Metallic Bonding and Alloys Flashcards

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What is metallic bonding?

Metallic bonding is the strong attraction between positive metal ions and delocalised electrons. This force holds the metal atoms together in a giant structure.

Describe the structure of a solid metal in terms of ions and electrons.

In a solid metal, atoms lose their outer electrons and become positive ions. The outer electrons become delocalised and move freely between the ions in a giant lattice.

Why can metals conduct electricity?

Metals can conduct electricity because they have delocalised electrons. These electrons can move through the metal and carry an electric charge.

Why do most metals have high melting and boiling points?

There are strong forces of attraction between the positive metal ions and the delocalised electrons. These forces are very strong. A lot of energy is needed to break them, so metals have high melting and boiling points.

Why are pure metals usually malleable and ductile?

In pure metals, the ions are arranged in regular layers. These layers can slide over each other. This means the metal can bend (malleable) or be drawn into wires (ductile).

What is an alloy?

An alloy is a mixture of a metal with other elements, usually other metals or carbon. The atoms in an alloy are not all the same size.

Why are alloys usually harder than pure metals?

In an alloy, different sized atoms distort the regular layers of ions. This makes it harder for the layers to slide. The alloy is therefore harder and less easy to bend.

Why are alloys often used instead of pure metals?

Alloys often have better properties than pure metals, such as being harder, stronger or more resistant to corrosion. This makes them more useful for tools, machines and everyday objects.

Give one example of an alloy and state one of its uses.

Steel is an alloy of iron with carbon and other elements. It is used in buildings and bridges because it is strong and tough.

What does the term 'delocalised electrons' mean in metallic bonding?

Delocalised electrons are outer electrons that are not fixed to one atom. They can move freely through the metal lattice and help form metallic bonds.

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