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
91–100 of 143
Question 91
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.
Question 92
2 marks · Hard
Answer and see the solution →Lead(II) bromide (PbBr_2) is an example of a giant ionic compound. Explain why solid lead(II) bromide does not conduct electricity, but molten lead(II) bromide does.
Question 93
5 marks · Hard
Answer and see the solution →Sodium sulfide (Na_2S) and aluminium oxide (Al_2O_3) are both giant ionic compounds.
(a)[2 marks]Describe the arrangement of ions in the lattice of a giant ionic compound.
(b)[3 marks]Explain, using your knowledge of structure, why the melting point of aluminium oxide is much higher than that of sodium sulfide.
Question 94
2 marks · Hard
Answer and see the solution →State and explain whether potassium iodide (KI) has a high or low melting point. Refer to its structure in your answer.
Question 95
1 mark · Easy
Answer and see the solution →State why crystals of sodium chloride have a regular shape.
Question 96
3 marks · Easy
Answer and see the solution →(a)[1 mark]Name the two types of ions found in sodium chloride.
(b)[1 mark]Describe the arrangement of ions around a single sodium ion in the lattice.
(c)[1 mark]State whether sodium chloride exists as molecules or as a giant ionic lattice.
Question 97
2 marks · Easy
Answer and see the solution →Ionic compounds often form crystals. Explain why the crystalline property is linked to the structure of their ions.
Question 98
3 marks · Easy
Answer and see the solution →The table shows part of the arrangement of ions around a sodium ion in sodium chloride:
Ion Count Distance from central sodium ion (pm) Chloride ion 6 280 Sodium ion 12 400 Chloride ion 8 490 (a)[1 mark]What type of lattice is formed by sodium chloride?
(b)[1 mark]How many chloride ions are nearest to each sodium ion?
(c)[1 mark]Describe how the pattern of ions continues in the lattice.
Question 99
1 mark · Easy
Answer and see the solution →State why ionic compounds such as sodium chloride have high melting points.
Question 100
3 marks · Easy
Answer and see the solution →(a)[1 mark]What does it mean if a substance is described as 'crystalline'?
(b)[2 marks]Explain how the structure of sodium chloride leads to its crystalline appearance.