Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Unit
Principles of Chemistry
991 practice questions
Topics covered
- States of Matter102 practice questions
- Elements, Compounds and Mixtures69 practice questions
- Atomic Structure108 practice questions
- The Periodic Table103 practice questions
- Chemical Formulae, Equations and Calculations Part 119 practice questions
- Chemical Formulae, Equations and Calculations Part 2144 practice questions
- Ionic Bonding143 practice questions
- Covalent Bonding68 practice questions
- Metallic Bonding19 practice questions
- Electrolysis198 practice questions
Practice questions
681–690 of 991
Question 681
5 marks · Easy
Answer and see the solution →This question is about ionic bonding in magnesium oxide and aluminium nitride.
(a)[3 marks]Draw a dot-and-cross diagram to show the ionic bonding in magnesium oxide (MgO).
Include charges on the ions.
(b)[2 marks]Aluminium is in Group 3 and nitrogen is in Group 5.
Using your answer to part (a) as a guide, describe how ions are formed when aluminium reacts with nitrogen to form aluminium nitride (AlN).
Question 682
6 marks · Normal
Answer and see the solution →This question is about the bonding and formulae for lithium fluoride and calcium chloride.
(a)[2 marks]Draw a dot-and-cross diagram to show the ionic bonding in lithium fluoride.
(b)[2 marks]Explain, using ion charges, why the formula for calcium chloride is .
(c)[2 marks]Write the formula for ammonium sulfate.
Question 683
6 marks · Normal
Answer and see the solution →This question is about the bonding and formulae of calcium chloride and other ionic compounds.
(a)[3 marks]Draw a dot-and-cross diagram to show the ionic bonding in calcium chloride ().
(b)[1 mark]State the electronic configuration of a chloride ion.
(c)[2 marks]Write the formula for copper(II) nitrate.
Question 684
6 marks · Normal
Answer and see the solution →This question is about explaining ionic bonding using calcium chloride and applying rules to deduce formulae for ionic compounds.
(a)[3 marks]Explain, in terms of electron transfer and ion formation, how calcium chloride () forms from its elements.
(b)[2 marks]Sodium oxide is another ionic compound. Write its formula and justify your answer using the charges on the ions.
(c)[1 mark]Copper(II) sulfate contains Cu2+ and SO4^2− ions. Explain why the correct formula is CuSO4.
Question 685
6 marks · Normal
Answer and see the solution →This question is about calcium chloride and how to write the formula for ionic compounds.
(a)[3 marks]Draw a dot-and-cross diagram to show how the electrons are arranged in calcium chloride (CaCl₂). Clearly show all outer shell electrons and use a key to show electrons from different atoms.
(b)[3 marks]Magnesium reacts with oxygen to form magnesium oxide. Write the formula for magnesium oxide and explain how you worked it out.
Question 686
7 marks · Hard
Answer and see the solution →Sodium chloride (NaCl) is a typical ionic compound. The arrangement of ions in its structure and the structure's properties explain many features of ionic solids.
(a)[2 marks]Describe how the ions are arranged in the giant ionic lattice of sodium chloride.
(b)[2 marks]Explain why sodium chloride has a high melting point, referring to its structure.
(c)[2 marks]State one feature of the overall appearance of pure sodium chloride crystals and relate it to the arrangement of ions in its lattice.
(d)[1 mark]Give one other property (besides melting point) that is explained by the structure of giant ionic lattices, and state how the arrangement of ions accounts for it.
Question 687
7 marks · Hard
Answer and see the solution →Magnesium oxide (MgO) and sodium chloride (NaCl) both form giant ionic lattices, but their melting points are very different.
(a)[2 marks]Describe the structure of a giant ionic lattice, using magnesium oxide as an example.
(b)[3 marks]Explain why magnesium oxide has a much higher melting point than sodium chloride. Refer to the types of ions present and their charges.
(c)[2 marks]Both substances conduct electricity when molten but not when solid. State and explain why.
Question 688
8 marks · Hard
Answer and see the solution →Sodium chloride and magnesium oxide are both ionic compounds with giant ionic lattice structures.
(a)[4 marks]Describe, in terms of ions, the arrangement and structure of sodium chloride.
(b)[4 marks]Magnesium oxide, like sodium chloride, forms a giant ionic lattice, but in magnesium oxide every magnesium ion is Mg^{2+} and every oxide ion is O^{2-}. Magnesium oxide has a higher melting point than sodium chloride. Using your answer to part (a), explain why magnesium oxide has a higher melting point than sodium chloride.
Question 689
1 mark · Easy
Answer and see the solution →State the type of particles that are attracted to each other in a covalent bond.
Question 690
3 marks · Easy
Answer and see the solution →Chlorine exists as diatomic molecules ( Cl2 ).
(a)[2 marks]Draw a dot-and-cross diagram to show the covalent bonding in a molecule of chlorine (Cl2).
(b)[1 mark]How many electrons are shared between the two chlorine atoms?