Bonding, Structure and Properties of Matter

Question 1

What is ionic bonding?

Answer 1

The transfer of electrons from metal atoms to non-metal atoms, forming ions

Question 2

What type of elements form ionic bonds?

Answer 2

Metal and non-metal

Question 3

What are the charges on ions formed in ionic bonding?

Answer 3

Metals form positive ions, non-metals form negative ions

Question 4

Why do ionic compounds have high melting and boiling points?

Answer 4

Strong electrostatic forces between ions require lots of energy to overcome

Question 5

What is a covalent bond?

Answer 5

A shared pair of electrons between two atoms

Question 6

What types of elements form covalent bonds?

Answer 6

Non-metal atoms

Question 7

What is a simple molecular substance?

Answer 7

Substances made of molecules with a small number of atoms bonded covalently

Question 8

Why do simple molecular substances have low melting and boiling points?

Answer 8

Weak intermolecular forces between molecules are easily overcome

Question 9

What is a giant ionic lattice?

Answer 9

A regular structure of ions held together by strong ionic bonds

Question 10

Why are ionic compounds brittle?

Answer 10

When layers shift, ions of the same charge repel each other causing the lattice to break

Question 11

What is metallic bonding?

Answer 11

Attraction between positive metal ions and a sea of delocalised electrons

Question 12

Why do metals conduct electricity?

Answer 12

Delocalised electrons can move through the metal and carry charge

Question 13

Why do metals have high melting and boiling points?

Answer 13

Strong metallic bonds require lots of energy to break

Question 14

What is a simple molecular substance?

Answer 14

Molecules with strong covalent bonds inside but weak intermolecular forces between molecules

Question 15

What is a giant covalent structure?

Answer 15

A large network of atoms bonded covalently throughout the structure

Question 16

Name two examples of giant covalent structures.

Answer 16

Diamond and graphite

Question 17

Why does diamond have a very high melting point?

Answer 17

Strong covalent bonds throughout the lattice require lots of energy to break

Question 18

Why is graphite soft and slippery?

Answer 18

Layers can slide over each other because of weak forces between layers

Question 19

Why does graphite conduct electricity?

Answer 19

Each carbon atom has one free electron that can move between layers

Question 20

What are nanoparticles?

Answer 20

Particles sized between 1 and 100 nanometers

Question 21

Why do nanoparticles have a large surface area to volume ratio?

Answer 21

Because their size is extremely small

Question 22

Give one use of nanoparticles.

Answer 22

Catalysts in chemical reactions

Question 23

Give one potential risk of nanoparticles.

Answer 23

They might be toxic or have unknown health effects

Question 24

What is a covalent bond’s electron sharing?

Answer 24

A shared pair of electrons between atoms

Question 25

How do covalent bonds hold atoms together?

Answer 25

By the electrostatic attraction between the shared electrons and the nuclei

Question 26

What is the difference between diamond and graphite?

Answer 26

Diamond: each carbon bonded to 4 others; graphite: carbon bonded to 3 with layers

Question 27

Why is diamond a good cutting tool?

Answer 27

It is very hard because of its rigid 3D covalent structure

Question 28

Why can graphite conduct electricity but diamond cannot?

Answer 28

Graphite has delocalised electrons; diamond does not

Question 29

Why do ionic compounds conduct electricity when molten or dissolved but not solid?

Answer 29

Ions are free to move and carry charge when molten or dissolved

Question 30

What are the properties of metals?

Answer 30

Malleable, ductile, conduct electricity and heat, high melting points

Question 31

What causes metals to be malleable?

Answer 31

Layers of atoms can slide over each other without breaking bonds

Question 32

Explain why sodium chloride has a high melting point.

Answer 32

Strong ionic bonds require a lot of energy to break

Question 33

Explain why water has a low melting point despite having hydrogen bonds.

Answer 33

Hydrogen bonds are weaker than ionic or covalent bonds

Question 34

How do intermolecular forces affect melting and boiling points?

Answer 34

Stronger intermolecular forces mean higher melting and boiling points

Question 35

What is a molecule?

Answer 35

Two or more atoms bonded covalently

Question 36

What is an alloy?

Answer 36

A mixture of metals or metals with other elements

Question 37

Why are alloys harder than pure metals?

Answer 37

Different sized atoms distort the layers, making them harder to slide

Question 38

What is a polymer?

Answer 38

A long chain molecule made of many repeating units

Question 39

Give an example of a polymer.

Answer 39

Polyethene

Question 40

How does the strength of covalent bonds compare to intermolecular forces?

Answer 40

Covalent bonds are much stronger than intermolecular forces

Question 41

What type of bonding occurs in hydrogen chloride (HCl)?

Answer 41

Covalent bonding

Question 42

Why do simple molecules not conduct electricity?

Answer 42

They have no free charged particles

Question 43

What bonding does diamond have?

Answer 43

Giant covalent bonding

Question 44

What bonding does sodium chloride have?

Answer 44

Ionic bonding