Structure & Bonding (Triple) quiz

1. Explain the term ionic bond

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

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

Question 1 of 20

2. Why do ionic compounds conduct electricity only when molten or in solution?

When solid the ions are arranged regularly. When molten or in solution the ions are arranged irregularly

When solid the electrons are held in place. When molten or in solution the electrons are free to move

When solid the ions are free to move. When molten or in solution the ions are held in place

When solid the ions are held in place. When molten or in solution the ions are free to move

Question 2 of 20

3. Describe the formation of a covalent bond

The transfer of electrons from one atom to another

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

The sharing of a pair of electrons between two nuclei

The sharing of a single electron between two nuclei

Question 3 of 20

4. Describe the bonding in a metal

The strong electrostatic attraction between a regular structure of positive ions and a sea of delocalised electrons

The strong electrostatic attraction between a shared pair of electrons and two nuclei

The strong electrostatic attraction between protons and neutrons

The strong electrostatic attraction between oppositely charged ions

Question 4 of 20

5. Give the definition of a covalent bond

Strong electrostatic attraction between a shared pair of electrons and a nucleus

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

Question 5 of 20

6. Explain why metals are malleable

Metals have strong covalent bonds which require a lot of energy to break

Metals have delocalised electrons which are free to move

Metals have layers of ions that can slide over each other

Metals have delocalised protons which can move

Question 6 of 20

7. Alloys contain different sized positive ions. What properties does this give alloys compared to pure metals?

Alloys are more ductile than pure metals

Alloys are harder and less malleable than pure metals

Alloys are more magnetic than pure metals

Alloys are harder and more magnetic than pure metals

Question 7 of 20

8. 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 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

NaCl has a giant ionic structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to break

Question 8 of 20

9. Why do covalent compounds (e.g H₂O) not conduct electricity?

There are weak intermolecular forces that require little energy to break

There are charged particles that are free to move

There are no charged particles that are free to move

There is a sea of delocalised electrons that are free to move

Question 9 of 20

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

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

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 10 of 20

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 delocalised protons which can move

Graphite has layers which can easily slide over each other

Question 11 of 20

12. 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 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

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

Question 12 of 20

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

V⁵⁺ and O²⁻

V²⁺ and O²⁻

V⁺ and O⁻

There are no ions because it is covalent

Question 13 of 20

14. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of chlorine (Cl₂), how many electrons should be shown in areas 1, 2 and 3?

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

There should be four electrons in area 2 and three in each of areas 1 and 3

There should be two electrons in area 2 and six in each of areas 1 and 3

There should be two electrons in area 2 and seven in each of areas 1 and 3

Question 14 of 20

15. State 3 properties that makes aluminium suitable for power cables

Ductile (can be drawn into a wire), bad conductor and low density

Ductile (can be drawn into a wire), good conductor and low density

Ductile (can be drawn into a wire), good conductor and light

Ductile (can be drawn into a wire), bad conductor and light

Question 15 of 20

16. What is an alloy?

An alloy is a mixture of a non-metal and one or more elements, usually other metals or carbon

An alloy is a mixture of a metal and one or more elements, usually other metals or carbon

An alloy is a mixture of a metal and one or more elements, usually other metals or hydrogen

An alloy is a mixture of a non-metal and one or more elements, usually other metals or hydrogen

Question 16 of 20

17. When can ionic substances conduct electricity?

In any state

When molten or dissolved

Never

Only when molten

Question 17 of 20

18. A student has drawn a diagram to show the structure of a metallic solid, but forgotten to label the parts. Which of the following correctly lists those parts?

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

Positive metal ions. Delocalised negative ions. Giant Structure.

Positive metal ions. Delocalised electrons. Giant Structure.

Oppositely charged ions in a sea of delocalised electrons. Giant structure.

Question 18 of 20

19. Do larger molecules have higher or lower boiling points than smaller molecules?

Lower

It depends on which atoms are present

Size doesn\'t affect boiling point

Higher

Question 19 of 20

20. Typically, do covalent substances conduct electricity?

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

Depends on the substance

No

Yes

Question 20 of 20

Structure & Bonding (Triple) quiz

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