Structure & Bonding (Double) quiz

1. Typically, do covalent substances conduct electricity?

Yes

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

No

Depends on the substance

Question 1 of 12

2. Give the definition of a covalent bond

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

Strong electrostatic attraction between oppositely charged ions

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

Question 2 of 12

3. Describe the formation of a covalent bond

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

The sharing of a pair of electrons between two nuclei

The transfer of electrons from one atom to another

The sharing of a single electron between two nuclei

Question 3 of 12

4. 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 delocalised electrons which can move

Graphite has layers which can easily slide over each other

Question 4 of 12

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

Any state

Solid or liquid

Gas or liquid

Solid

Question 5 of 12

6. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of water (H₂O), how many electrons should be shown in areas 1, 2, 3 and 4?

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

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

There should be two electrons in each of areas 1 and 2, and zero electrons in areas 3 and 4. There should also be an additional 4 electrons around the outside of the oxygen atom.

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

Question 6 of 12

7. What holds ions together?

Ions are held together by a strong electrostatic attraction between the similarly charged ions

Ions are held together by a strong magnetic attraction between the oppositely charged ions

Ions are held together by a strong electrostatic attraction between the shared pair of electrons and their nuclei

Ions are held together by a strong electrostatic attraction between the oppositely charged ions

Question 7 of 12

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

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.

Magnesium and oxygen are more reactive elements

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

V⁵⁺ and O²⁻

V²⁺ and O²⁻

There are no ions because it is covalent

V⁺ and O⁻

Question 10 of 12

11. When can ionic substances conduct electricity?

Never

Only when molten

When molten or dissolved

In any state

Question 11 of 12

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

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

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

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

Question 12 of 12

Structure & Bonding (Double) quiz

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