Metallic bonding

Last updated: 04/02/2020

AQA A-Level Chemistry Bonding Metallic bonding

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Question 1 of 20

1. Question
What is the definition of metallic bonding?
- Attractions between positive ions and delocalised electrons
- Attractions between positive ions and negative ions
- Attractions between negative ions and delocalised electrons
- Atoms in a metal bonded together
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Question 2 of 20

2. Question
What is the definition of a metallic lattice?
- Delocalised electrons spread throughout the structure, surrounding fixed positive ions leaving a balanced charge
- Delocalised electrons spread throughout the structure, surrounding fixed negative ions leaving a balanced charge
- Delocalised negative ions spread throughout the structure, surrounding fixed negative ions leaving a negative charge
- Delocalised positive ions spread throughout the structure, surrounding fixed positive ions leaving a negative charge
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Question 3 of 20

3. Question
What is the definition of a delocalised electron?
- A free electron in a structure
- Shared electrons
- A transferred electron
- Electrons that cannot move freely
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Question 4 of 20

4. Question
What is the definition of a localised electron?
- Electrons that cannot move freely
- A transferred electron
- Shared electrons
- A free electron in a structure
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Question 5 of 20

5. Question
What is the definition of a cation?
- Positive ion
- An ion
- Negative ion
- Delocalised electron
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Question 6 of 20

6. Question
What is the definition of ductile?
- Substances that can be drawn out
- Substances can be hammered into different shapes
- Substances are very rigid
- Substances are very volatile
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Question 7 of 20

7. Question
What is the definition of malleable?
- Substances that can be hammered into different shapes
- Substances that contain high melting and boiling points
- Substances that are easily evaporated
- Substances that are very rigid
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Question 8 of 20

8. Question
Within a metal, how are atoms held together?
- Metallic bonding
- Ionic bonding
- Covalent bonding
- By strong intermolecular bonds
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Question 9 of 20

9. Question
Describe the movement of free electrons within a metal.
- Movement from negative to positive
- Equal distribution between positive and negative areas
- Random movement between charges
- Movement from positive to negative
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Question 10 of 20

10. Question
Why can metal ions slide past each other within the structure of a metal?
- The layers of metal ions can slide over each other
- The cations are small enough to slide past one another
- The free electrons enable movability
- The metal ions pass energy to each other
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Question 11 of 20

11. Question
Describe the melting and boiling points of compounds with giant metallic lattices.
- Melting point – high, boiling point – high
- Melting point – high, boiling point – low
- Melting point – low, boiling point – low
- Melting point – low, boiling point – high
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Question 12 of 20

12. Question
What happens to the melting and boiling points of a metal as the number of delocalised electrons increases?
- Melting and boiling points increase
- Melting and boiling points suddenly decrease
- Melting and boiling points decrease
- Nothing happens to the melting and boiling points
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Question 13 of 20

13. Question
Why do compounds with giant metallic lattices have high melting and boiling points?
- More energy is needed to overcome the strong attractions between the positive ions and negative delocalised electrons
- More energy is needed to overcome the strong attractions between the positive ions and negative ions
- More energy is needed to overcome the strong attractions between the negative ions and delocalised electrons
- More energy is needed to overcome the charge from the delocalised electrons
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Question 14 of 20

14. Question
Describe the electrical conductivity of compounds with giant metallic lattices.
- Conduct electricity
- Do not conduct electricity
- Only conducts electricity when molten
- Only conducts electricity when solid
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Question 15 of 20

15. Question
Why are compounds with giant metallic lattices good conductors of electricity?
- They contain free electrons
- They do not contain enough electronegativity
- They do not contain a charged particle
- There are no free particles to carry the charge
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Question 16 of 20

16. Question
Describe the solubility of compounds with giant metallic lattices.
- Insoluble, except in liquid metals
- Soluble in polar substances
- Soluble in non-polar substances
- Insoluble
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Question 17 of 20

17. Question
Which of the following properties do metals contain?
- They are ductile
- Low melting and boiling points
- Do not conduct electricity
- They are not very malleable
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Question 18 of 20

18. Question
Which of the following properties do metals contain?
- They are malleable
- They are not ductile
- Low melting and boiling points
- Only conducts electricity when solid
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Question 19 of 20

19. Question
Why are metals ductile?
- As they contain free electrons
- As they contain fixed negative ions
- As they can easily be melted
- As they contain fixed positive ions
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Question 20 of 20

20. Question
Why are metals malleable?
- As they contain free electrons
- As they contain fixed negative ions
- As they can easily be melted
- As they contain fixed positive ions
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