Structure & Bonding (Triple) quiz

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

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

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

Question 1 of 20

2. 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 sharing of a pair of electrons between two nuclei

The transfer of electrons from one atom to another

Question 2 of 20

3.

State whether covalent substances conduct electricity, and explain why

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

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

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

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

Question 3 of 20

4. 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 simple molecular structure with strong intermolecular forces that require a lot of 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 giant covalent structure with many weak covalent bonds which require little energy to overcome

Question 4 of 20

5. Describe the bonding in a metal

The strong electrostatic attraction between protons and neutrons

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

The strong electrostatic attraction between oppositely charged ions

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

Question 5 of 20

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

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

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.

Magnesium and oxygen are more reactive elements

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

Question 6 of 20

7. Do ionic substances conduct electricity?

No, ionic substances never conduct electricity

Yes, ionic substances always conduct electricity

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

Only when molten

Question 7 of 20

8. 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 8 of 20

9. Give the definition of a covalent bond

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

Strong electrostatic attraction between oppositely charged ions

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 9 of 20

10. What is a mixture of metals called?

An alloy

An ore

A compound

A solution

Question 10 of 20

11. Explain what is meant by electric current

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

The rate of flow of electrons only

Question 11 of 20

12. 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 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 12 of 20

13. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of ethene (C₂H₄), how many electrons should be shown in areas 1, 2, 3, 4, and 5?

There should be four electrons in each of areas 1, 2, 3 and 4, and two electrons in area 5

There should be two electrons in each of areas 1, 2, 3, 4 and 5

There should be four electrons in each of areas 1, 2, 3, 4 and 5

There should be two electrons in each of areas 1, 2, 3 and 4, and four electrons in area 5

Question 13 of 20

14. 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 14 of 20

15. What holds ions together?

Ions are held together by a strong magnetic 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 electrostatic attraction between the oppositely charged ions

Ions are held together by a strong electrostatic attraction between the shared pair of electrons and their nuclei

Question 15 of 20

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

Alloys are more magnetic than pure metals

Alloys are harder and more magnetic than pure metals

Alloys are more ductile than pure metals

Alloys are harder and less malleable than pure metals

Question 16 of 20

17. Explain whether solid ionic compounds conduct electricity

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

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

Question 17 of 20

18. State two properties of aluminium that make it suitable for use in food cans

Light and reactive

Malleable and low density

Light and resists corrosion

Ductile and malleable

Question 18 of 20

19. 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?

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.

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

Question 19 of 20

20. What does the word malleable mean?

Able to be hammered or pressed into shape without breaking or cracking

Able to be drawn into a wire

Able to carry current

Will break or crack under pressure

Question 20 of 20

Structure & Bonding (Triple) quiz

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