Structure & Bonding (Double) quiz

1. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of water (H₂O), how many electrons should be shown in areas 1, 2, 3 and 4?

There should be two electrons in each of areas 1 and 2, and zero electrons in areas 3 and 4.

There should be two electrons in each of areas 1 and 2, and zero electrons in areas 3 and 4. There should also be an additional 4 electrons around the outside of the oxygen atom.

There should be two electrons in each of areas 1 and 2, and two electrons in each of areas 3 and 4.

There should be four electrons in each of areas 1 and 2, and zero electrons in areas 3 and 4.

Question 1 of 12

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

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

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

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

Question 2 of 12

3. Explain why carbon dioxide gas, CO₂, is a gas at room temperature

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

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

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

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

Question 3 of 12

4. 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 4 of 12

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

Ionic

Covalent

Covalent or ionic

Metallic

Question 5 of 12

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

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

Question 6 of 12

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

Graphite has layers which can easily slide over each other

Graphite has delocalised electrons which can move

Graphite has positive ions which can move

Graphite has delocalised protons which can move

Question 7 of 12

8. Describe the formation of a covalent bond

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

The sharing of a single electron between two nuclei

The transfer of electrons from one atom to another

The sharing of a pair of electrons between two nuclei

Question 8 of 12

9. What holds ions together?

Ions are held together by a strong electrostatic attraction between the oppositely charged ions

Ions are held together by a strong electrostatic attraction between the similarly charged ions

Ions are held together by a strong magnetic attraction between the oppositely charged ions

Ions are held together by a strong electrostatic attraction between the shared pair of electrons and their nuclei

Question 9 of 12

10. Do ionic substances conduct electricity?

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

Only when molten

Yes, ionic substances always conduct electricity

No, ionic substances never conduct electricity

Question 10 of 12

11. Why is the melting point of a smaller molecule lower than that of a larger molecule?

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

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 more attractions between them. These take less energy to overcome.

Question 11 of 12

12. What is needed to complete this diagram to show the ionic bonding in potassium oxide, K₂O ?

1) eight electrons around the oxide (six dots and two cross) 2) A charge of +1 on the potassium and -2 on the oxide 3) A second oxide ion the same as the first

1) eight electrons around the oxide (six dots and two cross) 2) A charge of +1 on the potassium and -2 on the oxide 3) A second potassium ion the same as the first

1) eight electrons around the potassium (any combination of dots and one crosses) 2) A charge of +2 on the oxide and -1 on the potassium 3) A second potassium ion the same as the first

1) eight electrons around the oxide (six dots and two cross) 2) A charge of +2 on the potassium and -1 on the oxide 3) A second potassium ion the same as the first

Question 12 of 12

Structure & Bonding (Double) quiz

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