Simple Molecules & Covalent Bonding quiz

1. What is the relative atomic mass (Aᵣ) of a sodium atom?

12

11

24

23

Question 1 of 16

2. Describe the formation of a covalent bond

The sharing of a single electron between two nuclei

The sharing of a pair of electrons between two nuclei

The transfer of electrons from one atom to another

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

Question 2 of 16

3. Explain, in terms of electrons, why isotopes have the same chemical properties

Isotopes have different masses

Isotopes are radioactive

Isotopes have the same number of protons but a different number of neutrons

Isotopes have the same number of electrons

Question 3 of 16

4. What are the two parts of an atom?

The nucleus and the electron cloud

The outside and inside

The centre and the electron shells

The nucleus and the electron shells

Question 4 of 16

5. Where are metals found on the periodic table?

At the top right

Only on the bottom row

Only in the left hand column

On the left, reaching across the middle

Question 5 of 16

6. Give the definition of a covalent bond

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

Strong electrostatic attraction between oppositely charged ions

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

Question 6 of 16

7. On the Periodic table what is the meaning of the word Group?

A Group is collection of elements with the same number of electron shells

A Group is a horizontal row of elements

A Group is a collection of similar elements

A Group is a vertical column of similar elements

Question 7 of 16

8. On the Periodic table what is the meaning of the word Group? What does that tell us about the electron configuration of the atom?

Same electronic configuration

Same number of electron shells

Same number of electrons in the inner shell

same number of electrons in the outer shell

Question 8 of 16

9. What is the total number of atoms in the formula Be(OH)₂ ?

3

5

4

2

Question 9 of 16

10. What is special about the elements in group 0?

They are all coloured gases

They are very unreactive (because they have full outer electron shells)

They are all diatomic

They have the same number of electrons

Question 10 of 16

11. In the dot and cross diagram of the outer electrons showing the covalent bonding of ammonia (NH₃), how many electrons should be shown in areas 1, 2, 3 and 4?

There should be one electron in each of the areas 1, 2, 3 and seven electrons in 4

There should be 2 electrons in each of the areas 1, 2, 3 but none in 4

There should be one electron in each of the areas 1, 2, 3 and five electrons in 4

There should be 2 electrons in each of the areas 1, 2, 3 and 4

Question 11 of 16

12. How many electrons in the outer shell of group 6 elements?

8

6

5

7

Question 12 of 16

13. In the test of a gas, a glowing splint relights. What is the gas?

Carbon dioxide

Hydrogen

Oxygen

Chlorine

Question 13 of 16

14. Explain why carbon dioxide gas, CO₂, is a gas at room temperature

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

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

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

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

Question 14 of 16

15. Why is the boiling point of a larger molecule higher than that of a smaller molecule?

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

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

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

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

Question 15 of 16

16. What colour is hydrated copper (II) sulfate?

White

Cream

Purple

Blue

Question 16 of 16

Simple Molecules & Covalent Bonding quiz

Simple Molecules & Covalent Bonding quiz

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