Structure & Bonding (Double) quiz

1. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of methane (CH₄), how many electrons should be shown in areas 1, 2, 3, and 4?

There should be two electrons in each of the areas 1, 2, 3 and 4, and an additional 6 electrons around the outside of each hydrogen atom

There should be one electron in each of the areas 1, 2, 3 and 4

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

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

Question 1 of 12

2. 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 strong covalent bonds which require a lot of 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 weak covalent bonds which require little energy to overcome

Question 2 of 12

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

A shared pair of electrons is attracted to 2 nuclei

A pair of electrons is transferred from bromine to hydrogen

A single electron is transferred from bromine to hydrogen

A shared pair of electrons is attracted to one nucleus

Question 3 of 12

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

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

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

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

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

Question 4 of 12

5. Do larger molecules have higher or lower boiling points than smaller molecules?

Lower

Higher

Size doesn\'t affect boiling point

It depends on which atoms are present

Question 5 of 12

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

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

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

Question 6 of 12

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

Covalent or ionic

Metallic

Covalent

Ionic

Question 7 of 12

8. Explain, in terms of structure and bonding, why sodium chloride has a very high melting point

NaCl has a giant ionic structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to break

NaCl has a giant ionic structure with weak electrostatic forces between oppositely charged ions that require little energy to break

NaCl has a simple molecular structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to break

NaCl has a simple molecular structure with weak intermolecular forces that require little energy to break

Question 8 of 12

9. When are ions attracted to each other?

When the ions have the same charge

When the ions are oppositely charged

When the ions are the same size

When the ions are very small

Question 9 of 12

10. When can ionic substances conduct electricity?

Never

When molten or dissolved

In any state

Only when molten

Question 10 of 12

11. Describe the formation of a covalent bond

The sharing of a single electron between two nuclei

The sharing of a pair of electrons 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

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 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 +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 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

Structure & Bonding (Double) quiz

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