Structure & Bonding (Triple) quiz

1. 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 a shared pair of electrons and two nuclei

Strong electrostatic attraction between oppositely charged ions

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

Question 1 of 20

2. State a property that makes iron suitable for building

High melting point

Resists corrosion

Magnetic

Strong

Question 2 of 20

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

Covalent

Ionic

Covalent or ionic

Metallic

Question 3 of 20

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

Alloys are harder and more magnetic than pure metals

Alloys are more magnetic than pure metals

Alloys are harder and less malleable than pure metals

Alloys are more ductile than pure metals

Question 4 of 20

5. If a substance has a simple molecular structure, what physical state might it be at room temperature?

Solid

Gas or liquid

Any state

Solid or liquid

Question 5 of 20

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

Lower

Higher

It depends on which atoms are present

Size doesn\'t affect boiling point

Question 6 of 20

7. 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 weak intermolecular forces that require little energy to break

There are charged particles that are free to move

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 electrons. Weak intermolecular forces.

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

Positive metal ions. Delocalised negative ions. Giant Structure.

Question 8 of 20

9. When can ionic substances conduct electricity?

When molten or dissolved

Only when molten

Never

In any state

Question 9 of 20

10. Describe the bonding in a metal

The strong electrostatic attraction between oppositely charged ions

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

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 10 of 20

11. What is a mixture of metals called?

An ore

A solution

An alloy

A compound

Question 11 of 20

12. Why do ionic compounds conduct electricity only when molten or in solution?

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

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

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

Question 12 of 20

13. 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 weak intermolecular forces that require little energy to overcome

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

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

Question 13 of 20

14. Describe the formation of a covalent bond

The transfer of electrons from one atom to another

The sharing of a single electron between two nuclei

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

The sharing of a pair of electrons between two nuclei

Question 14 of 20

15. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of oxygen (O₂), how many electrons should be shown in areas 1, 2 and 3?

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

There should be three electrons in area 1, two electrons in area 2, and three 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 15 of 20

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

Graphite has layers which can easily slide over each other

Graphite has delocalised electrons which can move

Graphite has delocalised protons which can move

Graphite has positive ions which can move

Question 16 of 20

17. Why do ionic substance have high melting and boiling points?

There is a strong electrostatic attraction between similarly charged ions, in a giant structure, which requires a lot of energy to overcome

There is a weak electrostatic attraction between oppositely charged ions, in a giant structure, which requires little energy to overcome

There are weak intermolecular forces, in a simple molecular structure, which require little energy to overcome

There is a strong electrostatic attraction between oppositely charged ions, in a giant structure, which requires a lot of energy to overcome

Question 17 of 20

18. Explain why metals are good conductors of electricity

Metals have positive ions which can move

Metals have delocalised electrons which are free to move

Metals have layers of ions that can slide over each other

Metals have delocalised protons which can move

Question 18 of 20

19. What is needed to complete this diagram to show the ionic bonding in sodium chloride, NaCl ?

1) eight electrons around the chloride (seven dots and one cross) 2) A charge of +1 on the sodium and -1 on the chloride

1) seven electrons around the sodium 2) one electon around the chloride 3) A charge of +1 on the sodium and -1 on the chloride

1) seven electrons around the chloride 2) one electon around the sodium 3) A charge of +1 on the sodium and -1 on the chloride

1) eight electrons around the chloride (seven dots and one cross) 2) A charge of -1 on the sodium and +1 on the chloride

Question 19 of 20

20. When are ions attracted to each other?

When the ions are the same size

When the ions are very small

When the ions are oppositely charged

When the ions have the same charge

Question 20 of 20

Structure & Bonding (Triple) quiz

Structure & Bonding (Triple) quiz

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