1. Metals and Metal Compounds
KS3 Chemistry
Metals and Metal Compounds

2. 9E Metals and Metal Compounds
Contents
9E Metals and Metal Compounds
Metals and non-metals
Metals and acids
Metal compounds and acids
Symbol equations
Summary activities

3. Metal or non-metal? iron (Fe) iodine (I) antimony (Sb) phosphorus (P)
Is this element a or a ?
metal
non-metal
iodine (I)
sulfur (S)
magnesium (Mg)
antimony (Sb)
copper (Cu)
phosphorus (P)
iron (Fe)
Hard to say! H Li Na K Rb Cs Fr Be Sc Ti Mg V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Ca Kr Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Ra Rf Db Sg Bh Hs Mt ? Ac Al P N O S Cl F Ne Ar Rn I Si Xe He B C As Mg Mg P P S S Fe Fe Cu Cu
On this slide there are seven elements to be identified as metal or non-metal. Sb Sb I I

4. Metals and non-metals in the periodic table
The periodic table is a list of all the known elements which are arranged according to the similarities in their properties.
Metals are on the
left and in the centre.
Non-metals are mostly on the right. Xe
What type of elements are between metals and non-metals?

5. Metals and non-metals in the periodic table

6. Metal, non-metal or metalloid?
scandium (Sc)
francium (Fr)
cobalt (Co)
krypton (Kr)
silicon (Si)
metal
non-metal
metalloid
metal
metal
Which side are the metals on?
Which side are the non-metals on?
What are
metalloids? H Li Na K Rb Cs Fr Be Sc Ti Mg V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Ca Kr Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Ra Rf Db Sg Bh Hs Mt ? Ac Al P N O S Cl F Ne Ar Rn I Si Xe He B C As
On this slide there are five elements to be identified as metal, non-metal or metalloid.
Metals are on the left and in the centre.
Metalloids sometimes behave like metals and
sometimes like non-metals.
Non-metals are mostly
on the right.

7. What are the properties of metals?
malleable
(easy to bend)
shiny
solid
sonorous
(makes a sound)
good conductor of electricity
Properties of metals
dense
strong
high melting point
good conductor of heat
Point out the metal exceptions which do not display these properties, e.g. mercury, sodium.
ductile
(can be drawn into wires)
high boiling point
Do all metals have these properties?

8. Properties of metals and non-metals

9. Metals and non-metals – true or false?

10. Using metals
Can all metals do the same job?.

11. Using metals activity

12. 9E Metals and Metal Compounds
Contents
9E Metals and Metal Compounds
Metals and non-metals
Metals and acids
Metal compounds and acids
Symbol equations
Summary activities

13. Reaction of metals with acids
Many metals react with acids. When this happens the metal fizzes as bubbles are produced.
hydrogen
burning splint
What do the bubbles mean?
magnesium + acid
A gas is produced.
How can you test to find out if the gas produced is hydrogen?
Place a burning splint next to the mouth of test tube.
A ‘squeaky pop’ as the gas ignites shows that hydrogen is the gas produced in this reaction.

14. Reaction of metals with acids
When a metal reacts with an acid, the products are a salt and hydrogen gas.
metal
acid
sulfuric
acid
hydrochloric acid
nitric acid
metal
chloride
metal sulfate
metal
nitrate
salt
hydrogen
The salt produced depends on the metal and type of acid involved in the reaction:
When a metal reacts with hydrochloric acid, the salt produced is a metal chloride.
When a metal reacts with sulfuric acid, the salt produced is a metal sulfate.
When a metal reacts with nitric acid, the salt produced is a metal nitrate.

15. Complete the word equations
Complete the word equations for metals reacting with acid:
magnesium
nitric acid ?
magnesium nitrate
hydrogen
iron
sulfuric acid ?
iron sulfate
hydrogen
zinc
hydrochloric acid
zinc chloride ?
hydrogen ?
lead
sulfuric acid ?
lead sulfate
hydrogen

16. increasing reactivity
Reactivity of metals
Some metals react more vigorously with acids than others.
Metals can be listed in order of how reactive they are.
This list is called the reactivity series.
potassium
sodium
calcium
magnesium
aluminium
zinc
iron
lead
(hydrogen)
copper
silver
gold
The more reactive the metal, the more vigorous the reaction.
increasing reactivity
A metal that is below hydrogen will not react with dilute acids.

17. 9E Metals and Metal Compounds
Contents
9E Metals and Metal Compounds
Metals and non-metals
Metals and acids
Metal compounds and acids
Symbol equations
Summary activities

18. Reaction of metal carbonates with acids
When a metal carbonate reacts with an acid, it fizzes giving off carbon dioxide gas.
Carbon dioxide can be tested for using the limewater test.
When carbon dioxide gas is bubbled through limewater, it turns the limewater cloudy or milky white.
Most metal carbonates are not very soluble and so the reactions may be slow.

19. Reaction of metal carbonates with acids
When a metal carbonate reacts with an acid, the products are a salt, carbon dioxide and water.
metal carbonate
sulfuric
acid
nitric acid
acid
hydrochloricacid
metal nitrate
salt
metal sulfate
metal chloride
carbon dioxide
water
The salt produced depends on the metal carbonate and type of acid involved in the reaction:
When a metal carbonate reacts with hydrochloric acid, the salt produced is a metal chloride.
When a metal carbonate reacts with sulfuric acid, the salt produced is a metal sulfate.
When a metal carbonate reacts with nitric acid, the salt produced is a metal nitrate.

20. Complete the word equations
metal carbonate
acid
salt
carbon dioxide
water
Complete the word equation for each reaction between a metal carbonates and an acid:
sodium carbonate ?
nitric
acid
sodium nitrate ?
carbon dioxide
water ?
calcium carbonate
nitric
acid
calcium nitrate
carbon dioxide
water
zinc carbonate
sulfuric acid ?
zinc sulfate
carbon dioxide ? ?
water

21. Reaction of metal oxides with acids
When a metal oxide reacts with an acid, the products are a salt and water.
metal oxide
acid
salt
water
A metal oxide is a type of chemical called a base.
Bases are chemicals that react with an acid to produce a salt and water.
A base that is soluble in water is called an alkali.
Using the products as a clue, what is the reaction between a base (such as a metal oxide) and an acid called?
neutralization

22. Complete the word equations
metal oxide
acid
salt
water
Complete the word equation for each reaction between a metal oxide and an acid:
magnesium oxide
nitric acid ?
magnesium nitrate ?
water
zinc oxide
sulfuric acid ?
zinc
sulfate
water ?
iron oxide
hydrochloric acid
iron chloride ? ?
water

23. 9E Metals and Metal Compounds
Contents
9E Metals and Metal Compounds
Metals and non-metals
Metals and acids
Metal compounds and acids
Symbol equations
Summary activities

24. Chemical formulae – what is the ratio of atoms?
The name of a chemical can also be written as a formula.
A formula uses chemical symbols and numbers to show the ratio of atoms of each element present in the chemical.
Name of salt
Formula
Ratio of atoms in salt
calcium chloride
CaCl2 Ca Cl 1 2
sodium sulphate
Na2SO4 Na S O 2 1 4
magnesium sulphate
MgSO4 Mg S O 1 1 4
magnesium nitrate
Mg(NO3)2 Mg N O 1 2 6
calcium sulphate
CaSO4 Ca 1 S 1 O 4

25. What is the ratio of atoms in each salt?
Name of salt
Formula
Ratio of atoms in salt
sodium chloride
NaCl
1 Na
1 Cl
magnesium chloride
MgCl2
1 Mg
2 Cl
potassium nitrate
KNO3
1 K
1 N
3 O
potassium sulphate
K2SO4
2 K
1 S
4 O
calcium nitrate
Ca(NO3)2
1 Ca
2 N
6 O

26. Writing equations using chemical formulae
The names of chemicals in a word equation can be replaced with chemical formulae.
When a chemical reaction is written using chemical formulae, the equation must be balanced.
zinc
hydrogen
hydrochloric acid
zinc chloride
Zn HCl → ZnCl H2 2
1 Zn
1 H, 1 Cl
2 H, 2 Cl
1 Zn, 2 Cl
2 H
Write down the formula for each chemical.
Count the number of atoms on each side of the equation.
Where needed, adjust the numbers in front of the formula
so that the numbers of atoms on each side are balanced.

27. Writing and balancing chemical equations
Use chemical formulae to write a balanced chemical equation for the reaction between lead and hydrochloric acid.
lead
hydrochloric acid
lead chloride
hydrogen
Pb HCl → PbCl H2 2
Use chemical formulae to write a balanced chemical equation for the reaction between calcium oxide and hydrochloric acid.
calcium
hydrochloric acid
calcium chloride
hydrogen
Ca HCl → CaCl H2 2

28. Balancing equations activity

29. 9E Metals and Metal Compounds
Contents
9E Metals and Metal Compounds
Metals and non-metals
Metals and acids
Metal compounds and acids
Symbol equations
Summary activities

30. alkali – A soluble base.
Glossary
alkali – A soluble base.
base – A compound (such as a metal oxide) that reacts
with an acid to produce a salt and water.
conductor – A material that allows heat and electricity
to travel through it easily.
malleable – A material that can be hammered into shape.
metal – An element found on the left of the periodic table which is usually hard, shiny and a good conductor.
metal carbonate – A compound made of a metal, carbon and oxygen. It reacts with acid to produce a salt, carbon dioxide and water.
metal oxide – A compound made of a metal and oxygen.
It reacts with acid to produce a salt and water.
property – A characteristic of a material.

31. Anagrams

32. Multiple-choice quiz