Metallic Bonding

Questions and Answers

The strong electrostatic attraction between the metal ions and delocalized electrons (correct)

The arrangement of atoms in regular layers

The ability of the delocalized electrons to carry thermal energy

The positive charge of the metal ions

The ability of the delocalized electrons to move and carry thermal energy and electric current (correct)

The arrangement of atoms in regular layers

The strong electrostatic attraction between the metal ions and delocalized electrons

The positive charge of the metal ions

The ability of the delocalized electrons to move and carry thermal energy and electric current

The arrangement of atoms in regular layers

The strong electrostatic attraction between the metal ions and delocalized electrons

The ability of the layers of atoms to slide over each other (correct)

The distortion of the layers of atoms due to the different sizes of atoms Signup and view all the answers

A sea of delocalized electrons Signup and view all the answers

A positive metal ion Signup and view all the answers

Study Notes

Metals consist of a giant structure of atoms arranged in regular layers.
In metals, the outer electrons are delocalized, meaning they are not attached to any individual atom and are free to move through the whole structure.
These delocalized electrons are often referred to as a "sea of delocalized electrons".
Each metal atom loses its outer electron, resulting in positive metal ions.
The strong electrostatic attraction between the sea of delocalized negative electrons and the positive metal ions is called a metallic bond.

Metals have high melting and boiling points due to the strong metallic bonds that need to be broken.
Metals are excellent conductors of heat and electricity due to the delocalized electrons that can move and carry thermal energy and electric current.
Metals can be bent and shaped because the layers of atoms can slide over each other.

An alloy is a mixture of metals.
In an alloy, the different sizes of atoms distort the layers, making it more difficult for the layers to slide over each other.
This makes alloys harder than pure metals.
Examples of metals that can be made harder by forming an alloy include copper, gold, iron, and aluminum.

Metals have a giant structure of atoms arranged in regular layers, with outer electrons delocalized, meaning they're not attached to individual atoms and can move freely.
Delocalized electrons form a "sea of electrons" that allows them to move through the entire structure.
Metal atoms lose their outer electrons, resulting in positive metal ions.
The strong electrostatic attraction between the delocalized negative electrons and positive metal ions is called a metallic bond.

Metals have high melting and boiling points due to strong metallic bonds that need to be broken.
Metals are excellent conductors of heat and electricity because delocalized electrons can move and carry thermal energy and electric current.
Metals can be bent and shaped because the layers of atoms can slide over each other.

An alloy is a mixture of metals, where different-sized atoms distort the layers, making it harder for the layers to slide over each other.
Alloys are harder than pure metals due to the distorted layers.
Examples of metals that can be made harder by forming an alloy include copper, gold, iron, and aluminum.