Structure & Bonding (Triple) quiz

1. What does the word malleable mean?

Able to carry current

Will break or crack under pressure

Able to be drawn into a wire

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

Question 1 of 20

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

A single electron is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

A pair of electrons is transferred from bromine to hydrogen

A shared pair of electrons is attracted to one nucleus

Question 2 of 20

3. Do ionic substances conduct electricity?

Yes, ionic substances always conduct electricity

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

Only when molten

No, ionic substances never conduct electricity

Question 3 of 20

4. 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 4 of 20

5. Describe the formation of a covalent bond

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 pair of electrons between two nuclei

The sharing of a single electron between two nuclei

Question 5 of 20

6. Describe the structure of metals

A giant 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 simple regular structure of positive metal ions surrounded by a sea of delocalised electrons

Question 6 of 20

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

Fe³⁺ and S²⁻

Fe³⁺ and S³⁻

Fe²⁺ and S²⁻

Fe⁺ and S⁻

Question 7 of 20

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

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

Question 8 of 20

9. Why are alloys harder than pure metals?

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

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

Alloys often contain carbon which is a very hard element

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

Question 9 of 20

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

It depends on which atoms are present

Size doesn\'t affect boiling point

Lower

Higher

Question 10 of 20

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

Hydrogen

Sulfur

Silicon

Carbon

Question 11 of 20

12. 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 12 of 20

13. How can atoms get a full outer shell?

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

Conversion of electrons to protons

Only transfer (ionic) of electrons

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

Question 13 of 20

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

Solid or liquid

Gas or liquid

Solid

Any state

Question 14 of 20

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

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

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

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

Question 15 of 20

16. In the dot and cross diagram of the outer electrons showing the covalent bonding in a molecule of ethane (C₂H₆), how many electrons should be shown in areas 1, 2, 3, 4, 5, 6 and 7?

There should be two electrons in each of areas 1, 2, 3, 4, 5, 6 and 7, and also two more on the outside of each hydrogen atom

There should be two electrons in each of areas 1, 3, 4, 5, 6 and 7, but none in area 2

There should be two electrons in each of areas 1, 2, 3, 4, 5, 6 and 7, and also seven more on the outside of each hydrogen atom

There should be two electrons in each of areas 1, 2, 3, 4, 5, 6 and 7

Question 16 of 20

17. State a property that makes iron suitable for building

Magnetic

Strong

Resists corrosion

High melting point

Question 17 of 20

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

There are charged particles that are free to move

There are weak intermolecular forces that require little energy to break

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

There are no charged particles that are free to move

Question 18 of 20

19. Typically, do covalent substances conduct electricity?

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

Depends on the substance

Yes

No

Question 19 of 20

20. 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 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

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

Question 20 of 20

Structure & Bonding (Triple) quiz

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