Structure & Bonding (Triple) quiz

1. Describe the bonding in a metal

The strong electrostatic attraction between oppositely charged ions

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

Question 1 of 20

2. 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 2 of 20

3.

State whether covalent substances conduct electricity, and explain why

Only when molten, because there are 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

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

Question 3 of 20

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

Covalent

Ionic

Metallic

Covalent or ionic

Question 4 of 20

5. 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 four electrons in each of areas 1, 2, 3, 4 and 5

There should be two 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 5 of 20

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

Low density and reactive

Low density and resists corrosion

Light and reactive

Light and resists corrosion

Question 6 of 20

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

Lower

Higher

Size doesn\'t affect boiling point

It depends on which atoms are present

Question 7 of 20

8. 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 weak electrostatic attraction between a regular 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

Question 8 of 20

9. Explain why methane gas, CH₄, is a gas at room temperature

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

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

Question 9 of 20

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

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

Question 10 of 20

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

A pair of electrons is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

A single electron is transferred from bromine to hydrogen

A shared pair of electrons is attracted to one nucleus

Question 11 of 20

12. What is needed to complete this diagram to show the ionic bonding in sodium chloride, NaCl ?

1) eight electrons around the chloride (seven dots and one cross) 2) A charge of -1 on the sodium and +1 on the chloride

1) eight electrons around the chloride (seven dots and one cross) 2) A charge of +1 on the sodium and -1 on the chloride

1) seven electrons around the sodium 2) one electon around the chloride 3) A charge of +1 on the sodium and -1 on the chloride

1) seven electrons around the chloride 2) one electon around the sodium 3) A charge of +1 on the sodium and -1 on the chloride

Question 12 of 20

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

Alloys are more ductile than pure metals

Alloys are harder and less malleable than pure metals

Alloys are harder and more magnetic than pure metals

Alloys are more magnetic than pure metals

Question 13 of 20

14. Describe the formation of a covalent bond

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

The transfer of electrons from one atom to another

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

Graphite has delocalised electrons which can move

Graphite has layers which can easily slide over each other

Graphite has positive ions which can move

Graphite has delocalised protons which can move

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 simple molecular structure with weak intermolecular forces that require little 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

Question 17 of 20

18. What is an alloy?

An alloy is a mixture of a metal and one or more elements, usually other metals or hydrogen

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 non-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 carbon

Question 18 of 20

19. Why do ionic substance have high melting and boiling points?

There is a strong electrostatic attraction between similarly charged ions, in a giant structure, which requires a lot of energy to overcome

There is a strong electrostatic attraction between oppositely charged ions, in a giant structure, which requires a lot of energy to overcome

There are weak intermolecular forces, in a simple molecular structure, which require little energy to overcome

There is a weak electrostatic attraction between oppositely charged ions, in a giant structure, which requires little energy to overcome

Question 19 of 20

20. 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 20 of 20

Structure & Bonding (Triple) quiz

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