Structure & Bonding (Triple) quiz

1. What is an alloy?

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 non-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 carbon

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

Question 1 of 20

2. Explain why nitrogen gas, N₂, is a gas at room temperature

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

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

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

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

Question 2 of 20

3. Do ionic substances conduct electricity?

Not when solid, but they do when either molten or in solution

Only when molten

No, ionic substances never conduct electricity

Yes, ionic substances always conduct electricity

Question 3 of 20

4. Explain why metals are good conductors of electricity

Metals have delocalised protons which can move

Metals have positive ions which can move

Metals have delocalised electrons which are free to move

Metals have layers of ions that can slide over each other

Question 4 of 20

5. Suggest why buckminsterfullerene, C₆₀, has a low melting point.

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

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

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

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

Question 5 of 20

6. 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 2 electrons in each of the areas 1, 2, 3 but none in 4

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

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

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

Question 6 of 20

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

There are weak intermolecular forces that require little energy to break

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

There are charged particles that are free to move

There are no charged particles that are free to move

Question 7 of 20

8. 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 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 8 of 20

9. 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 transfer of electrons from one atom to another

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

Question 9 of 20

10. 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. Giant Structure.

Positive metal ions. Delocalised negative ions. Giant Structure.

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

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

Question 10 of 20

11. Why do ionic substance have high melting and boiling points?

There is a weak electrostatic attraction between oppositely charged ions, in a giant structure, which requires little energy to overcome

There are weak intermolecular forces, in a simple molecular structure, which require little energy to overcome

There is a strong electrostatic attraction between oppositely charged ions, in a giant structure, which requires a lot of energy to overcome

There is a strong electrostatic attraction between similarly charged ions, in a giant structure, which requires a lot of energy to overcome

Question 11 of 20

12. Explain the term ionic bond

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

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

An ionic bond is the strong electrostatic attraction between similarly charged ions

Question 12 of 20

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

V⁵⁺ and O²⁻

There are no ions because it is covalent

V⁺ and O⁻

V²⁺ and O²⁻

Question 13 of 20

14. Describe the structure of metals

A simple regular structure of positive metal ions surrounded by a sea of delocalised electrons

A giant random structure of positive metal ions surrounded by a sea of delocalised electrons

A giant regular structure of positive metal ions surrounded by a sea of delocalised electrons

A simple random structure of positive metal ions surrounded by a sea of delocalised electrons

Question 14 of 20

15. Why are alloys harder than pure metals?

Alloys often contain carbon which is a very hard element

Alloys contain different sized positive ions, so there are no layers of ions to slide over each other

Alloys are more magnetic than pure metals so when they are formed the ions are packed closer together

Alloys have higher melting points because they are mixtures so are harder

Question 15 of 20

16. Explain how the atoms are held together in a hydrogen bromide molecule

A single electron is transferred from bromine to hydrogen

A pair of electrons is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

A shared pair of electrons is attracted to one nucleus

Question 16 of 20

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

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

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

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 17 of 20

18. 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 has strong forces of attraction between layers. These layers can slide over each other

Graphite is a smooth metal so creates a surface with little friction

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

Question 18 of 20

19. State 3 properties that makes iron suitable for saucepans

Good insulator, high melting point and malleable

Good conductor of heat, high melting point and malleable

Good insulator, high melting point and brittle

Good conductor of heat, high melting point and brittle

Question 19 of 20

20. 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 20 of 20

Structure & Bonding (Triple) quiz

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