C3 Structure & Bonding

Question 1

Covalent bond

Answer 1

The attraction between two atoms that share one or more electrons

Question 2

Ionic bond

Answer 2

The electrostatic force of attraction between positively and negatively charged ions

Question 3

Intermolecular forces

Answer 3

The attraction between the individual molecules in a covalently bonded substance

Question 4

Polymer

Answer 4

A substance made from very large molecules made up of repeating units

Question 5

Delocalized electrons

Answer 5

Bonding electron that is no longer associated with any one particular atom

Question 6

Fullerene

Answer 6

Form of the elements carbon that can exist as large cage like structures, based on hexagonal rings of carbon atoms

Question 7

Metallic bonding

Answer 7

the electrostatic attraction between the positively charged atom nuclei of metal electrons and the delocalized electrons in a metal

Question 8

Alloy

Answer 8

A mixture of two or more elements, at least one of which is a metal

Question 9

Structures and properties

Answer 9

Graphite: a form of carbon in which the atoms form layers. Layers can slide over each other, so graphite is much softer than diamond. It is used in pencils. each carbon atom in a layer is joined to 3 other carbons. Conduct electricity

Question 10

Structures and properties

Answer 10

Diamond: a form of carbon where each carbon atom is joined to four other carbons. Diamond is very hard and has a high melting point. It does not conduct electricity.

Question 11

Structures and properties

Answer 11

Silica: similar structure to diamond. It is hard and has a high melting point. Contains silicon and oxygen atoms, instead of carbon atoms. It is a semiconductor, which makes it useful in the electronics industry

Question 12

Ionic bonding

Answer 12

• electrons are transferred
• ions are formed
• between metals and nonmetals
• high melting/boiling points
• strong electrostatic forces between ions
• conductive when liquid/molten

Question 13

Covalent bonding

Answer 13

• electrons are shared
• no ions are formed
• between nonmetals
• low melting/boiling points
• weak intermolecular forces between molecules
• non-conductive - no free electrons

Question 14

Metallic bonding

Answer 14

Metallic bonding is is the strong attraction between closely packed positive metal ions and a sea of delocalised electrons

• high melting and boiling points as metallic bonds are strong and a lot of energy is needed to break them, this is why metals have high melting and boiling points
• conducting electricity: metals contain electrons that are free to move carrying charge allowing metals to conduct electricity well