2.3 - The Metallic Model
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What is a metallic bond?
an electrostatic attraction between a cation lattice and delocalized electrons
What do metallic bonds depend on?
charge of ions and radius of metal ions
What is metallic character?
loss of control of outer electrons which can become delocalized and spread out over the metal structure
Why are metals good conductors of heat?
because delocalized electrons move over closely packed cations, carrying thermal energy
Why are metals good conductors of electricity?
because delocalized electrons carry charges around
Why are metals malleable/ductile?
because metallic bonds stay in place while electrons move around and the electrons are non-directional even when deformed
Why do metals have a high melting point?
because a high amount of energy is required to overcome the force of attraction between the atoms
Why are metals lustrous?
because delocalized electrons in the crystal structure reflect light
What is metallic bond strength determined by?
number of delocalized electrons (more=stronger), charge of cation (higher=stronger), radius of cation (smaller=stronger)
Why does the strength of metallic bonding decrease down a column of the periodic table?
because ionic radius increases
Why do transition metals have even higher melting points?
because there are even more electrons available for delocalization in the d block because the 4s and 3d are close in energy