Structure & Bonding (Triple) quiz

1. Why are alloys harder than pure metals?

Alloys often contain carbon which is a very hard element

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

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

Alloys are more magnetic than pure metals so when they are formed the ions are packed closer together

Question 1 of 20

2. Explain why nitrogen gas, N₂, is a gas at room temperature

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

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

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

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

Question 2 of 20

3. 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 +1 on the potassium and -2 on the oxide 3) A second oxide 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

Question 3 of 20

4. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of nitrogen (N₂), how many electrons should be shown in areas 1, 2 and 3?

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

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

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

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

Question 4 of 20

5. Describe the formation of a covalent bond

The sharing of a pair of electrons between two nuclei

The transfer of electrons from one atom to another

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

The sharing of a single electron between two nuclei

Question 5 of 20

6. What is an alloy?

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

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

Question 6 of 20

7. State 3 properties that makes aluminium suitable for power cables

Ductile (can be drawn into a wire), bad conductor and light

Ductile (can be drawn into a wire), bad conductor and low density

Ductile (can be drawn into a wire), good conductor and light

Ductile (can be drawn into a wire), good conductor and low density

Question 7 of 20

8.

State whether covalent substances conduct electricity, and explain why

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

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

Question 8 of 20

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

Covalent

Covalent or ionic

Ionic

Metallic

Question 9 of 20

10. 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 electrons. Giant Structure.

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

Positive metal ions. Delocalised negative ions. Giant Structure.

Question 10 of 20

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

A pair of electrons is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

A single electron is transferred from bromine to hydrogen

A shared pair of electrons is attracted to one nucleus

Question 11 of 20

12. What does the word malleable mean?

Able to be drawn into a wire

Will break or crack under pressure

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

Able to carry current

Question 12 of 20

13. 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 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

Question 13 of 20

14. 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 the attraction between positive metal ions and a sea of delocalised electrons

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

A giant structure held together by intermolecular forces

Question 14 of 20

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

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

Question 15 of 20

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

Fe⁺ and S⁻

Fe²⁺ and S²⁻

Fe³⁺ and S³⁻

Fe³⁺ and S²⁻

Question 16 of 20

17. Do larger molecules have higher or lower boiling points than smaller molecules?

Size doesn\'t affect boiling point

Lower

Higher

It depends on which atoms are present

Question 17 of 20

18. Describe the structure of metals

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 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 18 of 20

19. Do ionic substances conduct electricity?

No, ionic substances never conduct electricity

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

Yes, ionic substances always conduct electricity

Only when molten

Question 19 of 20

20. Explain, in terms of its structure, why graphite can act as a lubricant.

Graphite has a low melting point so becomes liquid when heated by friction

Graphite is a smooth metal so creates a surface with little friction

Graphite has weak forces of attraction between layers. These layers can slide over each other

Graphite has strong forces of attraction between layers. These layers can slide over each other

Question 20 of 20

Structure & Bonding (Triple) quiz

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