Structure & Bonding (Triple) quiz

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

Light and reactive

Malleable and low density

Light and resists corrosion

Ductile and malleable

Question 1 of 20

2. Do ionic substances conduct electricity?

No, ionic substances never conduct electricity

Only when molten

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

Yes, ionic substances always conduct electricity

Question 2 of 20

3. Explain the term ionic bond

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

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

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 3 of 20

4. 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 magnetic than pure metals

Alloys are more ductile than pure metals

Question 4 of 20

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

Ionic

Covalent

Metallic

Covalent or ionic

Question 5 of 20

6. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of ethane (C₂H₆), how many electrons should be shown in areas 1, 2, 3, 4, 5, 6 and 7?

There should be two electrons in each of areas 1, 2, 3, 4, 5, 6 and 7

There should be two electrons in each of areas 1, 3, 4, 5, 6 and 7, but none in area 2

There should be two electrons in each of areas 1, 2, 3, 4, 5, 6 and 7, and also two more on the outside of each hydrogen atom

There should be two electrons in each of areas 1, 2, 3, 4, 5, 6 and 7, and also seven more on the outside of each hydrogen atom

Question 6 of 20

7. 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 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

Question 7 of 20

8. Describe the bonding in a metal

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

The strong electrostatic attraction between oppositely charged ions

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 8 of 20

9. Describe the formation of a covalent bond

The transfer of electrons from one atom to another

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

Question 9 of 20

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

There are no charged particles that are free to move

There are weak intermolecular forces that require little energy to break

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

There are charged particles that are free to move

Question 10 of 20

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

A single electron is transferred from bromine to hydrogen

A shared pair of electrons is attracted to one nucleus

A pair of electrons is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

Question 11 of 20

12. Explain why magnesium oxide has a higher melting point than sodium chloride.

Magnesium and oxygen are more reactive elements

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.

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

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

Question 12 of 20

13. What is a mixture of metals called?

A solution

An alloy

An ore

A compound

Question 13 of 20

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

Graphite has layers which can easily slide over each other

Graphite has delocalised electrons which can move

Graphite has delocalised protons which can move

Graphite has positive ions which can move

Question 14 of 20

15. What does the word malleable mean?

Able to be drawn into a wire

Able to carry current

Will break or crack under pressure

Able to be hammered or pressed into shape without breaking or cracking

Question 15 of 20

16. 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 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 chloride ion the same as the first

Question 16 of 20

17. Why is the boiling point of a larger molecule higher than that of a smaller 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 17 of 20

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

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

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

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

Question 18 of 20

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

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

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

Question 19 of 20

20. 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. Giant Structure.

Positive metal ions. Delocalised negative ions. Giant Structure.

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

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

Question 20 of 20

Structure & Bonding (Triple) quiz

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