Structure & Bonding (Triple) quiz

1. 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 1 of 20

2. 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 there is a sea of delocalised electrons that can move

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

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

Question 2 of 20

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

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

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

Question 3 of 20

4. What is an alloy?

An alloy is a mixture of a metal and one or more elements, usually other metals or carbon

An alloy is a mixture of a metal and one or more elements, usually other metals or hydrogen

An alloy is a mixture of a non-metal and one or more elements, usually other metals or carbon

An alloy is a mixture of a non-metal and one or more elements, usually other metals or hydrogen

Question 4 of 20

5. 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 simple regular 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

Question 5 of 20

6. Describe the formation of a covalent bond

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

The transfer of electrons from one atom to another

The sharing of a pair of electrons between two nuclei

The sharing of a single electron between two nuclei

Question 6 of 20

7. 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 7 of 20

8. 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

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

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 8 of 20

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

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

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

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

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

Question 9 of 20

10. Why do metals have high melting and boiling points?

There is a strong electrostatic attraction between a regular structure of positive metal ions and a sea of delocalised electrons

There is a strong electrostatic attraction between a regular structure of negative metal ions and a sea of delocalised protons

There is a weak electrostatic attraction between a regular structure of positive metal ions and a sea of delocalised electrons

There is a strong electrostatic attraction between an irregular structure of positive metal ions and a sea of delocalised electrons

Question 10 of 20

11.

State whether covalent substances conduct electricity, and explain why

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

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

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

Question 11 of 20

12. 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 seven 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 six electrons in areas 1 and 3, and two electrons in area 2

Question 12 of 20

13. Typically, do covalent substances conduct electricity?

Depends on the substance

No

Yes

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

Question 13 of 20

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

Higher

Lower

It depends on which atoms are present

Size doesn\'t affect boiling point

Question 14 of 20

15. 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 more ductile than pure metals

Alloys are harder and less malleable than pure metals

Question 15 of 20

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

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

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

Question 16 of 20

17. When can ionic substances conduct electricity?

Only when molten

When molten or dissolved

Never

In any state

Question 17 of 20

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

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

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

Question 18 of 20

19. 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 a nucleus

Strong electrostatic attraction between oppositely charged ions

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

Question 19 of 20

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

Graphite has delocalised electrons which can move

Graphite has delocalised protons which can move

Graphite has positive ions which can move

Graphite has layers which can easily slide over each other

Question 20 of 20

Structure & Bonding (Triple) quiz

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