Structure & Bonding (Double) quiz

1. When are ions attracted to each other?

When the ions are the same size

When the ions are very small

When the ions have the same charge

When the ions are oppositely charged

Question 1 of 12

2. Explain, in terms of its structure, why graphite can conduct electricity.

Graphite has delocalised electrons which can move

Graphite has layers which can easily slide over each other

Graphite has delocalised protons which can move

Graphite has positive ions which can move

Question 2 of 12

3. Why do ionic substance have high melting and boiling points?

There is a weak electrostatic attraction between oppositely charged ions, in a giant structure, which requires little energy to overcome

There is a strong electrostatic attraction between similarly charged ions, in a giant structure, which requires a lot of energy to overcome

There are weak intermolecular forces, in a simple molecular structure, which require little energy to overcome

There is a strong electrostatic attraction between oppositely charged ions, in a giant structure, which requires a lot of energy to overcome

Question 3 of 12

4. A substance is found not to conduct electricity even when molten. What type of bonding does the substance have?

Ionic

Covalent

Metallic

Covalent or ionic

Question 4 of 12

5. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of nitrogen (N₂), how many electrons should be shown in areas 1, 2 and 3?

There should be two electrons in area 1, four electrons in area 2, and two electrons in area 3

There should be three electrons in area 1, four electrons in area 2, and three electrons in area 3

There should be two electrons in area 1, six electrons in area 2, and two electrons in area 3

There should be four electrons in area 1, two electrons in area 2, and four electrons in area 3

Question 5 of 12

6. How can atoms get a full outer shell?

Conversion of electrons to protons

Either the transfer (covalent) or sharing (ionic) of electrons

Only transfer (ionic) of electrons

Either the transfer (ionic) or sharing (covalent) of electrons

Question 6 of 12

7. Do ionic substances conduct electricity?

No, ionic substances never conduct electricity

Not when solid, but they do when either molten or in solution

Yes, ionic substances always conduct electricity

Only when molten

Question 7 of 12

8. Explain why methane gas, CH₄, is a gas at room temperature

Methane has a simple molecular structure with strong intermolecular forces that require a lot of energy to overcome

Methane has a giant covalent structure with many weak covalent bonds which require little energy to overcome

Methane has a simple molecular structure with weak intermolecular forces that require little energy to overcome

Methane has a giant covalent structure with many strong covalent bonds which require a lot of energy to overcome

Question 8 of 12

9. Suggest why buckminsterfullerene, C₆₀, has a low melting point.

Buckminsterfullerene has a simple molecular structure with strong intermolecular forces that require a lot of energy to overcome

Buckminsterfullerene has a giant metallic structure with weak forces of attraction between layers

Buckminsterfullerene has a simple molecular structure with weak intermolecular forces that require little energy to overcome

Buckminsterfullerene has a giant covalent structure with many strong covalent bonds that need a lot of energy to break

Question 9 of 12

10. Why is the boiling point of a larger molecule higher than that of a smaller molecule?

Larger molecules have more attractions between them. These take more energy to overcome.

Larger molecules have fewer attractions between them. These take more energy to overcome.

Larger molecules have fewer attractions between them. These take less energy to overcome.

Larger molecules have more attractions between them. These take less energy to overcome.

Question 10 of 12

11. Describe the formation of a covalent bond

The electrostatic attraction between positive metal ions and a sea of delocalised electrons

The sharing of a pair of electrons between two nuclei

The transfer of electrons from one atom to another

The sharing of a single electron between two nuclei

Question 11 of 12

12. Explain how the atoms are held together in a hydrogen bromide molecule

A pair of electrons is transferred from bromine to hydrogen

A shared pair of electrons is attracted to one nucleus

A single electron is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

Question 12 of 12

Structure & Bonding (Double) quiz

Structure & Bonding (Double) quiz

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