Structure & Bonding (Triple) quiz

1. Explain whether solid ionic compounds conduct electricity

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

Solid ionic compounds can conduct electricity because 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 sometimes conduct electricity, only when the ions are free to move

Question 1 of 20

2. 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 electrons only

The rate of flow of ions only

Question 2 of 20

3. 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.

Positive metal ions. Delocalised electrons. Giant Structure.

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

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

Question 3 of 20

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

Carbon dioxide has a simple molecular structure with weak intermolecular forces that 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 giant covalent structure with many weak covalent bonds which 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 4 of 20

5. Give the definition of a covalent bond

Strong electrostatic attraction between oppositely charged 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

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

Question 5 of 20

State whether covalent substances conduct electricity, and explain why

No. Because there are no 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

Only when molten, because there are charged particles that are free to move

Question 6 of 20

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

Low density and resists corrosion

Light and resists corrosion

Light and reactive

Low density and reactive

Question 7 of 20

8. 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 similarly charged ions

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

Question 8 of 20

9. Why do metals have high melting and boiling points?

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 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 9 of 20

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

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 +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 chloride ion the same as the first

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

Question 10 of 20

11. When can ionic substances conduct electricity?

Never

When molten or dissolved

In any state

Only when molten

Question 11 of 20

12. 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 12 of 20

13. Explain, in terms of structure and bonding, why magnesium oxide has a higher melting point than sodium chloride

Mg²⁺ and O²⁻ ions are larger than sodium and chloride therefore the electrostatic forces between the ions are much stronger. This requires more energy to break.

Magnesium and oxygen are more reactive elements

Sodium chloride is a simple molecular substance so there are only weak intermolecular forces which require little energy to break

NaCl and MgO both have a giant ionic structure with strong electrostatic forces between oppositely charged ions. The Ions in MgO have a charge of 2 and -2, but in NaCl the charges are 1 and -1. So the bonds in MgO require more energy to break

Question 13 of 20

14. Describe the formation of a covalent bond

The sharing of a pair of electrons between two nuclei

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

The sharing of a single electron between two nuclei

The transfer of electrons from one atom to another

Question 14 of 20

15. 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 15 of 20

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

It depends on which atoms are present

Higher

Size doesn\'t affect boiling point

Lower

Question 16 of 20

17. Why are alloys harder than pure metals?

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

Alloys often contain carbon which is a very hard element

Question 17 of 20

18. 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, 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

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

Question 18 of 20

19. 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 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 carbon

Question 19 of 20

20. 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 20 of 20

Structure & Bonding (Triple) quiz

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