1. Reaction with Metals - general
Many metals react with acids to form a salt and hydrogen gas.
The general word equation is:
metal +
acid 
a salt
hydrogen
The salt will depend upon the metal and the acid used.
Hydrochloric acid gives metal chlorides
Sulphuric acid gives metal sulphates
Nitric acid gives metal nitrates
So, for example
magnesium +
hydrochloricacid 
magnesium chloride +
hydrogen

2. Evidence of Reaction
Some of these reactions show bubbles being produced. These are bubbles of hydrogen gas. This proves that a reaction is taking place because a new substance is forming.
How do we test for hydrogen?
Oxygen in the air
hydrogen
Lighted spill
Mg + acid

3. Use the general equation to finish of the word equations below metal +
Activity
Use the general equation to finish of the word equations below
metal +
acid 
a salt
hydrogen
magnesium +
sulphuric acid 
magnesium sulphate
hydrogen
iron +
nitric acid 
iron nitrate
hydrogen
calcium +
sulphuric acid 
calcium sulphate
hydrogen
Zinc + hydrochloric 
acid
zinc chloride
hydrogen

4. React with Metals – Metal Reactivity
We can use the activity series of metals to predict how vigorously (if at all) a metal will react.
The more reactive the metal, the more vigorous the reaction.
The least reactive metals do not react at all.
Potassium
sodium
calcium
magnesium
aluminium
zinc
Iron
Lead
(Hydrogen)
copper
silver
gold
Decreasing activity
Which metal fits the description silver; potassium; iron
Explodes in acid
Bubbles slowly in warm acid
Doesn’t react
potassium
iron
silver

5. Formula of salts
Chemists often use formula equations to show not just what atoms are present but also how many.
To do this we need to understand what the numbers in a formula represent. Here are some examples.
Name of Salt
Formula
Contains
sodium chloride
NaCl
one Na
one Cl
magnesium chloride
MgCl2
one Mg
two Cl
potassium nitrate
KNO3
one K
one N
three O
potassium sulphate
K2SO4
two K
one S
four O
calcium nitrate
Ca(NO3)2
one Ca
two N
six O

6. How many of each type of atom does the formula of the salt represent?
Activity
How many of each type of atom does the formula of the salt represent?
Name of Salt
Formula
Contains
calcium chloride
CaCl2 Ca Cl
sodium sulphate
Na2SO4 Na S O
magnesium sulphate
MgSO4 Mg
magnesium nitrate
Mg(NO3)2 N
calcium sulphate
CaSO4
one
two
two
one
four
one
one
four
two
one
six
one
one
four

7. Neither H nor Cl balance.Need 2 HCl
Formula Equations:
Step 1: Write down the word equation.
Step 2: Replace words with the chemical formula . (You will be given or need to look up the formula at this stage.)
Step 3: Check that there are equal numbers of each type of atom on both sides of the equation. If not, then balance the equation by using more than one.
E.g. The reaction of magnesium with hydrochloric acid
magnesium +
hydrochloric acid 
magnesium chloride
hydrogen Mg +
HCl 
MgCl2 H2
Neither H nor Cl balance.Need 2 HCl Mg +
2HCl 
MgCl2 H2

8. Already balances; No change
Activity
Can you finish off the equations below:
Step 1: Write down the word equation.
Step 2: Replace words with the chemical formula.
Step 3: Balance the type of atom on both sides.
magnesium +
sulphuric acid 
magnesium sulphate
hydrogen Mg +
H2SO4 
MgSO4 H2
Already balances; No change
potassium +
sulphuric acid 
potassium sulphate
hydrogen K +
H2SO4 
K2SO4 H2
Need 2 K on both sides 2K +
H2SO4 
K2SO4 H2

9. Metals with Hydrochloric Acid
hydrochloric acid +
magnesium
magnesium chloride +
hydrogen Mg +
HCl 
MgCl2 H2 2 
hydrochloric acid +
copper
No reaction Cu +
HCl  - 2 
hydrochloric acid +
aluminium
aluminium chloride +
hydrogen Al +
HCl 
AlCl3 H2 2 6 2 3 
hydrochloric acid +
calcium
calcium chloride +
hydrogen Ca +
HCl 
CaCl2 H2 2

10. Metals with sulphuric and nitric Acid
sulphuric acid +
zinc
zinc sulphate +
hydrogen Zn +
H2SO4 
ZnSO4 H2  
nitric acid +
magnesium
magnesium nitrate +
hydrogen Mg +
HNO3 
Mg(NO3)2 H2 2 
nitric acid +
iron
iron nitrate +
hydrogen Fe +
HNO3 
Fe(NO3)3 H2 2 6 2 3 
sulphuric acid +
calcium
calcium sulphate +
hydrogen Ca +
H2SO4 
CaSO4 H2 

11. Metal oxide + acid  a salt + water
Metal oxides and acids
Metal oxide + acid  a salt + water
Most metal oxides are not soluble.
i.e. They are bases but not alkalis. This means they are often slower and may need heating to make them react
Acid
Oxide 
sulphuric acid +
Copper oxide
copper sulphate +
water

12. Metal oxide + acid  a salt + water
Metal oxides and acids
Metal oxide + acid  a salt + water 
sulphuric acid +
zinc oxide
zinc sulphate +
water
ZnO +
H2SO4 
ZnSO4
H2O 
hydrochloric acid +
sodium oxide
sodium chloride +
water
Na2O +
2HCl 
2NaCl
H2O 
nitric acid +
iron oxide
iron nitrate +
water
Fe2O3 +
3HNO3 
Fe(NO3)3
3H2O

13. Metal carbonates and acids
Metal carbonate + acid
 a salt + water + carbon dioxide
When metal carbonates react with acids they fizz giving off carbon dioxide gas.
Most metal carbonates are not very soluble and so reactions may be slow. 
hydrochloric acid +
calcium carbonate
calcium chloride +
water +
carbon dioxide

14. Metal carbonates and acids
Metal carbonate + acid  a salt + water + carbon dioxide +
zinc carbonate
sulphuric acid 
zinc sulphate +
water +
carbon dioxide
ZnCO3 +
H2SO4 
ZnSO4
H2O
CO2 +
sodium carbonate
hydrochloric acid 
sodium chloride +
water +
carbon dioxide
Na2CO3 +
2HCl 
2NaCl
H2O
CO2 +
nickel carbonate
nitric acid 
nickel nitrate +
water +
carbon dioxide
NiCO3 +
2HNO3 
Ni(NO3)2
H2O
CO2

15. Which of these is NOT a typical property of metals?
conduct
strong
dense
brittle

16. What is the symbol for Gold?Au Ag au

17. Which of the following elements is not a metal?
copper
lead
lithium
neon

18. Which of these is a salt?
Sodium carbonate
Sodium chloride
Sodium hydroxide
Sodium

19. Which of these do all acids contain?
Hydrogen
Sulphur
Oxygen
Nitrogen

20. Which of these salts might be formed from nitric acid?
Potassium chloride
Sodium nitride
Aluminium sulphate
Calcium nitrate

21. Which of these metals might not react with hot dilute acid?
Sodium
Calcium
Silver
Iron

22. Which of these substances would not neutralise an acid?
Silver nitrate
Sodium carbonate
Calcium oxide
Magnesium hydroxide

23. What number must replace X to balance the equation?
Fe(OH) X HCl  3H2O FeCl3 1 2 3 4

24. What number must replace X to balance the equation?
CaCO X H2SO4  H2O + CaSO CO2 1 2 3 4