Structure & Bonding (Triple) quiz

1. Explain, in terms of its structure, why graphite can act as a lubricant.

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

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 a low melting point so becomes liquid when heated by friction

Question 1 of 20

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

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

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

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

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

Question 2 of 20

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

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

Question 3 of 20

4. Do ionic substances conduct electricity?

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

No, ionic substances never conduct electricity

Only when molten

Yes, ionic substances always conduct electricity

Question 4 of 20

5. Why are alloys harder than pure metals?

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

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

Alloys often contain carbon which is a very hard element

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

Question 5 of 20

6. 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 negative ions. Giant Structure.

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

Positive metal ions. Delocalised electrons. Giant Structure.

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

Question 6 of 20

7. Explain why metals are malleable

Metals have delocalised protons which can move

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

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 less energy to overcome.

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 fewer attractions between them. These take more energy to overcome.

Question 8 of 20

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

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

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

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

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

Question 9 of 20

10. What is a mixture of metals called?

An alloy

A solution

A compound

An ore

Question 10 of 20

11. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of hydrogen (H₂), how many electrons should be shown in areas 1, 2 and 3?

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

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

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

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

Question 11 of 20

12. Explain what is meant by electric current

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

The rate of flow of elephants

The rate of flow of electrons only

The rate of flow of ions only

Question 12 of 20

13. 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 giant metallic structure with weak forces of attraction between layers

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

Question 13 of 20

14. Describe the formation of a covalent bond

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

The sharing of a single electron between two nuclei

Question 14 of 20

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

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

Question 15 of 20

16. How can atoms get a full outer shell?

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

Conversion of electrons to protons

Only transfer (ionic) of electrons

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

Question 16 of 20

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

A shared pair of electrons is attracted to one nucleus

A shared pair of electrons is attracted to 2 nuclei

A single electron is transferred from bromine to hydrogen

A pair of electrons is transferred from bromine to hydrogen

Question 17 of 20

18.

State whether covalent substances conduct electricity, and explain why

Only under pressure, because there are charged particles that are free to move

Only when molten, because there are charged particles that are free to move

Yes, because there are charged particles that are free to move

No. Because there are no charged particles that are free to move

Question 18 of 20

19. What holds ions together?

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

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

Question 19 of 20

20. Describe the structure of metals

A simple regular 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 giant random 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 20 of 20

Structure & Bonding (Triple) quiz

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