Structure & Bonding (Double) quiz

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

Solid or liquid

Gas or liquid

Any state

Solid

Question 1 of 12

2. Do ionic substances conduct electricity?

Only when molten

Yes, ionic substances always conduct electricity

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

No, ionic substances never conduct electricity

Question 2 of 12

3. 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 3 of 12

4. 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 4 of 12

5. Typically, do covalent substances conduct electricity?

Depends on the substance

Yes

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

Question 5 of 12

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

There should be zero electrons in areas 1 and 3, and two electrons in area 2

There should be zero electrons in area 1, two electrons in area 2, and six electrons in area 3

There should be one electron in area 1, two electrons in area 2, and seven electrons in area 3

There should be six electrons in area 1, two electrons in area 2, and six electrons in area 3

Question 6 of 12

7. 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 giant metallic structure with weak forces of attraction between layers

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

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

Question 7 of 12

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

Graphite has layers which can easily slide over each other

Graphite has delocalised protons which can move

Graphite has positive ions which can move

Graphite has delocalised electrons which can move

Question 8 of 12

9. Why is the melting point of a smaller molecule lower than that of a larger molecule?

Larger molecules have fewer attractions between them. These take more energy to overcome.

Larger molecules have more attractions between them. These take more energy to overcome.

Larger molecules have more attractions between them. These take less energy to overcome.

Larger molecules have fewer attractions between them. These take less energy to overcome.

Question 9 of 12

10. Explain, in terms of structure and bonding, why sodium chloride has a very high melting point

NaCl has a giant ionic structure with weak electrostatic forces between oppositely charged ions that require little energy to break

NaCl has a simple molecular structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to break

NaCl has a simple molecular structure with weak intermolecular forces that require little energy to break

NaCl has a giant ionic structure with strong electrostatic forces between oppositely charged ions that require a lot of energy to break

Question 10 of 12

11. What holds ions together?

Ions are held together by a strong magnetic attraction between the oppositely charged ions

Ions are held together by a strong electrostatic attraction between the shared pair of electrons and their nuclei

Ions are held together by a strong electrostatic attraction between the oppositely charged ions

Ions are held together by a strong electrostatic attraction between the similarly charged ions

Question 11 of 12

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

A single electron is transferred from bromine to hydrogen

A pair of electrons is transferred from bromine to hydrogen

A shared pair of electrons is attracted to 2 nuclei

A shared pair of electrons is attracted to one nucleus

Question 12 of 12

Structure & Bonding (Double) quiz

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