Structure & Bonding (Triple) quiz

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

Carbon

Silicon

Hydrogen

Sulfur

Question 1 of 20

2. Explain why methane gas, CH₄, is a gas at room temperature

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

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

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

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

Question 2 of 20

3. 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 metallic structure with weak forces of attraction between layers

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 strong intermolecular forces that require a lot of energy to overcome

Question 3 of 20

4. 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 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 is a smooth metal so creates a surface with little friction

Question 4 of 20

5. Explain why metals are malleable

Metals have layers of ions that can slide over each other

Metals have delocalised protons which can move

Metals have delocalised electrons which are free to move

Metals have strong covalent bonds which require a lot of energy to break

Question 5 of 20

6. Do ionic substances conduct electricity?

Only when molten

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

Yes, ionic substances always conduct electricity

No, ionic substances never conduct electricity

Question 6 of 20

7. Describe the structure of metals

A giant random 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 regular 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

Question 7 of 20

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

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

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

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

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

Question 8 of 20

9. Explain what is meant by electric current

The rate of flow of charged particles (e.g. of electrons or ions)

The rate of flow of electrons only

The rate of flow of elephants

The rate of flow of ions only

Question 9 of 20

10. 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, two electrons in area 2, and four 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 three electrons in area 1, two electrons in area 2, and three electrons in area 3

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

Question 10 of 20

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

Fe³⁺ and S³⁻

Fe²⁺ and S²⁻

Fe⁺ and S⁻

Fe³⁺ and S²⁻

Question 11 of 20

12. 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 12 of 20

13. 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 13 of 20

14. 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 14 of 20

15. Describe the formation of a covalent bond

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

The sharing of a pair of electrons between two nuclei

The sharing of a single electron between two nuclei

The transfer of electrons from one atom to another

Question 15 of 20

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

Size doesn\'t affect boiling point

It depends on which atoms are present

Lower

Higher

Question 16 of 20

17. Give the definition of a covalent bond

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

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

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

Strong electrostatic attraction between oppositely charged ions

Question 17 of 20

18. 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 18 of 20

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

There are 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 no charged particles that are free to move

Question 19 of 20

20. How can atoms get a full outer shell?

Only transfer (ionic) of electrons

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

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

Conversion of electrons to protons

Question 20 of 20

Structure & Bonding (Triple) quiz

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