Structure & Bonding (Triple) quiz

1. What is a mixture of metals called?

A compound

An alloy

A solution

An ore

Question 1 of 20

2. Explain why carbon dioxide gas, CO₂, is a gas at room temperature

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

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

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

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

Question 2 of 20

3. Explain why metals are malleable

Metals have delocalised electrons which are free to move

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

Question 3 of 20

4. 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 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

Question 4 of 20

5. 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 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 fewer attractions between them. These take more energy to overcome.

Question 5 of 20

6. 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 sharing of a single electron between two nuclei

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

Question 6 of 20

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

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

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

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

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

Question 7 of 20

8. Why are alloys harder than pure metals?

Alloys often contain carbon which is a very hard element

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

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

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 negative ions. Giant Structure.

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

Positive metal ions. Delocalised electrons. Giant Structure.

Question 9 of 20

10. Typically, do covalent substances conduct electricity?

No

Yes

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

Depends on the substance

Question 10 of 20

11.

State whether covalent substances conduct electricity, and explain why

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

Only when molten, because there are 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

Question 11 of 20

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

Light and resists corrosion

Low density and resists corrosion

Low density and reactive

Light and reactive

Question 12 of 20

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

A shared pair of electrons is attracted to one nucleus

A single electron is transferred from bromine to hydrogen

A pair of electrons is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

Question 13 of 20

14. Describe the structure of metals

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 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 14 of 20

15. 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 15 of 20

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

Graphite has positive ions which can move

Graphite has delocalised protons which can move

Graphite has layers which can easily slide over each other

Graphite has delocalised electrons which can move

Question 16 of 20

17. State the fomula for the two ions in vanadium (V) oxide

V⁵⁺ and O²⁻

There are no ions because it is covalent

V⁺ and O⁻

V²⁺ and O²⁻

Question 17 of 20

18. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of hydrogen (H₂), how many electrons should be shown in areas 1, 2 and 3?

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

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

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

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

Question 18 of 20

19. 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 19 of 20

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

Fe³⁺ and S³⁻

Fe³⁺ and S²⁻

Fe⁺ and S⁻

Fe²⁺ and S²⁻

Question 20 of 20

Structure & Bonding (Triple) quiz

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