Chapter 3.1 - Metals
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The outer electrons are delocalised and this produces an electrostatic force of attraction between
The positive metal ions and the negative delocalised electrons, this acts as a glue holding the atoms together.
Metallic bonds occur
Between the atoms of metal elements
The ‘sea’ of delocalised electrons are the reason for metals being
Good conductors of electricity.
As one electron moves into the metal from the power supply, another
Will jump off the metal. Metals remain unchanged throughout the process.
Only the metals above Hydrogen in the reactivity series will react with an
Acid because all acids contain H+ ions.
Only the most reactive metals react strongly with
Oxygen
Most metals don’t react except the very reactive metals such as caesium and potassium with
Water
The flow of electrons in a cell is produced because of the difference in the
reactivity of the two metals
Electrons will flow from the
most reactive metal (oxidation) to the least reactive metal (reduction)
An ion bridge
completes the circuit
A fuel cell converts
chemical energy from a fuel into electrical energy
Rechargeable batteries reverse the direction of the
electrical flow, this revers the chemical reaction making it ready to use again.
In displacement reactions a reactive metal
displaces a metal that is less reactive from solution
When substances lose electrons it is known as
oxidation
when substances gain electrons it is known as
reduction
Mg —> Mg2+ + 2e is a
oxidation reaction
Cu2+ + 2e- —> Cu is a
Reduction reaction
Redox reaction is when both
oxidation and reduction take place
Less reactive metals such as gold are found as pure metal because they are
very unreactive
The more reactive a metal is, the harder it is to
extract
A reducing agent is a substance
that can donate electrons
Most very reactive metals require
electrolysis to be removed