Structure & Bonding (Triple) quiz

1. 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 fewer 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 more attractions between them. These take more energy to overcome.

Question 1 of 20

2. 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 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 2 of 20

3. 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 more magnetic than pure metals

Alloys are more ductile than pure metals

Alloys are harder and more magnetic than pure metals

Question 3 of 20

4. 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 weak 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 strong electrostatic attraction between a regular structure of negative metal ions and a sea of delocalised protons

Question 4 of 20

5. When can ionic substances conduct electricity?

Only when molten

Never

In any state

When molten or dissolved

Question 5 of 20

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

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

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

Question 6 of 20

7. Explain what is meant by electric current

The rate of flow of ions only

The rate of flow of elephants

The rate of flow of electrons only

The rate of flow of charged particles (e.g. of electrons or ions)

Question 7 of 20

8. Describe the formation of a covalent bond

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

The sharing of a single electron between two nuclei

Question 8 of 20

9. 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 zero electrons in 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 two electrons in each of 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 9 of 20

10. 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 has weak 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

Question 10 of 20

11.

State whether covalent substances conduct electricity, and explain why

Yes, 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

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

Question 11 of 20

12. 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?

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

Positive metal ions. Delocalised electrons. Giant Structure.

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

Positive metal ions. Delocalised negative ions. Giant Structure.

Question 12 of 20

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

NaCl has a giant ionic structure with weak electrostatic forces between oppositely charged ions that require little energy to break

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 simple molecular structure with weak intermolecular forces 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

Question 13 of 20

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

Low density and reactive

Light and reactive

Light and resists corrosion

Low density and resists corrosion

Question 14 of 20

15. Describe the bonding in a metal

The strong electrostatic attraction between oppositely charged ions

The strong electrostatic attraction between protons and neutrons

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

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

Question 15 of 20

16. Explain why Silica, SiO₂ is a solid with a high melting point

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

Silica has a giant covalent structure with many strong covalent bonds that need a lot of energy to break

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

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

Question 16 of 20

17. Explain the term ionic bond

An ionic bond is the strong magnetic attraction between oppositely charged ions

An ionic bond is the strong electrostatic attraction between a shared pair of electrons and two nuclei

An ionic bond is the strong electrostatic attraction between oppositely charged ions

An ionic bond is the strong electrostatic attraction between similarly charged ions

Question 17 of 20

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

A pair of electrons is transferred from bromine to hydrogen

A single electron is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

A shared pair of electrons is attracted to one nucleus

Question 18 of 20

19. 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 chloride 2) one electon around the sodium 3) 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

Question 19 of 20

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

Question 20 of 20

Structure & Bonding (Triple) quiz

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