Chem-Periodic Table & Trends

Question 1

Define Electronegativity and explain it’s trend:

Answer 1

• The pull of the nuclei on a neighbors electrons

- points toward “F”(Florine), which means it increases when an element is closer to “F” than farther away

Question 2

Define Ionization energy and it’s trend:

Answer 2

• Energy to remove the outer most electron
• The closer the electron is to the nucleus the harder it is to remove
• Moving across the periods/moving up in families = increase

Question 3

Define Atomic Radii and it’s trend:

Answer 3

• distance from the center of nucleus to the electron cloud

- Moving across the periods/moving up in families = decrease

Question 4

Define Periodic Law:

Answer 4

the regular repeating change in chemical properties as you move across a row in the periodic table

Question 5

What are the names for Group 1,2,17,and 18 on the periodic table?

Answer 5

• 1 = Alkali Metals
• 2 = Alkaline Earth metals
• 17 = Halogens
• 18 = noble gases

Question 6

What are the names for d-block, f-block, 1st and 2nd top row f-block n the periodic table?

Answer 6

• d-block = transition metals
• f-block = inner transition metals
• 1st row f-block = Lanthande
• 2nd row f-block = Actinide

Question 7

How can you tell if an element/group is more reactive than the other?

Answer 7

Depends on it’s atomic radii, so if element is more radioactive when it’s higher and/or more left on the periodic table.

Question 8

As atomic number increases across a period, atomic radii increases/decreases. Why?

Answer 8

• decreases

- more protons

Question 9

How can you tell if an element has a larger atomic radii than the other?

Answer 9

The atomic radii is bigger when moving down a family and/or moving behind on a row.

Question 10

How can you tell if an element has a larger electronegativity than the other?

Answer 10

Depends on how close it is to the element Florine(aka “F”), so the closer it is to said element, the higher the electronegativity.

Question 11

How can you tell if an element has a higher ionization energy than the other?

Answer 11

Depends on how small the atomic radii is, so ionization increases when moving across the period and/or moving up a family.

Question 12

As atomic number increases down a group, ionization energy increases/decreases. Why?

Answer 12

• decreases

- you have more shielding layers of electrons

Question 13

Define electronegativity:

Answer 13

the pull of one nucleus on a neighbors electron close

Question 14

What tends to have the highest electronegativity values?

-metals/nonmetals and why?+

Answer 14

• nonmetals

- smaller radius so nuclear charge extends beyond the cloud

Question 15

What tends to have the highest electronegativity values?

-metals/nonmetals and why?

Answer 15

• nonmetals

- smaller radius so nuclear charge extends beyond the cloud