Structure & Bonding (Triple) quiz

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

Fe³⁺ and S²⁻

Fe⁺ and S⁻

Fe³⁺ and S³⁻

Fe²⁺ and S²⁻

Question 1 of 20

2. 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 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

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

Question 2 of 20

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

Hydrogen

Silicon

Carbon

Sulfur

Question 3 of 20

4. Explain, in terms of structure and bonding, why magnesium oxide has a higher melting point than sodium chloride

NaCl and MgO both have a giant ionic structure with strong electrostatic forces between oppositely charged ions. The Ions in MgO have a charge of 2 and -2, but in NaCl the charges are 1 and -1. So the bonds in MgO require more energy to break

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

Question 4 of 20

5.

State whether covalent substances conduct electricity, and explain why

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

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

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

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

Question 5 of 20

6. Do ionic substances conduct electricity?

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

Only when molten

No, ionic substances never conduct electricity

Yes, ionic substances always conduct electricity

Question 6 of 20

7. 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 +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

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

Question 7 of 20

8. Alloys contain different sized positive ions. What properties does this give alloys compared to pure metals?

Alloys are harder and less malleable than pure metals

Alloys are harder and more magnetic than pure metals

Alloys are more ductile than pure metals

Alloys are more magnetic than pure metals

Question 8 of 20

9. Typically, do covalent substances conduct electricity?

Yes

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

Depends on the substance

No

Question 9 of 20

10. What does the word malleable mean?

Will break or crack under pressure

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

Able to carry current

Able to be drawn into a wire

Question 10 of 20

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

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

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

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 11 of 20

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

It depends on which atoms are present

Higher

Lower

Size doesn\'t affect boiling point

Question 12 of 20

13. Explain whether solid ionic compounds conduct electricity

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 can conduct electricity because there is a sea of delocalised electrons that can move

Solid ionic compounds sometimes conduct electricity, only when the ions are free to move

Question 13 of 20

14. Describe the bonding in a metal

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

The strong electrostatic attraction between protons and neutrons

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

The strong electrostatic attraction between oppositely charged ions

Question 14 of 20

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

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

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

Question 15 of 20

16. 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.

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.

Question 16 of 20

17. State two properties of aluminium that make it suitable for use in food cans

Malleable and low density

Light and resists corrosion

Light and reactive

Ductile and malleable

Question 17 of 20

18. Suggest why buckminsterfullerene, C₆₀, has a low melting point.

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

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

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

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

Question 18 of 20

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

A shared pair of electrons is attracted to 2 nuclei

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

Question 19 of 20

20. Describe the formation of a covalent bond

The sharing of a single electron between two nuclei

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

Question 20 of 20

Structure & Bonding (Triple) quiz

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