Structure & Bonding (Triple) quiz

1. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of methane (CH₄), how many electrons should be shown in areas 1, 2, 3, and 4?

There should be two electrons in each of the areas 1, 2, 3 and 4, and an additional 6 electrons around the outside of each hydrogen atom

There should be four electrons in each of the areas 1, 2, 3 and 4

There should be one electron in each of the areas 1, 2, 3 and 4

There should be two electrons in each of the areas 1, 2, 3 and 4

Question 1 of 20

2. Typically, do covalent substances conduct electricity?

No

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

Depends on the substance

Yes

Question 2 of 20

3. Why do ionic compounds conduct electricity only when molten or in solution?

When solid the ions are free to move. When molten or in solution the ions are held in place

When solid the ions are held in place. When molten or in solution the ions are free to move

When solid the ions are arranged regularly. When molten or in solution the ions are arranged irregularly

When solid the electrons are held in place. When molten or in solution the electrons are free to move

Question 3 of 20

4. When are ions attracted to each other?

When the ions are the same size

When the ions have the same charge

When the ions are very small

When the ions are oppositely charged

Question 4 of 20

5. State a property that makes iron suitable for building

Strong

High melting point

Resists corrosion

Magnetic

Question 5 of 20

6. 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 giant metallic structure with weak forces of attraction between layers

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

Question 6 of 20

7. What does the word malleable mean?

Able to be drawn into a wire

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

Will break or crack under pressure

Able to carry current

Question 7 of 20

8. 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.

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

Positive metal ions. Delocalised electrons. Giant Structure.

Question 8 of 20

9. Why is the melting point of a smaller molecule lower than that of a larger molecule?

Larger molecules have more attractions between them. These take less energy to overcome.

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 more energy to overcome.

Question 9 of 20

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

A shared pair of electrons is attracted to 2 nuclei

A pair of electrons is transferred from bromine to hydrogen

A shared pair of electrons is attracted to one nucleus

A single electron is transferred from bromine to hydrogen

Question 10 of 20

11. Alloys contain different sized positive ions. What properties does this give alloys compared to pure metals?

Alloys are harder and more magnetic than pure metals

Alloys are more ductile than pure metals

Alloys are harder and less malleable than pure metals

Alloys are more magnetic than pure metals

Question 11 of 20

12. Explain, in terms of structure and bonding, why sodium chloride has a very high melting point

NaCl has a giant ionic structure with weak electrostatic forces between oppositely charged ions that require little energy to break

NaCl has a simple molecular structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to break

NaCl has a giant ionic structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to break

NaCl has a simple molecular structure with weak intermolecular forces that require little energy to break

Question 12 of 20

13. Describe the structure of metals

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

A giant 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 13 of 20

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

Graphite has delocalised electrons which can move

Graphite has delocalised protons which can move

Graphite has layers which can easily slide over each other

Graphite has positive ions which can move

Question 14 of 20

15. Do ionic substances conduct electricity?

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

Yes, ionic substances always conduct electricity

No, ionic substances never conduct electricity

Only when molten

Question 15 of 20

16. Describe the formation of a covalent bond

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

The sharing of a pair of electrons between two nuclei

The transfer of electrons from one atom to another

The sharing of a single electron between two nuclei

Question 16 of 20

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

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 +2 on the potassium and -1 on the oxide 3) A second potassium ion the same as the first

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 oxide ion the same as the first

Question 17 of 20

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

There are weak intermolecular forces that require little energy to break

There are charged particles that are free to move

There are no charged particles that are free to move

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

Question 18 of 20

19. Apart from being a mixture of metals, what non-metal is often added to alloys to make them stronger?

Hydrogen

Silicon

Carbon

Sulfur

Question 19 of 20

20. If a substance has a simple molecular structure, what physical state might it be at room temperature?

Solid or liquid

Solid

Any state

Gas or liquid

Question 20 of 20

Structure & Bonding (Triple) quiz

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