Structure & Bonding (Triple) quiz

1. State the fomula for the two ions in iron (II) sulfide

Fe²⁺ and S²⁻

Fe⁺ and S⁻

Fe³⁺ and S²⁻

Fe³⁺ and S³⁻

Question 1 of 20

2. What does the word malleable mean?

Able to carry current

Will break or crack under pressure

Able to be drawn into a wire

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

Question 2 of 20

3. Suggest why buckminsterfullerene, C₆₀, has a low melting point.

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

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

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

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

Question 3 of 20

4. 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 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 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 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 4 of 20

5. Describe the structure of metals

A giant random structure of positive metal ions surrounded by a sea of delocalised electrons

A giant regular structure of positive metal ions surrounded by a sea of delocalised electrons

A simple random structure of positive metal ions surrounded by a sea of delocalised electrons

A simple regular structure of positive metal ions surrounded by a sea of delocalised electrons

Question 5 of 20

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

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

Question 6 of 20

7. Give the definition of a covalent bond

Strong electrostatic attraction between a shared pair of electrons and a nucleus

Strong electrostatic attraction between oppositely charged ions

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

Strong electrostatic attraction between a shared pair of electrons and two nuclei

Question 7 of 20

State whether covalent substances conduct electricity, and explain why

Yes, because there are charged particles that are free to move

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

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

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

Question 8 of 20

9. 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 9 of 20

10. Describe the formation of a covalent bond

The transfer of electrons from one atom to another

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

The sharing of a single electron between two nuclei

The sharing of a pair of electrons between two nuclei

Question 10 of 20

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

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

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

Question 11 of 20

12. State 3 properties that makes aluminium suitable for power cables

Ductile (can be drawn into a wire), bad conductor and low density

Ductile (can be drawn into a wire), good conductor and low density

Ductile (can be drawn into a wire), good conductor and light

Ductile (can be drawn into a wire), bad conductor and light

Question 12 of 20

13. Do ionic substances conduct electricity?

No, ionic substances never conduct electricity

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

Only when molten

Yes, ionic substances always conduct electricity

Question 13 of 20

14. 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 contain different sized positive ions, so there are no layers of ions to slide over each other

Alloys have higher melting points because they are mixtures so are harder

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 less energy to overcome.

Larger molecules have more attractions between them. These take more 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.

Question 15 of 20

16. 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 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

Question 16 of 20

17. 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 three electrons in area 1, four electrons in area 2, and three electrons in area 3

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

There should be two electrons in area 1, six 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

Question 17 of 20

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

Graphite has positive ions which can move

Graphite has delocalised electrons which can move

Graphite has layers which can easily slide over each other

Graphite has delocalised protons which can move

Question 18 of 20

19. 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 19 of 20

20. 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 cannot conduct electricity because the ions are not free to move

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

Question 20 of 20

Structure & Bonding (Triple) quiz

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