Periodic Trends

Question 1

Atomic radius going across a period

Answer 1

Decreases, due to the same energy levels and the increase of protons in each atom which increases the nuclear charge by pulling the valence electrons in and resulting in a smaller electro cloud

Question 2

Atomic radius going down a group

Answer 2

Increases, the inner electrons shield the outer electrons from the positive charge of the nucleus, decreasing the effective nuclear charge lead to the electron electron repulsion increasing as the amount of electrons increase

Question 3

Ionic radius going down a group

Answer 3

Increases, more valence electrons are added, increasing the distance between the outer electrons that’s are being shielded by the inner electrons that weakens the nuclear pull on the outer electrons

Question 4

Ionic Radius going across a period

Answer 4

Decreases,the effective nuclear charge increases, resulting in a stronger attraction that the nuclear has with the outer electrons

Question 5

Ionization Energy going down a group

Answer 5

Decreases, outer electrons are farther from nucleus and are shielded by inner electrons thus the hold on the electrons are less strong

Question 6

Ionization Energy going across a period

Answer 6

Increases, increase of effective nuclear charge which means the nucleus has a stronger hold

Question 7

Electron affinity going down a group

Answer 7

Decreases, P+ and e- are farther away and attractive force between the nucleus and new electrons decrease

Question 8

Electron affinity going across a period

Answer 8

Increases, attractive force between nucleus and new electron increase

Question 9

Electronegativity going across a period

Answer 9

Increases, atomic radius decrease and distance between nucleus and electrons decrease this the attraction between P+ and e- increase

Question 10

Electronegativity going down a group

Answer 10

Decreases, distance between nucleus and bond electrons increase this attraction between P+ and e- decrease as there is more shielding