Simple Molecules & Covalent Bonding quiz

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

Solid

Solid or liquid

Gas or liquid

Any state

Question 1 of 16

2. Give the definition of a covalent bond

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

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

Question 2 of 16

3. Which particle(s) in an atom has a positive charge?

Protons and electrons

Electron

Neutron

proton

Question 3 of 16

4. Describe the test for carbon dioxide gas

Turns moist litmus paper white (bleaches)

Bubble the gas through limewater and see if it goes cloudy

Relights a glowing splint

Turns damp red litmus paper blue

Question 4 of 16

5. Describe the formation of a covalent bond

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

The sharing of a single electron between two nuclei

The transfer of electrons from one atom to another

The sharing of a pair of electrons between two nuclei

Question 5 of 16

6. On the Periodic Table what is the meaning of the word Period? What does that tell us about the electron configuration of the atom?

Same electronic configuration

Same number of electrons in the inner shell

same number of electrons in the outer shell

same number of electron shells

Question 6 of 16

7.

Explain, in terms of the arrangement of electrons in its atoms, why neon is very unreactive

Neon has the same number of electrons and protons so it is unreactive

Neon is a noble gas

Neon has 8 electrons in the outer shell, so it is full. Therefore it does not easily gain or lose electrons

Neon has an even number of electrons so it does not need to form bonds

Question 7 of 16

8. How many neutrons in a typical atom of sulfur?

15

16

32

42

Question 8 of 16

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

3

4

5

2

Question 9 of 16

10. Why do elements in the same group of the periodic table have similar chemical properties?

Elements in the same group of the periodic table have the same number of electrons in their outer shell

Elements in the same group of the periodic table are all the same type of element (metal, non-metal etc.)

Elements in the same group of the periodic table have different numbers of electrons in their outer shell

Elements in the same group of the periodic table have the same number of protons

Question 10 of 16

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

A Group is a collection of similar elements

A Group is a vertical column of similar elements

A Group is a horizontal row of elements

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

Question 11 of 16

12. How many electron shells do the elements in the second period have?

2

1

3

4

Question 12 of 16

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

Purple

Blue

White

Cream

Question 13 of 16

14. Where are metals found on the periodic table?

On the left, reaching across the middle

At the top right

Only in the left hand column

Only on the bottom row

Question 14 of 16

15. 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 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

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

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

Question 15 of 16

16. 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 16 of 16

Simple Molecules & Covalent Bonding quiz

Simple Molecules & Covalent Bonding quiz

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