a

What Are Metallic Bonds? | Properties of Matter | Chemistry | FuseSchool

Metals are used in many everyday objects.

This morning when I woke up I decided to have a soft-boiled egg and a cup of

coffee.

The pot I used is made of metal. The kettle is made of plastic, but the coiled

heating element inside it is made of metal. Metals are good conductors of heat.

This is the reason why metals are used to make these everyday objects.

You would never see a pot made of wood or heating element made of plastic.

Metals are also good conductors of electricity.

The wire connecting your kettle to the electrical socket is actually made of

many copper wires, insulated with a layer of rubber. Think about the shapes of the

everyday objects we described. The pot, the heating element inside the kettle,

and the copper wires. Notice that they are very different. Metals are malleable.

This means that they can be moulded into different shapes. Metals are very ductile.

This means that they can be stretched into wires. To fully understand these

properties of metals we must understand metallic bonding.

When we talk about metallic bonding we are actually describing the

electrostatic attraction between the metal ions, arranged in a lattice

structure and the free-floating electrons around them.

Since these electrons are free to move around, the term sea of electrons is also

used.

What is a lattice structure, and where have you heard this term before?

Pause the lesson to think about this and resume when you are done.

The term 'lattice structure' means that there is a regular repeating pattern. We

have heard this term before when discussing ionic lattices. It is used

to describe the alternating positions of the metal and nonmetal ions. In metallic

structures however there are only metal ions. These metal ions are arranged

side-by-side in a regular repeating pattern. The free-floating electrons act

like a glue and hold the structure in place.

This is a very strong attraction and explains why metals have high melting

and boiling points.

A lot of heat energy is needed to overcome this attraction.

This is also why metals are very good conductors of heat. Free-floating

electrons are the reason why metals can conduct electricity.

Metals are malleable and ductile because no matter what shape the metal takes, the

free-floating electrons will conform to that shape. The strong electrostatic

attraction will remain and therefore the structure stays intact.

Let's think about it: cars, bicycles trains, planes, buildings, cutlery,

spectacles, furniture and endless items can be made for metals. To recap the

electrostatic attraction between metal ions arranged in the lattice structure

and free-floating electrons is known as metallic bonding.

This explains many properties of metals: they are good conductors of heat and

electricity, have high melting and boiling points, and are malleable and

ductile.