Structure & Bonding (Triple) quiz

1. Why do covalent compounds (e.g H₂O) not conduct electricity?

There are no charged particles that are free to move

There is a sea of delocalised electrons that are free to move

There are weak intermolecular forces that require little energy to break

There are charged particles that are free to move

Question 1 of 20

2. Describe the bonding in a metal

The strong electrostatic attraction between oppositely charged ions

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 a regular structure of positive ions and a sea of delocalised electrons

Question 2 of 20

3. What is an alloy?

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 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 3 of 20

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

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

Question 4 of 20

5. 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 transfer of electrons from one atom to another

The sharing of a pair of electrons between two nuclei

Question 5 of 20

6. Why are alloys harder than pure metals?

Alloys often contain carbon which is a very hard element

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

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

Question 6 of 20

7. Explain what is meant by electric current

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

The rate of flow of electrons only

Question 7 of 20

8. Explain the term ionic bond

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

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 similarly charged ions

Question 8 of 20

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

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

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

Question 9 of 20

10. Give the definition of a covalent bond

Strong electrostatic attraction between oppositely charged ions

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

Question 10 of 20

11. When can ionic substances conduct electricity?

Never

Only when molten

When molten or dissolved

In any state

Question 11 of 20

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

Light and reactive

Low density and reactive

Low density and resists corrosion

Light and resists corrosion

Question 12 of 20

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

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

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

Question 13 of 20

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

There should be one electron in area 1, two electrons in area 2, and seven electrons in area 3

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

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

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

Question 14 of 20

15. 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 more energy to overcome.

Larger molecules have fewer attractions between them. These take less 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.

Question 15 of 20

16. 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 16 of 20

17. Explain why metals are good conductors of electricity

Metals have delocalised electrons which are free to move

Metals have positive ions which can move

Metals have delocalised protons which can move

Metals have layers of ions that can slide over each other

Question 17 of 20

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

Graphite has delocalised protons which can move

Graphite has layers which can easily slide over each other

Graphite has positive ions which can move

Graphite has delocalised electrons which can move

Question 18 of 20

19. 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 negative ions. Giant Structure.

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.

Question 19 of 20

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

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

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

Question 20 of 20

Structure & Bonding (Triple) quiz

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