C02.6 Periodicity Pt 2 Lecture

Increasing the charge of the particles

Decreasing the distance between the charges

Decreasing the charge of the particles

Increasing the distance between the charges

From right to left and top to bottom

From left to right and bottom to top

From top to bottom and left to right

From right to left and bottom to top

Yes

No

Element X

IE = 450 kJ/mol

Element Y

IE = 325 kJ/mol

F

I

Ionization energy increases from left to right due to increasing nuclear charge.

Ionization energy decreases from left to right due to decreasing atomic size.

Ionization energy remains constant across a period.

Ionization energy decreases due to increasing electron shielding.

Cs

Hg

Sr

P

Element W

EA = -450 kJ/mol

Element Z

EA = -325 kJ/mol

Ionization energy decreases down a group.

Atoms get smaller down a group.

Valence electrons move closer to the nucleus down a group.

Elements further down a group lose electrons easier.

Li and Be

O and F

Ne and He

C and N

They have the lowest ionization energies.

They have the highest ionization energies.

They have full electron shells.

They are nonmetals.

as electron affinity increases the likelihood that an electron will be gained also increases

as electron affinity increases the likelihood that an electron will be gained decreases

electron affinity has no affect on the gaining of electrons only the amount of energy change

electron affinity decreases L to R across a row

electron affinity increases L to R across a row

electron affinity does not change across a row

electron affinity goes up and down across a row

Li and Be

O and F

Ne and He

C and N

Na

H

O

Se

Al

Sodium

Magnesium

Aluminum

Zinc