8) Metallic Bonding:

What is metallic bonding?

Metallic bonding is the electrostatic attraction between positive metal ions and delocalised electrons in a regular structure.

What role do delocalised electrons play in metals?

Delocalised electrons in metals produce their characteristic properties, such as high conductivity and malleability.

Why are most metals solid at room temperature?

Most metals are solid at room temperature because the strong electrostatic forces between metal atoms and delocalised electrons require a lot of energy to break, leading to high melting and boiling points.

Why are metals good conductors of electricity?

Metals are good conductors because delocalised electrons can carry electric charge through the whole structure.

Why are metals good conductors of heat?

Delocalised electrons in metals can carry thermal energy, making them good conductors of heat.

What does it mean for a metal to be malleable?

A metal is malleable if its layers of atoms can slide over each other, allowing it to be bent, hammered, or rolled into flat sheets.

Why are alloys harder than pure metals?

Alloys are harder because different sized atoms distort the metal layers, making it harder for them to slide over each other.

What is an alloy?

An alloy is a mixture of two or more metals (or a metal and another element) designed to be harder and more useful than pure metals.

Why are pure metals often too soft for certain applications?

Pure metals are often too soft, so they are mixed with other elements to form harder alloys for specific uses.

How does metallic bonding contribute to the high melting points of metals?

The strong electrostatic forces between positive metal ions and delocalised electrons in the giant structure require a lot of energy to break, resulting in high melting points.