Structure & Bonding (Triple) quiz

1. 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 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

An alloy is a mixture of a metal and one or more elements, usually other metals or hydrogen

Question 1 of 20

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

Graphite has delocalised protons which can move

Graphite has positive ions which can move

Graphite has delocalised electrons which can move

Graphite has layers which can easily slide over each other

Question 2 of 20

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

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

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

Question 3 of 20

4.

State whether covalent substances conduct electricity, and explain why

Only when molten, because there are charged particles that are free to move

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

Yes, because there are charged particles that are free to move

Only under pressure, because there are charged particles that are free to move

Question 4 of 20

5. Describe the structure of metals

A giant 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 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

Question 5 of 20

6. 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 one electron 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

Question 6 of 20

7. How can atoms get a full outer shell?

Either the transfer (ionic) or sharing (covalent) of electrons

Conversion of electrons to protons

Either the transfer (covalent) or sharing (ionic) of electrons

Only transfer (ionic) of electrons

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. Giant Structure.

Positive metal ions. Delocalised negative ions. Giant Structure.

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

Positive metal ions. Delocalised electrons. Weak intermolecular forces.

Question 8 of 20

9. Give the definition of a covalent bond

Strong electrostatic attraction between a postive ion and a sea of delocalised positive ions

Strong electrostatic attraction between oppositely charged ions

Strong electrostatic attraction between a shared pair of electrons and a nucleus

Strong electrostatic attraction between a shared pair of electrons and two nuclei

Question 9 of 20

10. Describe the structure of an ionic compound, e.g NaCl

A giant structure held together by the attraction between oppositely charged ions

A giant structure held together by intermolecular forces

A giant structure held together by the attraction between similarly charged ions

A giant structure held together by the attraction between positive metal ions and a sea of delocalised electrons

Question 10 of 20

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

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 weak intermolecular forces that require little energy to overcome

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 11 of 20

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

Ionic

Metallic

Covalent

Covalent or ionic

Question 12 of 20

13. Describe the formation of a covalent bond

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 pair of electrons between two nuclei

The sharing of a single electron between two nuclei

Question 13 of 20

14. When can ionic substances conduct electricity?

Only when molten

Never

When molten or dissolved

In any state

Question 14 of 20

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

Low density and reactive

Light and reactive

Low density and resists corrosion

Light and resists corrosion

Question 15 of 20

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

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 strong covalent bonds which 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 16 of 20

17. Why is the boiling point of a larger molecule higher than that of a smaller molecule?

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.

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.

Question 17 of 20

18. Why are alloys harder than pure metals?

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 contain different sized positive ions, so there are no layers of ions to slide over each other

Alloys often contain carbon which is a very hard element

Question 18 of 20

19. Why do metals have high melting and boiling points?

There is a strong electrostatic attraction between an irregular structure of positive metal ions and a sea of delocalised electrons

There is a weak electrostatic attraction between a regular structure of positive metal ions and a sea of delocalised electrons

There is a strong electrostatic attraction between a regular structure of positive metal ions and a sea of delocalised electrons

There is a strong electrostatic attraction between a regular structure of negative metal ions and a sea of delocalised protons

Question 19 of 20

20. 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 shared pair of electrons and their nuclei

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

Question 20 of 20

Structure & Bonding (Triple) quiz

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