metal reactions, OILRIG and transition metals

Question 1

Reactions of metals what would the products
of the reactions below be?

Metal + oxygen

Metal + water

Metal + steam

Metal + acid (hydrochloric acid or sulphuric acid)
e.g Copper + sulphuric acid

Answer 1

Metal + oxygen → metal oxide

Metal + water → Metal hydroxide + hydrogen

Metal + steam→ Metal oxide + hydrogen

Metal + acid (hydrochloric acid or sulphuric acid) → Salt + hydrogen

Copper + sulphuric acid→ Copper sulphate + hydrogen

Question 2

metal displacement reaction:
using this list work out:

1. sodium + Aluminium sulphate =
2. Zinc + magnesium oxide =
   3.Aluminium chloride + zinc =
3. Zinc sulphate + magnesium =
4. Lead oxide + Iron =
5. Iron sulphate + Tin =

Potassium (K)
Sodium (Na)
Calcium (Ca)
Magnesium (Mg)
Aluminum (Al)
Zinc (Zn)
Iron (Fe)
Tin (Sn)
Lead (Pb)
Hydrogen (H) (reference point for acids)
Copper (Cu)
Silver (Ag)
Gold (Au)

Answer 2

• sodium sulphate + aluminium
• no reaction zinc is less reactive than magnesium
  -no reaction
• magnesium sulphate+ zinc
• iron oxide + lead
• no reaction

Question 3

metal reactivity down a group:
As you go down the group, the reactivity..?

a. number of shells..?
b. atomic radius ?
c. Nuclear attraction .. which means?

Answer 3

increases
increases
increases
decreases which means its easier to lose an electron

Question 4

metal reactivity across a period

a. number of shells..?
b. atomic radius..?
c. nuclear attraction..? which means..?

Answer 4

a. stays the same
b. decreases
c. increases which means its harder to lose an electron

Question 5

explain the difference in reactivity of these metals with reference to their:
Potassium (K)
Sodium (Na)
Magnesium (Mg)
(magnesium least reactive and potassium most reactive)
a. position in periodic table
b. electronic configuration

Question 6

what does OILRIG stand for

Answer 6

oxidation
is
loss
reduction
is
gain

Question 7

how can you work out whether an element has been oxidised or reduced

Answer 7

Rule 1: If the oxidation state increases during a reaction the element has been oxidised (lost electrons)

Rule 2: If the oxidation state decreases during a reaction the element has been reduced (gained electrons)