Structure & Bonding (Triple) quiz

1. 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 cannot conduct electricity because the ions are not free to 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 1 of 20

2. Do ionic substances conduct electricity?

Yes, ionic substances always conduct electricity

No, ionic substances never conduct electricity

Only when molten

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

Question 2 of 20

3. Explain why metals are malleable

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

Metals have layers of ions that can slide over each other

Metals have delocalised protons which can move

Metals have delocalised electrons which are free to move

Question 3 of 20

4. 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 4 of 20

5. Why are alloys harder than pure metals?

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

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

Question 5 of 20

6. Why is the boiling point of a larger molecule higher than that of a smaller 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 more attractions between them. These take more energy to overcome.

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

Question 6 of 20

7. State 2 properties that makes aluminium suitable for manufacturing aircraft

Light and reactive

Low density and resists corrosion

Light and resists corrosion

Low density and reactive

Question 7 of 20

8. Describe the structure of metals

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 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 8 of 20

9. Describe the formation of a covalent bond

The transfer of electrons from one atom to another

The sharing of a pair of electrons between two nuclei

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

The sharing of a single electron between two nuclei

Question 9 of 20

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

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

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

Question 10 of 20

11. 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 negative ions. Giant Structure.

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

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

Positive metal ions. Delocalised electrons. Giant Structure.

Question 11 of 20

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

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

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

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

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

Question 12 of 20

13. What holds ions together?

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

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

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

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

Question 13 of 20

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

Silicon

Hydrogen

Sulfur

Carbon

Question 14 of 20

15. 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 15 of 20

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

There are weak intermolecular forces that require little energy to break

There are no charged particles that are free to move

There are charged particles that are free to move

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

Question 16 of 20

17. 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 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

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

Question 17 of 20

18. In the dot and cross diagram of the outer electrons showing the covalent bonding of ammonia (NH₃), how many electrons should be shown in areas 1, 2, 3 and 4?

There should be 2 electrons in each of the areas 1, 2, 3 but none in 4

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

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

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

Question 18 of 20

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

A pair of electrons is transferred from bromine to hydrogen

A single electron is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

A shared pair of electrons is attracted to one nucleus

Question 19 of 20

20. What is needed to complete this diagram to show the ionic bonding in sodium chloride, NaCl ?

1) eight electrons around the chloride (seven dots and one cross) 2) A charge of +1 on the sodium and -1 on the chloride

1) seven electrons around the sodium 2) one electon around the chloride 3) A charge of +1 on the sodium and -1 on the chloride

1) seven electrons around the chloride 2) one electon around the sodium 3) A charge of +1 on the sodium and -1 on the chloride

1) eight electrons around the chloride (seven dots and one cross) 2) A charge of -1 on the sodium and +1 on the chloride

Question 20 of 20

Structure & Bonding (Triple) quiz

Structure & Bonding (Triple) quiz

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