chemistry revision quiz

1. GCSE Chemistry Revision
Atomic structure, flame tests, bonding,
extraction of metals, testing for ions,
formula mass, percentage composition,
rates of reaction,

4. Starter
How many Protons, Neutrons and
Electrons do the following atoms contain?
Na Cl Ca
Draw the electron structure and write
the electron configuration

5. How would you carry out
a flame test?
What would you learn
from doing a flame test?

6. Element Colour of
Flame

8. What could you tell me about;
1. Group 1
2. Group 7
3. When Group 1 & 7 react

9. What would be the charge?
1.Lithium
2.Calcium
3.Aluminium
4.Iodine
5.Nitrogen

10. From the ions above work out the
formula of the following compounds;
Na+ Al3+ O2-
K+ Li+ S2-
Mg2+ Cl - NO3
-
Ca2+ Br - SO4
2-
1. Potassium Bromide 2. Magnesium Chloride
3. Aluminium Bromide 4. Calcium Oxide
5. Lithium Nitrate 6. Sodium Sulphate

11. What’s the formula?
Of the compound formed between;
1. Lithium and Bromine
2. Potassium and Fluorine
3. Magnesium and Bromine
4. Sodium and Oxygen
5. Calcium and Oxygen
6. Lithium and Nitrogen
7. Aluminium and Oxygen

12. Molecular Ions
Molecules which have a charge
Hydroxide
OH-
Nitrate
NO3
-
Sulphate
SO4
2-
Carbonate
CO3
2-

13. Molecular Ions
What would be the formula of;
1. Lithium Hydroxide
2. Potassium Nitrate
3. Potassium Sulphate
4. Calcium Carbonate
5. Sodium Carbonate Hydroxide
OH-
Nitrate
NO3
-
Sulphate
SO4
2-
Carbonate
CO3
2-

14. Should Hydrogen be in
group 1?
Use your understanding of the
periodic table to evaluate the
properties of Hydrogen

15. Showing the shared pair of electrons
Orbitals overlap
Atoms share electrons to complete their outer shell –
both have 8

16. A Covalent
Bond is a
Shared Pair Of
Electrons
Non Metals share electrons to form covalent
bonds
They have a full outer shell
Covalent bonds are strong physical bonds
Orbitals Overlap, and electrons are
inside the overlap

17. Dot And Cross Diagrams
(Showing Covalent Bonding)
A Covalent Bond
is a shared Pair
Of Electrons
Dots are
electrons from
Hydrogens
Crosses are
electrons from
Carbon
Electrons In
Orbital Overlap

18. Regular arrangement of metal ions
Positively charged metal ions
‘sea’ of electrons surrounding the ions
Properties?

19. • Metallic bonding is strong bonding.
• Each metal atom contributes one or two electrons
to a shared ‘sea’ of electrons.
• The shared bonding electrons can move through
the whole metal structure, so metals conduct.
Metallic Bonding

20. Attraction between
positive and negative ions
Small molecules with a few
covalent bonds
Lots of atoms bonded
together by strong physical
bonds
Positive ions surrounded by
a sea of electrons
High Mpt
Soluble in
H2O
Doesn’t
conduct as
solid, but
does as liquid
Low Mpt
Soluble in
H2O
Doesn’t
conduct as
solid, or liquid
High Mpt
Insoluble
Conducts as
solid
High Mpt
Insoluble
Doesn’t
conduct as
solid or liquid

21. What tests could you
carry out that would help
you to determine the
bonding type of a
substance?

22. Attraction between
positive and negative ions
Small molecules with a few
covalent bonds
Lots of atoms bonded
together by strong physical
bonds
Positive ions surrounded by
a sea of electrons
High Mpt
Soluble in
H2O
Doesn’t
conduct as
solid, but
does as liquid
Low Mpt
Soluble in
H2O
Doesn’t
conduct as
solid, or liquid
High Mpt
Insoluble
Conducts as
solid
High Mpt
Insoluble
Doesn’t
conduct as
solid or liquid

24. Electrolysis of Aluminium
• Cathode equation:
– Al³⁺ + 3e⁻  Al
• Anode equation:
– 2O²⁻  O₂ – 4e⁻
• Overall equation:
– 2Al₂Oз (l)  4Al (l) + 3O₂ (g)
Aluminium oxide  aluminium + oxygen
+ +
Carbon Cathode
Carbon Anodes
+ +
Aluminium
Alumina + Cryolite
Aluminium out
Steel container
Back to Contents
Remember that
oxidation happens at
the anode and
reduction happens
at the cathode

25. Testing For Ions
• It’s important for Chemists to be able to identify
ions, and know chemical tests that will help them
work out what is in an unknown solution
• This is an introduction for you to experience some
of these tests, and the observations you would
make

26. Expected Results – Positive Ions
Positive ion solution
Positive ion solution and sodium
hydroxide solution
iron(II), Fe2+ green precipitate
iron(III), Fe3+ red-brown precipitate
copper(II),Cu2+ light blue precipitate
calcium, Ca2+ white precipitate
zinc , Zn2+
white precipitate dissolves in
excess sodium hydroxide solution
Solution A red-orange precipitate

27. Expected Observations – Negative Ions
Negative ion solution Result of test for ion
chloride, Cl white precipitate
bromide, Br cream precipitate
iodide, I yellow precipitate
sulfate, SO4
2 white precipitate
carbonate, CO3
2 bubbles of CO2 gas;
limewater turns cloudy
Solution A
white precipitate with
silver nitrate test

28. What’s the relative molecular mass?
1.CuSO4
2.K2SO4
3.Al2(OH)3
4.Lithium Hydroxide
5.Iron (II) Oxide
6.Sodium Carbonate
LiOH
FeO
Na2CO3

29. Key terms
Actual Yield
Theoretical Yield
Percentage Yield
Relative Molecular Mass
Do you know these?

30. Two key formulas
% Yield =
Theoretical Yield
Actual Yield
X 100
You need to know these

31. Which Ore Is Best?
You are in charge of a Blast Furnace and have two
choices of ore to use. The question is, which one is
best?
Which Ore has the highest percentage of Iron?
FeO Fe2O3
Method;
Relative mass of metal
x 100
Relative mass of compound
Iron (II) Oxide Iron (III) Oxide

32. How much would you get?
If we had 100g of Iron (II) Oxide, how much Iron
could we extract?
STEP 1;
Write a balanced equation
STEP 2;
Mass Reactant = Mass Product
Relative Mass Relative Mass
Reactant Product

33. What factors affect the rate of
a chemical reaction?

34. What factors affect the rate of
a chemical reaction?

35. What factors affect the rate of
a chemical reaction?

36. Collision Theory?

37. Collision Theory?

38. Collision Theory?

39. How would you know
that a chemical reaction
is taking place?
Be prepared to give an answer!

40. What is a catalyst and what do
catalysts do?

41. What is collision theory?

42. Why is it important to control the
rate of reaction of a chemical
reaction?