Electrons in metallic bonds are called "delocalized electrons", which means they exist in an atoms orbitals, but are extended over multiple atoms. It is often called a "sea of electrons" because the electrons are free to "roam" between atoms, and is what gives metal the ability to conduct electricity.
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their valence electrons are free-roaming they allow for the conductivity of electricity APEX :) <3 JAmie
Free- Roaming electrons, and conductivity
A positive metal ion and the electrons surrounding it.
Metallic bonds don't really have a shape. They are sometimes described as a cloud or sea of electrons.
Metallic bonds involve free electrons delocalised over the metal. A very simple description is a sea of electrons with positivelly charged metal atoms.
their valence electrons are free-roaming they allow for the conductivity of electricity APEX :) <3 JAmie
Free- Roaming electrons, and conductivity
Metallic bonds as found in metals
A positive metal ion and the electrons surrounding it.
are formed by electrons that are delocalized throughout the object bonded by the metallic bonds.
Metallic bonds don't really have a shape. They are sometimes described as a cloud or sea of electrons.
Metallic bonds.
Covalent (molecular) bonds share electrons, while ionic bonds transfer electrons.
Metallic bonding is found in gold or copper
Metallic bonds involve free electrons delocalised over the metal. A very simple description is a sea of electrons with positivelly charged metal atoms.
The formation of metallic bonds causes them to be flexible and strong. Metallic bonds become strong because positive and negative charged electrons have a strong force of attraction. Metallic bonds are flexible because of their malleability.
Whichever metal can contribute the most valence electrons will form the strongest metallic bonds.