Structure & Bonding (Triple) quiz

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

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

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

Question 1 of 20

2. 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 more energy to overcome.

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

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

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

Question 2 of 20

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

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

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

Question 3 of 20

4. Do ionic substances conduct electricity?

Only when molten

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

Yes, ionic substances always conduct electricity

No, ionic substances never conduct electricity

Question 4 of 20

5. Explain why metals are malleable

Metals have delocalised protons which can move

Metals have strong covalent bonds which require a lot of energy to break

Metals have delocalised electrons which are free to move

Metals have layers of ions that can slide over each other

Question 5 of 20

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

Ionic

Covalent or ionic

Metallic

Covalent

Question 6 of 20

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

Carbon

Hydrogen

Sulfur

Silicon

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?

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

Positive metal ions. Delocalised electrons. Giant Structure.

Positive metal ions. Delocalised negative ions. Giant Structure.

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

Question 8 of 20

9. Describe the structure of metals

A simple regular 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 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

Question 9 of 20

10. 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 magnetic than pure metals

Alloys are more ductile than pure metals

Alloys are harder and less malleable than pure metals

Question 10 of 20

11. 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 +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 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 11 of 20

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

A shared pair of electrons is attracted to one nucleus

A shared pair of electrons is attracted to 2 nuclei

A pair of electrons is transferred from bromine to hydrogen

A single electron is transferred from bromine to hydrogen

Question 12 of 20

13. 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 13 of 20

14.

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 14 of 20

15. 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 transfer of electrons from one atom to another

The sharing of a single electron between two nuclei

Question 15 of 20

16. 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 simple molecular structure with weak intermolecular forces that require little 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

Question 16 of 20

17. State a property that makes iron suitable for building

High melting point

Strong

Magnetic

Resists corrosion

Question 17 of 20

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

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

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

Question 18 of 20

19. Explain the term ionic bond

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

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

Question 19 of 20

20. 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

There should be four electrons 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, and an additional 6 electrons around the outside of each hydrogen atom

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

Question 20 of 20

Structure & Bonding (Triple) quiz

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