Chemistry Chapter 4 - (Ionic, Covalent And Metallic Bonding)

Why do atoms react with one another?

To achieve a full and stable noble gas electronic configuration.

What are noble gases and why are they like this?

Noble gases are inert (unreactive) because they have full outer shells.

What are the three types of bonding?

Ionic, Covalent and Metallic.

Define the term “Ionic Bond”.

A strong electrostatic attraction between oppositely charged ions.

Properties of an Ionic Structure.

Giant lattice structure.

High melting and boiling points.

Low volatility.

Define the term “Covalent Bond”.

A pair of electrons shared between two atoms.

Simple Molecular Properties.

Low melting and boiling points.

Volatile.

Do not conduct electricity.

What are Giant Covalent Structures?

A 3D regular arrangement of atoms or molecules joined by strong covalent bonds.

Physical properties of Giant Covalent Structures.

High melting and boiling points.

Solid at room temperature.

Do not conduct electricity (Except Graphite).

What is Diamond and what is it used for?

Valuable gemstone.

Used to make the tips of drills and cutting edges.

Properties of Diamond.

Very hard.

High melting and boiling points.

Very strong covalent bonds.

What is Graphite and what is it used for?

Soft, slippery and fairly unreactive.

Used for dry lubricants.

Properties of Graphite.

Conducts electricity from its free moving outer electrons (delocalised).

High melting and boiling points.

What is Silicon (IV) Oxide and what is it used for?

Made of up silicon and oxygen.

Used to make glass.

Properties of Silicon (IV) Oxide.

Very hard.

High melting and boiling points.

Do not conduct electricity (no free-moving electrons).

Define the term “Metallic Bonding”.

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

Structure of Metals.

Giant lattice structure.

Delocalised electrons moving freely.

Properties of Metals.

Good electrical conductivity (e.g Copper/Aluminium).

Malleable and Ductile.