7D - Metallic Bonding Review

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

Why do metals have high electrical conductivity?

Back

Metals have high electrical conductivity because they contain delocalized electrons that can move freely, allowing electric current to flow.

Front

What does it mean for a metal to be malleable?

Back

A metal is malleable if it can be hammered or pressed into shape without breaking.

Front

What are delocalized electrons?

Back

Delocalized electrons are electrons that are not associated with a single atom or bond and can move freely within the metallic structure.

Front

What is the state of most metals at room temperature?

Back

Most metals are solid at room temperature.

Front

How does metallic bonding affect the properties of metals?

Back

Metallic bonding gives metals properties such as electrical conductivity, malleability, ductility, and luster.

Front

What is ductility in metals?

Back

Ductility is the ability of a metal to be drawn into wires without breaking.

Front

What is the difference between metallic and ionic bonding?

Back

Metallic bonding involves delocalized electrons and metal ions, while ionic bonding involves the transfer of electrons from one atom to another, forming charged ions.

Front

Why are metals shiny?

Back

Metals are shiny because they reflect light due to the presence of free electrons that can absorb and re-emit light.

Front

What is the significance of the term 'oxidation number' in metallic bonding?

Back

The oxidation number indicates the charge of an atom in a compound, but in metallic bonding, it is less relevant as metals share electrons.