Structure & Bonding (Double) quiz

1. 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 1 of 12

2. Explain what is meant by electric current

The rate of flow of electrons only

The rate of flow of ions only

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

The rate of flow of elephants

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 a nucleus

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

Strong electrostatic attraction between oppositely charged ions

Question 3 of 12

4. Explain the term ionic bond

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 oppositely charged ions

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

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 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

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

Question 5 of 12

6. 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 weak intermolecular forces that require little energy to overcome

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

Question 6 of 12

7. When can ionic substances conduct electricity?

Only when molten

In any state

Never

When molten or dissolved

Question 7 of 12

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

Carbon dioxide has a giant covalent structure with many weak covalent bonds which require little 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 strong intermolecular forces that require a lot of energy to overcome

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

Question 8 of 12

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

There are no ions because it is covalent

V⁺ and O⁻

V⁵⁺ and O²⁻

V²⁺ and O²⁻

Question 9 of 12

10. 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 10 of 12

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

Graphite has positive ions which can move

Graphite has delocalised electrons which can move

Graphite has layers which can easily slide over each other

Graphite has delocalised protons which can move

Question 11 of 12

12. 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 less 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.

Question 12 of 12

Structure & Bonding (Double) quiz

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