Structure & Bonding (Triple) quiz

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

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

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

Question 1 of 20

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

Ionic

Covalent

Covalent or ionic

Metallic

Question 2 of 20

3. Explain whether solid ionic compounds conduct electricity

Solid ionic compounds can conduct electricity because the ions are free to move

Solid ionic compounds cannot conduct electricity because the ions are not 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

Question 3 of 20

4. 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. Weak intermolecular forces.

Positive metal ions. Delocalised electrons. Giant Structure.

Positive metal ions. Delocalised negative ions. Giant Structure.

Question 4 of 20

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

Size doesn\'t affect boiling point

Higher

It depends on which atoms are present

Lower

Question 5 of 20

6. 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 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 6 of 20

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

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

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

Question 7 of 20

8. What is a mixture of metals called?

An alloy

A compound

A solution

An ore

Question 8 of 20

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

Fe²⁺ and S²⁻

Fe³⁺ and S³⁻

Fe³⁺ and S²⁻

Fe⁺ and S⁻

Question 9 of 20

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

There are no charged particles that are free to move

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

There are charged particles that are free to move

There are weak intermolecular forces that require little energy to break

Question 10 of 20

11. State 3 properties that makes iron suitable for saucepans

Good insulator, high melting point and malleable

Good conductor of heat, high melting point and brittle

Good insulator, high melting point and brittle

Good conductor of heat, high melting point and malleable

Question 11 of 20

12. 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 one nucleus

A shared pair of electrons is attracted to 2 nuclei

Question 12 of 20

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

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

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 a low melting point so becomes liquid when heated by friction

Question 13 of 20

14. What does the word malleable mean?

Able to be drawn into a wire

Able to carry current

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

Will break or crack under pressure

Question 14 of 20

15. Do ionic substances conduct electricity?

No, ionic substances never conduct electricity

Yes, ionic substances always conduct electricity

Only when molten

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

Question 15 of 20

16. 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 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 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 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 16 of 20

17. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of water (H₂O), how many electrons should be shown in areas 1, 2, 3 and 4?

There should be two electrons in each of areas 1 and 2, and zero electrons in areas 3 and 4. There should also be an additional 4 electrons around the outside of the oxygen atom.

There should be two electrons in each of areas 1 and 2, and zero electrons in areas 3 and 4.

There should be four electrons in each of areas 1 and 2, and zero electrons in areas 3 and 4.

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

Question 17 of 20

18. Explain why magnesium oxide has a higher melting point than sodium chloride.

Mg²⁺ and O²⁻ ions have a higher charge than sodium and chloride therefore the electrostatic forces between the ions are much stronger. This requires more energy to break.

Magnesium and oxygen are more reactive elements

Mg²⁺ and O²⁻ ions are larger than sodium and chloride therefore the electrostatic forces between the ions are much stronger. This requires more energy to break.

Sodium chloride is a simple molecular substance so there are only weak intermolecular forces which require little energy to break

Question 18 of 20

19. Describe the bonding in a metal

The strong electrostatic attraction between a shared pair of electrons and two nuclei

The strong electrostatic attraction between oppositely charged ions

The strong electrostatic attraction between protons and neutrons

The strong electrostatic attraction between a regular structure of positive ions and a sea of delocalised electrons

Question 19 of 20

20. Describe the formation of a covalent bond

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

The sharing of a single electron between two nuclei

The sharing of a pair of electrons between two nuclei

The transfer of electrons from one atom to another

Question 20 of 20

Structure & Bonding (Triple) quiz

Related Posts:

Share This Story, Choose Your Platform!