Redox reactions and reactivity of Group 2 Metals

Question 1

What makes an Element a Group 2 Metal?

Answer 1

When the outer shell contains only two electrons

Question 2

What do all Group 2 Metals have in common?

Answer 2

They all have two electrons on their outer shell
They all can only from a 2+ ion
They all lie in the s2 orbital

Question 3

What pattern does the group display?

Answer 3

They get more reactive as they go down the periods - as shielding increases

Question 4

The relative reactivities of the Group 2 elements Mg → Ba shown by their redox reactions with: OXYGEN

Answer 4

Group 2 Metal + Oxygen → White Ionic Metal Oxide

                            M(s) + O2(g) → MO(s)

The metal is Oxidised from Oxidation No. 0 to +2

The Oxygen is Reduced from Oxidation No. 0 to -2

Question 5

The relative reactivities of the Group 2 elements Mg → Ba shown by their redox reactions with:
WATER

Answer 5

Group 2 metal + Water → Metal Hydroxide + Hydrogen

                            M(s) + H2O(l) → M(OH)2(aq) + H2(g)
															They produce hydrogen and hydroxide

Question 6

The relative reactivities of the Group 2 elements Mg → Ba shown by their redox reactions with:
Dilute acid

Answer 6

Metal + Acid → Salt + Hydrogen
They produce salts and hydrogen gas, the reactivity increase down the group

Question 7

Reactivity down group 2

Answer 7

• Ionisation energy increase down the group
• This is because it is much easier to remove an outer shell electron as you go further down the group

Question 8

Reaction of group 2 compunds

Answer 8

Group 2 compounds are used to dilute highly acid conditions