Chemists use models to explain observable properties. A model which attempts to explain the attractive forces between atoms in a metal must account for properties of metals such as their
One model which explains the observed properties of metals has metals existing as cations in a sea of electrons.
This is consistent with the known tendency of metals to react to form cations.
Metallic bonding is due to the sharing of the outer electrons released in formation of a metal cation with other metal cations in the lattice.
How does the model explain conduction of electricity and heat by metals?
Conduction of electricity is movement of charge.
In this model, the electrons are not associated with any particular cation, and they are small enough to move through the lattice.
The movement of electrons is also responsible for the conduction of heat.
Is the model consistent with the malleability and ductility of metals?
In this model, the electrons "swim" around the cations.
The strength of the metallic bonding does not depend on any particular orientation of the cations and the electrons.
Hammering into a sheet or drawing the metal into a wire may temporarily disturb the orientation of the layers of cations and their electrons with respect to one another but it does not change the attractive force between the cations and the electrons around them.
Is the model consistent with the wide range of boiling point for metals?
The strength of the metallic bond is related to the number of electrons in the electron sea.
Group 1 metals which have 1 electron per cation in the electron sea are lower boiling that Group 2 metals which have 2 electrons per cation in the electron sea.
ductility, malleability, conduction of electricity and heat, high boiling points
Copper modeled as cations in electron sea
This is consistent with the known tendency of metals to react to form cations.
Metallic bonding is due to the sharing of the outer electrons released in formation of a metal cation with other metal cations in the lattice.
How does the model explain conduction of electricity and heat by metals?
Conduction of electricity is movement of charge.
In this model, the electrons are not associated with any particular cation, and they are small enough to move through the lattice.
The movement of electrons is also responsible for the conduction of heat.
Is the model consistent with the malleability and ductility of metals?
In this model, the electrons "swim" around the cations.
The strength of the metallic bonding does not depend on any particular orientation of the cations and the electrons.
Hammering into a sheet or drawing the metal into a wire may temporarily disturb the orientation of the layers of cations and their electrons with respect to one another but it does not change the attractive force between the cations and the electrons around them.
Is the model consistent with the wide range of boiling point for metals?
The strength of the metallic bond is related to the number of electrons in the electron sea.
Group 1 metals which have 1 electron per cation in the electron sea are lower boiling that Group 2 metals which have 2 electrons per cation in the electron sea.