Structure & Bonding (Triple) quiz

1. If a substance has a simple molecular structure, what physical state might it be at room temperature?

Any state

Solid or liquid

Gas or liquid

Solid

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

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

Question 2 of 20

3. Describe the formation of a covalent bond

The sharing of a single electron between two nuclei

The transfer of electrons from one atom to another

The sharing of a pair of electrons between two nuclei

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

Question 3 of 20

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

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

Ductile (can be drawn into a wire), bad 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 4 of 20

5.

State whether covalent substances conduct electricity, and explain why

Only when molten, 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

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

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?

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

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

Positive metal ions. Delocalised electrons. Giant Structure.

Positive metal ions. Delocalised negative ions. Giant Structure.

Question 6 of 20

7. 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 non-metal and one or more elements, usually other metals or hydrogen

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

Question 7 of 20

8. A substance is found not to conduct electricity even when molten. What type of bonding does the substance have?

Ionic

Metallic

Covalent or ionic

Covalent

Question 8 of 20

9. 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 postive ion and a sea of delocalised positive ions

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

Question 9 of 20

10. Explain why magnesium oxide has a higher melting point than sodium chloride.

Magnesium and oxygen are more reactive elements

Mg²⁺ and O²⁻ ions have a higher charge than sodium and chloride therefore the electrostatic forces between the ions are much stronger. This requires more energy to break.

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

Question 10 of 20

11. What is needed to complete this diagram to show the ionic bonding in magnesium chloride, MgCl₂ ?

1) eight electrons around the chloride (seven dots and one cross) 2) A charge of +1 on the magnesium and -2 on the chloride 3) A second chloride ion the same as the first

1) eight electrons around the chloride (seven dots and one cross) 2) A charge of +2 on the magnesium and -1 on the chloride 3) A second chloride ion the same as the first

1) eight electrons around the magnesium (any combination of dots and one crosses) 2) A charge of +2 on the magnesium and -1 on the chloride 3) A second chloride ion the same as the first

1) eight electrons around the chloride (seven dots and one cross) 2) A charge of +2 on the magnesium and -1 on the chloride 3) A second magensium ion the same as the first

Question 11 of 20

12. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of water (H₂O), how many electrons should be shown in areas 1, 2, 3 and 4?

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

There should be two electrons in each of areas 1 and 2, and zero electrons in areas 3 and 4. There should also be an additional 4 electrons around the outside of the oxygen atom.

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

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

Question 12 of 20

13. 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 13 of 20

14. When are ions attracted to each other?

When the ions are the same size

When the ions are oppositely charged

When the ions have the same charge

When the ions are very small

Question 14 of 20

15. 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 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 less malleable than pure metals

Alloys are harder and more magnetic than pure metals

Alloys are more ductile than pure metals

Question 16 of 20

17. 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 simple molecular structure with weak intermolecular forces that require little energy to overcome

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

Question 17 of 20

18. Explain whether solid ionic compounds conduct electricity

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

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

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

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

Question 18 of 20

19. When can ionic substances conduct electricity?

Never

When molten or dissolved

In any state

Only when molten

Question 19 of 20

20. Explain, in terms of its structure, why graphite can conduct electricity.

Graphite has layers which can easily slide over each other

Graphite has delocalised electrons which can move

Graphite has delocalised protons which can move

Graphite has positive ions which can move

Question 20 of 20

Structure & Bonding (Triple) quiz

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