Metallic Bonding

Front

What is metallic bonding?

Back

Metallic bonding is the electrostatic attraction between positively charged metal ions and delocalized electrons that are free to move throughout the structure.

Front

What are delocalized electrons?

Back

Delocalized electrons are electrons in a metal that are not associated with a specific atom and can move freely throughout the metallic structure, contributing to conductivity.

Front

What is ductility in metals?

Back

Ductility is the ability of a substance, particularly metals, to be stretched into a thin wire without breaking.

Front

What is malleability in metals?

Back

Malleability is the ability of a metal to be hammered or pressed into thin sheets without breaking.

Front

What is an alloy?

Back

An alloy is a mixture of two or more elements, where at least one is a metal, designed to enhance certain properties such as strength or corrosion resistance.

Front

Give an example of a common alloy.

Back

Steel, which is an alloy of iron and carbon.

Front

What is the significance of the sea of electrons model in metallic bonding?

Back

The sea of electrons model explains how metals conduct electricity and heat, as the delocalized electrons can move freely.

Front

How does the structure of metals contribute to their properties?

Back

The closely packed arrangement of metal ions and the presence of delocalized electrons contribute to properties like conductivity, malleability, and ductility.

Front

What is the difference between metals and nonmetals in terms of bonding?

Back

Metals typically form metallic bonds characterized by a sea of delocalized electrons, while nonmetals form covalent bonds by sharing electrons.

Front

Why are metals good conductors of electricity?

Back

Metals are good conductors of electricity due to the presence of delocalized electrons that can move freely and carry electric current.