Exam 2 Lecture

Question 1

How do you find atomic radius using the periodic table?

Answer 1

• Atomic radius increases as you move down a group (column) because additional electron shells are added, making the atom larger.
• Atomic radius decreases as you move from left to right across a period (row). This is due to increasing nuclear charge, which pulls electrons closer to the nucleus

Question 2

Based on their positions in the periodic table, predict which has the smallest atomic radius: Mg, Sr, Si, Cl, I

Answer 2

Cl

Question 3

Based on their positions in the periodic table, predict which has the largest atomic radius: Li, Rb, N, F, I.

Answer 3

Rb

Question 4

What is the trend in ionization energy on the periodic table?

Answer 4

• Ionization energy generally increases from left to right across a period. This is due to the increasing nuclear charge (more protons) which holds the electrons more tightly, making them harder to remove.
• Ionization energy generally decreases as you move down a group.

Question 5

Based on their positions in the periodic table, predict which has the largest first ionization energy: Mg, Ba, B, O, Te.

Answer 5

O

Question 6

Based on their positions in the periodic table, predict which has the smallest first ionization energy: Li, Cs, N, F, I.

Answer 6

Cs

Question 7

Based on their positions in the periodic table, rank the following atoms in order of increasing first ionization energy: F, Li, N, Rb

Answer 7

Rb, Li, N, F

Question 8

Based on their positions in the periodic table, rank the following atoms in order of increasing first ionization energy: Mg, O, S, Si

Answer 8

Mg, Si, S, O

Question 9

Based on their positions in the periodic table, list the following atoms in order of increasing radius: Mg, Ca, Rb, Cs.

Answer 9

Mg, Ca, Rb, Cs

Question 10

Based on their positions in the periodic table, list the following atoms in order of increasing radius: Sr, Ca,