Structure & Bonding (Double) quiz

1. If a substance has a simple molecular structure, what physical state might it be at room temperature?

Solid or liquid

Gas or liquid

Any state

Solid

Question 1 of 12

2. In the dot and cross diagram of the outer electrons showing the covalent bonding of ammonia (NH₃), how many electrons should be shown in areas 1, 2, 3 and 4?

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

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

There should be 2 electrons in each of the areas 1, 2, 3 but none in 4

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

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 one nucleus

A shared pair of electrons is attracted to 2 nuclei

A single electron is transferred from bromine to hydrogen

A pair of electrons is transferred from bromine to hydrogen

Question 3 of 12

4. Explain what is meant by electric current

The rate of flow of ions only

The rate of flow of elephants

The rate of flow of charged particles (e.g. of electrons or ions)

The rate of flow of electrons only

Question 4 of 12

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

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

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

Question 5 of 12

6. 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 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 6 of 12

7. Explain why Silica, SiO₂ is a solid with a high melting point

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

Silica has a giant metallic structure with weak forces of attraction between layers

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

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

Question 7 of 12

8. 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 +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

Question 8 of 12

9. When can ionic substances conduct electricity?

Never

When molten or dissolved

In any state

Only when molten

Question 9 of 12

10. When are ions attracted to each other?

When the ions have the same charge

When the ions are oppositely charged

When the ions are very small

When the ions are the same size

Question 10 of 12

11. Describe the formation of a covalent bond

The transfer of electrons from one atom to another

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

Question 11 of 12

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

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

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

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

Question 12 of 12

Structure & Bonding (Double) quiz

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