Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Chapter
Ionic Bonding
143 practice questions
Topics covered
- Ionic bonding in magnesium oxide19 practice questions
- Other examples of ionic bonding19 practice questions
- Calcium chloride19 practice questions
- Formulae for ionic compounds18 practice questions
- Giant ionic structures19 practice questions
- The physical properties of ionic substances19 practice questions
- The electrical conductivity of ionic substances19 practice questions
Practice questions
31–40 of 60 · Normal
Question 31
2 marks · Normal
Answer and see the solution →Write the formula for these ionic compounds:
(a)[1 mark]sodium phosphate
(b)[1 mark]calcium carbonate
Question 32
4 marks · Normal
Answer and see the solution →For each of the following, state the ions present, their charges, and the correct formula for the compound:
(a)potassium nitrate
(i)[1 mark]State the ions and their charges.
(ii)[1 mark]Write the formula for potassium nitrate.
(b)magnesium chloride
(i)[1 mark]State the ions and their charges.
(ii)[1 mark]Write the formula for magnesium chloride.
Question 33
2 marks · Normal
Answer and see the solution →Sodium chloride is an ionic compound with a giant lattice structure.
State TWO properties of sodium chloride that are linked to its giant ionic lattice, and briefly explain why the lattice causes each property.
(a)[2 marks](b)[0 marks]Question 34
4 marks · Normal
Answer and see the solution →Magnesium oxide (MgO) is a typical giant ionic compound.
(a)[1 mark]State the ions present in magnesium oxide.
(b)[2 marks]Explain why magnesium oxide has a very high melting point.
(c)[1 mark]Describe what happens to the ions when solid magnesium oxide melts.
Question 35
3 marks · Normal
Answer and see the solution →Explain why giant ionic structures conduct electricity when molten but do not conduct when solid.
Question 36
4 marks · Normal
Answer and see the solution →The table below gives the melting points and ability to conduct electricity in the solid and molten states for some ionic compounds:
Melting points and conductivity of ionic compounds Compound Melting point (°C) Conducts electricity when solid? Conducts electricity when molten? Sodium chloride 801 No Yes Magnesium oxide 2852 No Yes Potassium bromide 734 No Yes (a)[1 mark]Which compound has the highest melting point?
(b)[2 marks]Suggest a reason why all three compounds do not conduct when solid.
(c)[1 mark]What allows these compounds to conduct when molten?
Question 37
1 mark · Normal
Answer and check →Which property best explains why potassium chloride has a high melting point?
- A.It consists of molecules joined by covalent bonds.
- B.Its ions are arranged in layers that slide past each other.
- C.It is made of positive and negative ions held by strong electrostatic forces.
- D.It has delocalised electrons that conduct electricity.
Question 38
2 marks · Normal
Answer and see the solution →Describe the structure of a giant ionic compound and explain how this structure is linked to its melting point.
Question 39
4 marks · Normal
Answer and see the solution →Calcium chloride is an ionic compound with the formula CaCl_2.
(a)[1 mark]Name the ions present in calcium chloride.
(b)[2 marks]Explain why calcium chloride is soluble in water but does not conduct electricity when solid.
(c)[1 mark]What must happen for solid calcium chloride to conduct electricity?
Question 40
3 marks · Normal
Answer and see the solution →A student is comparing the melting points and electrical conductivity of two compounds: sodium chloride (NaCl) and magnesium oxide (MgO).
(a)[1 mark]Sodium chloride melts at around 801°C, while magnesium oxide melts at about 2852°C. Calculate the difference in melting points between these two ionic compounds.
(b)[2 marks]Explain, using the structure and bonding in giant ionic lattice structures, why magnesium oxide has a much higher melting point than sodium chloride.