Saint Ninian’s High School National 4/5 Chemistry
Chemical Changes and Structure Part 2 Bonding
1. (a) Use a diagram to show how two hydrogen atoms form a hydrogen molecule.
(b) Use the diagram to explain in your own words how a covalent bond is formed.
2. Draw diagrams to show how the outer electrons form covalent bonds in each of the
following molecules.
(a) Nitrogen hydride NH3
(b) Hydrogen oxide H2O
(c) Hydrogen bromide HBr
(d) Carbon hydride CH4
3. For each of the examples in question 2, draw and name the shape of the molecule.
4. Write the ionic formulae for the following compounds.
(a) Aluminium sulphide
(d) Calcium nitrate
(b) Sodium oxide
(e) Tin(II) Carbonate
(c) Magnesium fluoride
(f) Lithium bromide
(g) Copper (II) phosphate
(h) Potassium nitride
(i) Barium hydroxide
(j) Titanium (III) chloride
(k) Strontium nitrate
(l) Caesium phosphide
5. Which of the following substances will conduct electricity?
liquid tin, solid copper chloride, liquid bromine, liquid magnesium iodide
liquid carbon chloride, solid sulphur, molten copper sulphate, solid zinc
6. a) Use your data booklet to give the melting points of sulphur dioxide and silicon
dioxide.
b) Explain why there is such a difference in the values by outlining the bonding
present in each compound.
7. Pupil A argued that the compound TiCl4 had ionic bonding because it was made from
a metal and a non-metal. Another pupil, B, argued that this was incorrect and that to
discover the bonding in TiCl4, certain chemical tests must be carried out. Using your
knowledge of chemistry describe which chemical tests could be carried out on TiCl4
to discover its bonding.
Saint Ninian’s High School National 4/5 Chemistry
Chemical Changes and Structure Part 2 Bonding
8. Aqueous copper chloride can be split up by passing electricity through it. The set up
for this process is shown below:
Chemical process
Positive
electrode
Negative
electrode
Aqueous copper chloride
(a) What name is given to this process?
(b) At which electrode would copper be formed? Explain your answer.
9. Which of the following compounds are made up of molecules.
Sodium bromide carbon dioxide phosphorus trichloride
Tin oxide lithium hydroxide sulphur fluoride
10. Name the seven elements that exist as diatomic molecules.
11. Look at the following reaction that produces uranium hexafluoride.
UF4 (s) + F2 (g)  UF6 (g)
Explain what type of bonding will be present in uranium hexafluoride.
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