Structure & Bonding (Triple) quiz

1. 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 layers which can easily slide over each other

Graphite has delocalised protons which can move

Question 1 of 20

2. Why is the boiling point of a larger molecule higher than that of a smaller molecule?

Larger molecules have fewer attractions between them. These take more 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 less energy to overcome.

Larger molecules have more attractions between them. These take less energy to overcome.

Question 2 of 20

3. 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 strong electrostatic forces between oppositely charged ions that require a lot of 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

Question 3 of 20

4.

State whether covalent substances conduct electricity, and explain why

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

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

Question 4 of 20

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

A shared pair of electrons is attracted to one nucleus

A single electron is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

A pair of electrons is transferred from bromine to hydrogen

Question 5 of 20

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

Alloys are harder and less malleable than pure metals

Alloys are more magnetic than pure metals

Alloys are more ductile than pure metals

Alloys are harder and more magnetic than pure metals

Question 6 of 20

7. 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 7 of 20

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

Buckminsterfullerene has a simple molecular structure with strong intermolecular forces that require a lot of 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 giant metallic structure with weak forces of attraction between layers

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

Question 8 of 20

9. 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), good conductor and low density

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

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

Question 9 of 20

10. Why do metals have high melting and boiling points?

There is a strong electrostatic attraction between a regular structure of positive metal ions and a sea of delocalised electrons

There is a strong electrostatic attraction between an irregular structure of positive metal ions and a sea of delocalised electrons

There is a strong electrostatic attraction between a regular structure of negative metal ions and a sea of delocalised protons

There is a weak electrostatic attraction between a regular structure of positive metal ions and a sea of delocalised electrons

Question 10 of 20

11. Explain why carbon dioxide gas, CO₂, is a gas at room temperature

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 weak covalent bonds which 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

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

Question 11 of 20

12. Describe the structure of metals

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

A simple 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

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

Question 12 of 20

13. Do ionic substances conduct electricity?

Yes, ionic substances always conduct electricity

No, ionic substances never conduct electricity

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

Only when molten

Question 13 of 20

14. Apart from being a mixture of metals, what non-metal is often added to alloys to make them stronger?

Carbon

Silicon

Hydrogen

Sulfur

Question 14 of 20

15. 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.

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

Positive metal ions. Delocalised electrons. Giant Structure.

Positive metal ions. Delocalised negative ions. Giant Structure.

Question 15 of 20

16. Describe the formation of a covalent bond

The sharing of a pair of electrons between two nuclei

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

The transfer of electrons from one atom to another

The sharing of a single electron between two nuclei

Question 16 of 20

17. Explain what is meant by electric current

The rate of flow of elephants

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

The rate of flow of ions only

The rate of flow of electrons only

Question 17 of 20

18. Explain whether solid ionic compounds conduct electricity

Solid ionic compounds sometimes conduct electricity, only when the ions are free to move

Solid ionic compounds cannot conduct electricity because the ions are not free to move

Solid ionic compounds can conduct electricity because the ions are free to move

Solid ionic compounds can conduct electricity because there is a sea of delocalised electrons that can move

Question 18 of 20

19. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of methane (CH₄), how many electrons should be shown in areas 1, 2, 3, and 4?

There should be four 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 4

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

There should be two electrons in each of the areas 1, 2, 3 and 4, and an additional 6 electrons around the outside of each hydrogen atom

Question 19 of 20

20. Explain the term ionic bond

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

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

Question 20 of 20

Structure & Bonding (Triple) quiz

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