Group 2

Question 1

Why does reactivity increase down the group?

Answer 1

Atomic Radius Increases

More shells → outer electrons are further from the nucleus.

Shielding Increases

More inner electron shells shield the outer electrons from the nucleus.

Nuclear Attraction Decreases

Despite increased nuclear charge, the effect is outweighed by shielding and distance.

Ionisation Energy Decreases

Easier to remove outer electrons → more reactive.
So, the easier it is to lose electrons, the more reactive the metal is.

Question 2

What are the observations when a Group 2 metal reacts with water?

Answer 2

Effervescence (H₂ gas)

Metal dissolves

Solution becomes alkaline

Question 3

Is the metal soluble?

Answer 3

No but its reaction products are.
Such as metal hydroxide.

Question 4

What are the observations when a Group 2 metal reacts with Oxygen?

Answer 4

Metal Oxide forms

Question 5

What are the observations when a Group 2 metal reacts with Acids?

Answer 5

For example, HCl,
Forms metal chloride plus Hydrogen

Question 6

Exam Tip
How would you go about explaining trends?

Answer 6

Using Atomic radius, Nuclear Attraction and Electron Shielding.

Question 7

Does 1st and 2nd ionisation energy increase or decrease down the group?

Answer 7

Decrease down the group.