Structure & Bonding (Triple) quiz

1. 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 oppositely 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 similarly charged ions, in a giant structure, which requires a lot of energy to overcome

Question 1 of 20

2. 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 negative ions. Giant Structure.

Positive metal ions. Delocalised electrons. Giant Structure.

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

Question 2 of 20

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

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

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

Question 3 of 20

4. Describe the formation of a covalent bond

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

The sharing of a pair of electrons between two nuclei

Question 4 of 20

5. Typically, do covalent substances conduct electricity?

Depends on conditions (e.g. pressure, temperature etc.)

Depends on the substance

No

Yes

Question 5 of 20

6. Why are alloys harder than pure metals?

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 have higher melting points because they are mixtures so are harder

Alloys often contain carbon which is a very hard element

Question 6 of 20

7. Describe the structure of metals

A giant random 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

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

Question 7 of 20

8. What holds ions together?

Ions are held together by a strong electrostatic attraction between the similarly charged ions

Ions are held together by a strong electrostatic attraction between the oppositely charged ions

Ions are held together by a strong magnetic attraction between the oppositely charged ions

Ions are held together by a strong electrostatic attraction between the shared pair of electrons and their nuclei

Question 8 of 20

9. What is needed to complete this diagram to show the ionic bonding in potassium oxide, K₂O ?

1) eight electrons around the potassium (any combination of dots and one crosses) 2) A charge of +2 on the oxide and -1 on the potassium 3) A second potassium ion the same as the first

1) eight electrons around the oxide (six dots and two cross) 2) A charge of +1 on the potassium and -2 on the oxide 3) A second potassium ion the same as the first

1) eight electrons around the oxide (six dots and two cross) 2) A charge of +1 on the potassium and -2 on the oxide 3) A second oxide ion the same as the first

1) eight electrons around the oxide (six dots and two cross) 2) A charge of +2 on the potassium and -1 on the oxide 3) A second potassium ion the same as the first

Question 9 of 20

10. Do ionic substances conduct electricity?

Only when molten

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

No, ionic substances never conduct electricity

Yes, ionic substances always conduct electricity

Question 10 of 20

11. 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 11 of 20

12. Give the definition of a covalent bond

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

Strong electrostatic attraction between oppositely charged ions

Question 12 of 20

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

Graphite has layers which can easily slide over each other

Graphite has delocalised protons which can move

Graphite has positive ions which can move

Graphite has delocalised electrons which can move

Question 13 of 20

14. 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, 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

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 seven more on the outside of each hydrogen atom

Question 14 of 20

15. 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 are charged particles that are free to move

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

Question 15 of 20

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

Light and reactive

Ductile and malleable

Malleable and low density

Light and resists corrosion

Question 16 of 20

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

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

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

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

Question 17 of 20

18. 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 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 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 19 of 20

20. Explain whether solid ionic compounds conduct electricity

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

Solid ionic compounds can conduct electricity because there is a sea of delocalised electrons that can move

Question 20 of 20

Structure & Bonding (Triple) quiz

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