Structure & Bonding (Double) quiz

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

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

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

Question 1 of 12

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

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 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

Question 2 of 12

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

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

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

Question 3 of 12

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

A shared pair of electrons is attracted to 2 nuclei

A shared pair of electrons is attracted to one nucleus

A single electron is transferred from bromine to hydrogen

A pair of electrons is transferred from bromine to hydrogen

Question 4 of 12

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

There should be one electron in area 1, two electrons in area 2, and seven electrons in area 3

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

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

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

Question 5 of 12

6. Do ionic substances conduct electricity?

No, ionic substances never conduct electricity

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

Only when molten

Yes, ionic substances always conduct electricity

Question 6 of 12

7. 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 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

Question 7 of 12

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

Covalent or ionic

Covalent

Ionic

Metallic

Question 8 of 12

9. Why is the melting point of a smaller molecule lower than that of a larger 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 more attractions between them. These take less energy to overcome.

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

Question 9 of 12

10. Explain the term ionic bond

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

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

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

Question 10 of 12

11. 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 +2 on the potassium and -1 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 +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

Question 11 of 12

12. 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 12 of 12

Structure & Bonding (Double) quiz

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