Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Chapter
Metallic Bonding
19 practice questions
Practice questions
11–19 of 19
Question 11
3 marks · Normal
Answer and see the solution →The melting point of magnesium (Group 2) is much higher than that of sodium (Group 1).
Using information about metallic bonding, calculate the number of delocalised electrons contributed per atom in each metal, and explain how this relates to their melting points.
Question 12
3 marks · Normal
Answer and see the solution →A student tries to represent a metallic lattice using the following statement:
'A metal is made up of separate molecules containing metal atoms.'
Does this statement accurately describe a metallic lattice? Give reasons for your answer, and describe the actual arrangement of particles in a metallic lattice.
Question 13
4 marks · Normal
Answer and see the solution →The table below shows data for three metals.
Properties of three metals Metal Ion formed Number of delocalised electrons per atom Melting point (°C) Sodium Na+ 1 98 Magnesium Mg2+ 2 650 Aluminium Al3+ 3 660 Use the data to answer the questions.
(a)[1 mark]For sodium, write the charge on the ion and state how many delocalised electrons each atom provides.
(b)[2 marks]Explain, using the table, why magnesium has a much higher melting point than sodium.
(c)[1 mark]Suggest, using the data, why aluminium and magnesium have similar melting points despite aluminium having a higher ion charge.
Question 14
1 mark · Normal
Answer and check →Which property of metals is directly explained by the presence of delocalised electrons in their structure?
- A.High density
- B.Shiny appearance
- C.Electrical conductivity
- D.High boiling point
Question 15
2 marks · Normal
Answer and see the solution →Calcium metal has a giant structure.
Draw and clearly label a simple 2D diagram to show the arrangement of ions and delocalised electrons in calcium metal.
Question 16
4 marks · Normal
Answer and see the solution →Read the paragraph and answer the questions.
Solid metals consist of positive metal ions in a sea of delocalised electrons. The bonding involves the electrostatic attraction between the ions and the electrons.
(a)[1 mark]Define metallic bonding.
(b)[1 mark]State what particles are involved in metallic bonding.
(c)[2 marks]Explain how metallic bonding holds the metal together.
Question 17
2 marks · Hard
Answer and see the solution →Explain, in terms of electrostatic forces, how metallic bonding holds a pure metal such as aluminium together. Your answer should refer specifically to the particles involved.
Question 18
5 marks · Hard
Answer and see the solution →Zinc is used to galvanise iron to prevent rusting because it is strong and resistant. Answer the following about the properties of zinc metal and its bonding.
(a)[2 marks]State and explain, in terms of metallic bonding, why zinc conducts electricity.
(b)[2 marks]Zinc can be hammered into thin sheets. Explain why this is possible, referring to its structure and bonding.
(c)[1 mark]Zinc has a high melting point. Explain this property in terms of attraction between its particles.
Question 19
2 marks · Hard
Answer and see the solution →Draw a simple 2D diagram to represent the arrangement of particles in a piece of barium metal. Clearly label the positive ions and the sea of delocalised electrons.