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What Are Metallic Bonds | Properties of Matter | Chemistry | FuseSchool - YouTube
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Metals are used in many everyday objects.
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This morning when I woke up I decided to have a soft-boiled egg and a cup of
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coffee.
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The pot I used is made of metal. The
kettle is made of plastic, but the coiled
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heating element inside it is made of
metal. Metals are good conductors of heat.
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This is the reason why metals are used to make these everyday objects.
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You would never see a pot made of wood or heating element made of plastic.
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Metals are also good conductors of
electricity.
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The wire connecting your kettle to the
electrical socket is actually made of
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many copper wires, insulated with a layer of rubber. Think about the shapes of the
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everyday objects we described. The pot, the heating element inside the kettle,
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and the copper wires. Notice that they
are very different. Metals are malleable.
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This means that they can be moulded into different shapes. Metals are very ductile.
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This means that they can be stretched
into wires. To fully understand these
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properties of metals we must understand metallic bonding.
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When we talk about metallic bonding we are actually describing the
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electrostatic attraction between the
metal ions, arranged in a lattice
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structure and the free-floating
electrons around them.
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Since these electrons are free to move
around, the term sea of electrons is also
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used.
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What is a lattice structure, and where
have you heard this term before?
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Pause the lesson to think about
this and resume when you are done.
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The term 'lattice structure' means that
there is a regular repeating pattern. We
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have heard this term before when
discussing ionic lattices. It is used
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to describe the alternating positions of the metal and nonmetal ions. In metallic
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structures however there are only metal ions. These metal ions are arranged
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side-by-side in a regular repeating
pattern. The free-floating electrons act
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like a glue and hold the structure in
place.
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This is a very strong attraction and
explains why metals have high melting
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and boiling points.
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A lot of heat energy is needed to
overcome this attraction.
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This is also why metals are very good
conductors of heat. Free-floating
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electrons are the reason why metals can conduct electricity.
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Metals are malleable and ductile because no matter what shape the metal takes, the
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free-floating electrons will conform to
that shape. The strong electrostatic
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attraction will remain and therefore the structure stays intact.
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Let's think about it: cars, bicycles
trains, planes, buildings, cutlery,
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spectacles, furniture and endless items can be made for metals. To recap the
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electrostatic attraction between metal
ions arranged in the lattice structure
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and free-floating electrons is known as metallic bonding.
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This explains many properties of metals: they are good conductors of heat and
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electricity, have high melting and
boiling points, and are malleable and
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ductile.
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