Metallic bonding
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6 Terms
Describe metallic bonding.
In metallic bonding, positive metal ions are held together by their attraction to a “sea” of delocalised electrons.
not fixed.
State the properties of metals.
High melting and boiling points
Good conductors of heat / electricity
Malleable & ductile
Why do metals have high melting and boiling points?
Strong attraction between the metal ions and electrons- requires a lot of energy to break.
Why are metals good conductors of heat / electricity?
Due to the 'sea’ of delocalised electrons- electrons are mobile and can transfer heat energy / electrical charge.
Why are metals malleable and ductile?
Electrons behave as a lubricant and the positive metal ions can move over each other.
What affects the strength of the metallic bonding?
The number of electrons in which the atom 'delocalises' into the sea of electrons.
The more free electrons, the greater the charge on the ion and therefore, the stronger the metallic bond.
For instance, a metal with a higher charge will have a higher melting and boiling point because the electrostatic forces are stronger so takes more heat energy to break.