Structure & Bonding (Double) quiz

1. Describe the formation of a covalent bond

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

The sharing of a single electron between two nuclei

The transfer of electrons from one atom to another

The sharing of a pair of electrons between two nuclei

Question 1 of 12

2. How can atoms get a full outer shell?

Either the transfer (ionic) or sharing (covalent) of electrons

Only transfer (ionic) of electrons

Conversion of electrons to protons

Either the transfer (covalent) or sharing (ionic) of electrons

Question 2 of 12

3. Give the definition of a covalent bond

Strong electrostatic attraction between oppositely charged ions

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

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 3 of 12

4. State the fomula for the two ions in iron (II) sulfide

Fe³⁺ and S³⁻

Fe²⁺ and S²⁻

Fe⁺ and S⁻

Fe³⁺ and S²⁻

Question 4 of 12

5. Explain, in terms of structure and bonding, why magnesium oxide has a higher melting point than sodium chloride

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.

Sodium chloride is a simple molecular substance so there are only weak intermolecular forces which require little energy to break

Magnesium and oxygen are more reactive elements

NaCl and MgO both have a giant ionic structure with strong electrostatic forces between oppositely charged ions. The Ions in MgO have a charge of 2 and -2, but in NaCl the charges are 1 and -1. So the bonds in MgO require more energy to break

Question 5 of 12

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

Graphite has delocalised electrons which can move

Graphite has layers which can easily slide over each other

Graphite has delocalised protons which can move

Graphite has positive ions which can move

Question 6 of 12

7. Typically, do covalent substances conduct electricity?

Yes

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

Depends on the substance

No

Question 7 of 12

8. 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 less energy to overcome.

Larger molecules have more 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 more energy to overcome.

Question 8 of 12

9. 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 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

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

Question 9 of 12

10. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of nitrogen (N₂), how many electrons should be shown in areas 1, 2 and 3?

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

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

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

There should be three electrons in area 1, four electrons in area 2, and three electrons in area 3

Question 10 of 12

11. When can ionic substances conduct electricity?

In any state

Only when molten

Never

When molten or dissolved

Question 11 of 12

12. Explain why methane gas, CH₄, is a gas at room temperature

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

Methane has a giant covalent structure with many weak covalent bonds which require little energy to overcome

Methane has a giant covalent structure with many strong covalent bonds which require a lot of energy to overcome

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

Question 12 of 12

Structure & Bonding (Double) quiz

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