE)

Answer 2

The energy required to remove an electron from an atom in the gas phase.

Question 3

Why does boron (B) have a lower ionization energy than beryllium (Be)?

Answer 3

The 2p electron in boron is farther from the nucleus than the 2s electron in Be, making it easier to remove.

Question 4

What is atomic radius?

Answer 4

Half the distance between the nuclei of two identical atoms

Question 5

What happens to atomic radius across a period

Answer 5

It decreases because Z_eff increases, pulling electrons closer to the nucleus.

Question 6

What happens to atomic radius down a group?

Answer 6

It increases because additional electron shells are added, making the atom larger.

Question 7

Which is larger: a cation or its neutral atom

Answer 7

The neutral atom is larger because the cation loses electrons, making it smaller.

Question 8

Which is larger: an anion or its neutral atom

Answer 8

The anion is larger because gaining electrons increases repulsion between electrons.

Question 9

What is effective nuclear charge (Z_eff)?

Answer 9

The net positive charge an electron experiences from the nucleus after accounting for shielding by inner electrons.

Question 10

What happens to ionization energy down a group

Answer 10

It decreases because outer electrons are farther from the nucleus and experience more shielding.