Periodic Trends

Question 1

Define atomic radius

Answer 1

The distance from the nucleus to the valence electrons

Question 2

Explain how the atomic radius changes as your go down a group on the periodic table

Answer 2

It gets bigger

Question 3

Explain why the atomic radius changes like that

Answer 3

You add more energy levels as you go down the periodic table, so the valence electrons get farther away from the nucleus causing a larger atomic radius

Question 4

Explain how the atomic radius changes as you go across a period on the periodic table

Answer 4

It gets smaller

Question 5

Explain why the atomic radius changes this way (across row question)

Answer 5

More protons are added to the nucleus as you go from the left to right, giving the nucleus a stronger positive charge. This pulls the electrons closer to the nucleus

Question 6

Define ionization energy

Answer 6

The energy needed to remove an electron

Question 7

Explain how the ionization energy changes as you go down q group on the periodic table

Answer 7

It decreases-is easier to remove electrons

Question 8

Explain why the ionization energy changes like that

Answer 8

The electrons are farther away from the nucleus, so the protons have a weak hold on the electrons, making it easier to remove the electron

Question 9

Explain how the ionization energy changes as you go across a period on the periodic table

Answer 9

It increases-electrons become harder to remove

Question 10

Explain why the ionization energy changes this way (across one)

Answer 10

Since the electrons are closer to the nucleus, the protons have a strong hold on the electrons, making it harder to remove them

Question 11

Explain the connection between how the atomic radius and how the ionization energy changes going in the same direction on the periodic table

Answer 11

As atomic radius gets bigger, the ionization energy decreases. As atomic radius gets smaller, the ionization energy increases. The ionization energy is inversely proportional to the atomic radius

Question 12

Which elements have the highest and lowest ionization energy

Answer 12

Lowest: Francium / Highest: helium

Question 13

Define electronegativity

Answer 13

Measures the tendency of an atom to gain electrons to become stable

Question 14

Explain how the electronegativity changes as you go down a group on the periodic table

Answer 14

It decreases-is less likely

Question 15

Explain why the electronegativity changes like that

Answer 15

The outermost energy level is farther away from the nucleus, so there is less pull on it, meaning there would be a very weak pull on loose electrons

Question 16

Explain how the electronegativity changes as you go across a period on the periodic table

Answer 16

It increases-is more likely

Question 17

Explain why the electronegativity changes this way (across)

Answer 17

The outermost energy level is closer to electrons, so there is a strong pull, meaning loose electrons would be pulled into the elements electron cloud

Question 18

Explain the connection between how the atomic radius changes and how the electronegativity changes going in the same direction on the periodic table

Answer 18

Atomic radius increases top to bottom and electronegativity decreases top to bottom. Atomic radius decreases left to right and electronegativity increases left to right. Electronegativity is inversely proportional to atomic radius

Question 19

Explain the connection between how ionization energy changes and how the electronegativity changes going in the same direction on the periodic table

Answer 19

I.E. Increases left to right and EN increases left to right. I.E. decreases top to bottom and EN decreases top to bottom. I.E. is proportional to EN