Structure & Bonding (Triple) quiz

1. Give the definition of a covalent bond

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

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

Strong electrostatic attraction between a postive ion and a sea of delocalised positive ions

Strong electrostatic attraction between oppositely charged ions

Question 1 of 20

2. Describe the structure of metals

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 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

Question 2 of 20

3. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of oxygen (O₂), how many electrons should be shown in areas 1, 2 and 3?

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

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

Question 3 of 20

4. Describe the formation of a covalent bond

The sharing of a single electron between two nuclei

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

Question 4 of 20

5.

State whether covalent substances conduct electricity, and explain why

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

Only under pressure, 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 negative ions. Giant Structure.

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

Positive metal ions. Delocalised electrons. Giant Structure.

Question 6 of 20

7. Do ionic substances conduct electricity?

Yes, ionic substances always conduct electricity

Only when molten

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

No, ionic substances never conduct electricity

Question 7 of 20

8. 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 harder and more magnetic than pure metals

Alloys are more ductile than pure metals

Alloys are more magnetic than pure metals

Question 8 of 20

9. Explain why metals are good conductors of electricity

Metals have positive ions which can move

Metals have layers of ions that can slide over each other

Metals have delocalised electrons which are free to move

Metals have delocalised protons which can move

Question 9 of 20

10. Explain what is meant by electric current

The rate of flow of electrons only

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

Question 10 of 20

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

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 strong intermolecular forces that require a lot of energy to overcome

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 11 of 20

12. When are ions attracted to each other?

When the ions are oppositely charged

When the ions are very small

When the ions are the same size

When the ions have the same charge

Question 12 of 20

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

Lower

It depends on which atoms are present

Higher

Size doesn\'t affect boiling point

Question 13 of 20

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

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

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

Question 14 of 20

15. Explain, in terms of structure and bonding, why sodium chloride has a very high melting point

NaCl has a simple molecular 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 giant ionic structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to break

NaCl has a simple molecular structure with weak intermolecular forces that require little energy to break

Question 15 of 20

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

Hydrogen

Sulfur

Carbon

Silicon

Question 16 of 20

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

Ductile and malleable

Light and resists corrosion

Light and reactive

Malleable and low density

Question 17 of 20

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

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 +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 magensium 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

Question 18 of 20

19. Why do ionic compounds conduct electricity only when molten or in solution?

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

When solid the electrons are held in place. When molten or in solution the electrons are free to move

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

Question 19 of 20

20. Explain why nitrogen gas, N₂, is a gas at room temperature

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

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

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

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

Question 20 of 20

Structure & Bonding (Triple) quiz

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