Part 4 – Bonding Structure and Properties
1. Write the chemical formula for the following molecules.
2. Which of the following 2 chemicals will be made up of molecules?
3.
(a) Explain what is meant by a diatomic molecule?
(b) Give three examples of diatomic elements.
4. Write the chemical formula for the following elements
5. Write the chemical formula for the following compounds
6. Write the chemical formula for the following compounds.
7. Draw the electron cloud diagrams to show how the electrons are shared in the following molecules.
(a) Hydrogen joined to carbon (b) Nitrogen joined to chlorine
(c) Hydrogen joined to oxygen (d) Nitrogen joined to nitrogen
8. Hence, write the chemical formula for the molecules in Q.7
9. Describe how the covalent bond holds the atoms together in a molecule of hydrogen chloride. Use a diagram to illustrate your answer.
11. Write chemical formula for following molecules:
12. For the following molecules,
(a) write the chemical formula (b) draw the shape.
13. Draw electron cloud diagrams to show how the following molecules form covalent bonds.
(a) Fluorine (b) Oxygen (c) Nitrogen
(d) Hydrogen iodide (e) Nitrogen hydride (f) Carbon hydride
14. Write chemical formula for the following
(a) Nitrogen (b) Aluminium (c) Hydrogen
(d) Chlorine (e) Bromine (f) Hydrogen oxide
(g) Carbon chloride (h) Nitrogen fluoride (i) Silicon bromide
(j) Silicon dioxide (k) Silicon tetraoxide (l) Dinitrogen tetraoxide
15. In a hydrogen molecule the atoms share 2 electrons in a covalent bond.
(a) Explain how the covalent bond holds the 2 hydrogen atoms together.
(b) The hydrogen molecule can be represented more simply as
(i) Showing all outer electrons, draw a similar diagram to represent a molecule of ammonia NH3.(ii) Draw another diagram to show the shape of an ammonia molecule.
16. Draw the true shapes for the following molecules:
(a) SiCl4 (b) H2S (c) NF3 (d) HCl (e) CH4
17.
(a) Name the charged particle that flows through metals when they conduct.
(b) Name a non-metal element that conducts electricity.
(c) Draw a labelled diagram of an experiment you would perform to test if a substance was an electrical conductor or insulator.
18. For the following compounds, state whether the bonding is ionic or covalent.
(a) Lithium iodide (b) Zinc oxide (c) Aluminium nitride
(d) Carbon chloride (e) Fluorine (f) Magnesium sulphide
(g) Nitrogen hydride
19.
(a) Which letter shows a non-metallic conductor?
(b) Which two letters show substances that never conduct?
(c) Which two letters shows a substance that conducts when solid?
(d) Which letter show a covalent compound?
(e) Which two letters show substances which could form an electrolyte?
(f) Which two letters show substances which conduct by movement of electrons?
20. During the electrolysis of a molten compound, the elements lead and chlorine were formed.
(a) What is meant by electrolysis?
(b) Name the compound being electrolysed.
(c) What type of bonding is present in this compound?
(d) Explain why the compound must be molten for electrolysis to work.
(e) At which electrode will the (i) lead (ii) chlorine be formed?
(f) Using page 7 of the data booklet, write ion electron equations for the formation of lead and chlorine.
21. Name the products at the (i) positive electrode (ii) negative electrode when melts of the following compounds are electrolysed:
(a) Lithium iodide (b) Calcium chloride (c) Zinc fluoride (d) Nickel bromide
22. Write ion electron equations for the following (use page 7 of the data booklet):
(a) forming copper from copper(II) ions
(b) forming lithium from lithium ions
(c) forming chlorine from chloride ions
(d) forming fluorine from fluoride ions
23. For the following compounds, suggest whether they will have (i) high melting points or (ii) low melting points
(a) Silver iodide (b) Carbon fluoride (c) Titanium oxide (d) Silicon bromide
24. Explain fully why:
(a) covalent compounds do not conduct electricity.
(b) metals conduct in the solid state.
(c) solid ionic compounds do not conduct.
(d) ionic compounds have very high melting points.
(e) carbon diamond has a high melting point.
25. Using sodium chloride and hydrogen chloride as examples, explain how an ionic bond and covalent bond are formed.
26. Copy and complete the following table
27. 
Which of the above ions has the same electron arrangement as neon?
28. Write formula, showing ions for the following compounds:
(a) Calcium oxide (b) Lithium bromide (c) Aluminium oxide
(d) Sodium sulphate (e) Magnesium hydroxide (f) Zinc (II) sulphide
(g) Lead (II) chloride (h) Silver (I) oxide (i) Copper (II) nitrate
(k) Ammonium nitrate (l) Potassium phosphate (m) Aluminium phosphate
29. Study the table opposite, and use the information to work out the expected colour of
(a) Nickel chloride
(b) Potassium dichromate
(c) Ammonium nitrate
(d) Ammonium nickel sulphate
