Structure & Bonding (Double) quiz

1. Explain, in terms of its structure, why graphite can act as a lubricant.

Graphite has strong forces of attraction between layers. These layers can slide over each other

Graphite is a smooth metal so creates a surface with little friction

Graphite has a low melting point so becomes liquid when heated by friction

Graphite has weak forces of attraction between layers. These layers can slide over each other

Question 1 of 12

2. When are ions attracted to each other?

When the ions are very small

When the ions are the same size

When the ions have the same charge

When the ions are oppositely charged

Question 2 of 12

3. Give the definition of a covalent bond

Strong electrostatic attraction between a postive ion and a sea of delocalised positive ions

Strong electrostatic attraction between a shared pair of electrons and two nuclei

Strong electrostatic attraction between a shared pair of electrons and a nucleus

Strong electrostatic attraction between oppositely charged ions

Question 3 of 12

4. Do ionic substances conduct electricity?

Only when molten

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

Yes, ionic substances always conduct electricity

No, ionic substances never conduct electricity

Question 4 of 12

5. Typically, do covalent substances conduct electricity?

Yes

Depends on conditions (e.g. pressure, temperature etc.)

Depends on the substance

No

Question 5 of 12

6. Describe the structure of an ionic compound, e.g NaCl

A giant structure held together by the attraction between similarly charged ions

A giant structure held together by the attraction between oppositely charged ions

A giant structure held together by the attraction between positive metal ions and a sea of delocalised electrons

A giant structure held together by intermolecular forces

Question 6 of 12

7. 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 four electrons in area 1, two electrons in area 2, and four 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 three electrons in area 1, four electrons in area 2, and three electrons in area 3

Question 7 of 12

8. State the fomula for the two ions in vanadium (V) oxide

V⁵⁺ and O²⁻

V²⁺ and O²⁻

V⁺ and O⁻

There are no ions because it is covalent

Question 8 of 12

9. 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 giant metallic structure with weak forces of attraction between layers

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

Question 9 of 12

10. Explain why nitrogen gas, N₂, is a gas at room temperature

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

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

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

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

Question 10 of 12

11. Describe the formation of a covalent bond

The sharing of a single electron between two nuclei

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

The transfer of electrons from one atom to another

The sharing of a pair of electrons between two nuclei

Question 11 of 12

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

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.

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.

Question 12 of 12

Structure & Bonding (Double) quiz

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