Structure & Bonding (Double) quiz

1. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of ethene (C₂H₄), how many electrons should be shown in areas 1, 2, 3, 4, and 5?

There should be four electrons in each of areas 1, 2, 3, 4 and 5

There should be four electrons in each of areas 1, 2, 3 and 4, and two electrons in area 5

There should be two electrons in each of areas 1, 2, 3 and 4, and four electrons in area 5

There should be two electrons in each of areas 1, 2, 3, 4 and 5

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 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

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

Question 2 of 12

3. Do ionic substances conduct electricity?

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

Yes, ionic substances always conduct electricity

Only when molten

No, ionic substances never conduct electricity

Question 3 of 12

4. Explain why magnesium oxide has a higher melting point than sodium chloride.

Magnesium and oxygen are more reactive elements

Sodium chloride is a simple molecular substance so there are only weak intermolecular forces which require little energy to break

Mg²⁺ and O²⁻ ions are larger than sodium and chloride therefore the electrostatic forces between the ions are much stronger. This requires more energy to break.

Mg²⁺ and O²⁻ ions have a higher charge than sodium and chloride therefore the electrostatic forces between the ions are much stronger. This requires more energy to break.

Question 4 of 12

5. Typically, do covalent substances conduct electricity?

No

Yes

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

Depends on the substance

Question 5 of 12

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

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

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 strong covalent bonds which require a lot of energy to overcome

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

Question 6 of 12

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

Graphite has delocalised protons which can move

Graphite has positive ions which can move

Graphite has layers which can easily slide over each other

Graphite has delocalised electrons which can move

Question 7 of 12

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

V²⁺ and O²⁻

There are no ions because it is covalent

V⁵⁺ and O²⁻

V⁺ and O⁻

Question 8 of 12

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

A shared pair of electrons is attracted to 2 nuclei

A single electron is transferred from bromine to hydrogen

A shared pair of electrons is attracted to one nucleus

A pair of electrons is transferred from bromine to hydrogen

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 sharing of a single electron between two nuclei

The transfer of electrons from one atom to another

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

The sharing of a pair of electrons between two nuclei

Question 11 of 12

12. Explain the term ionic bond

An ionic bond is the strong electrostatic attraction between oppositely charged ions

An ionic bond is the strong electrostatic attraction between similarly charged ions

An ionic bond is the strong magnetic attraction between oppositely charged ions

An ionic bond is the strong electrostatic attraction between a shared pair of electrons and two nuclei

Question 12 of 12

Structure & Bonding (Double) quiz

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