Structure & Bonding (Triple) quiz

1. 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 1 of 20

2.

State whether covalent substances conduct electricity, and explain why

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

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

Question 2 of 20

3. Explain what is meant by electric current

The rate of flow of elephants

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 electrons only

Question 3 of 20

4. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of nitrogen (N₂), how many electrons should be shown in areas 1, 2 and 3?

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

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

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

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

Question 4 of 20

5. Describe the structure of an ionic compound, e.g NaCl

A giant structure held together by the attraction between similarly charged ions

A giant structure held together by the attraction between oppositely charged ions

A giant structure held together by intermolecular forces

A giant structure held together by the attraction between positive metal ions and a sea of delocalised electrons

Question 5 of 20

6. Do ionic substances conduct electricity?

Yes, ionic substances always conduct electricity

Only when molten

No, ionic substances never conduct electricity

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

Question 6 of 20

7. Describe the structure of metals

A simple random 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 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

Question 7 of 20

8. Describe the formation of a covalent bond

The transfer of electrons from one atom to another

The sharing of a single electron between two nuclei

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

The sharing of a pair of electrons between two nuclei

Question 8 of 20

9. What does the word malleable mean?

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

Will break or crack under pressure

Able to carry current

Able to be drawn into a wire

Question 9 of 20

10. Give the definition of a covalent bond

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

Strong electrostatic attraction between a shared pair of electrons and a nucleus

Question 10 of 20

11. 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 11 of 20

12. State 2 properties that makes aluminium suitable for manufacturing aircraft

Low density and resists corrosion

Light and reactive

Low density and reactive

Light and resists corrosion

Question 12 of 20

13. Do larger molecules have higher or lower boiling points than smaller molecules?

Lower

Higher

It depends on which atoms are present

Size doesn\'t affect boiling point

Question 13 of 20

14. What holds ions together?

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

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

Question 14 of 20

15. How can atoms get a full outer shell?

Only transfer (ionic) of electrons

Conversion of electrons to protons

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

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

Question 15 of 20

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

Sulfur

Hydrogen

Carbon

Silicon

Question 16 of 20

17. Why are alloys harder than pure metals?

Alloys often contain carbon which is a very hard element

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

Question 17 of 20

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

Carbon dioxide has a giant covalent structure with many strong covalent bonds which require a lot of 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 simple molecular structure with strong intermolecular forces that require a lot of energy to overcome

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

Question 18 of 20

19. 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 19 of 20

20. 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 sometimes conduct electricity, only when the ions are free to 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

Question 20 of 20

Structure & Bonding (Triple) quiz

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