Metals Flashcards
Metallic Bonding
The outer electrons are delocalised (free to move). This produces an electrostatic force of attraction between the positively charged metal ions, and the negetively charged delocalised electrons
The electrochemcial series
When metals form ions, they give away one or more of their outer electrons. Some metals lose their electrons easily (eg lithium or sodium). Other metal do not give away electrons easily (eg silver or gold).
Reactions of metals
Metals can react with water, acid and oxygen. The reactivity of the metal determines which reactions the metal participates in.
Reactions with water
When metals react with water, metal hydroxides and hydrogen gas are formed.
Reaction with acid
When metal reacts with acid, a salt of the metal an hydrogen gas are formed.
Reactions with oxygen
When metal react with oxygen, metal oxides are formed.
Metal ores
Ores are naturally occuring rocks that contain metals or metal compounds in suffiecient amounts to make it worthwhile extracting them.
stability of the ore/ reactivity of metal
The method used to extract a given metal from its ore depends upon the reactivity of the metal and so how stable the ore is
Oxidation
the loss of electrons by a reactant
Oxidised
when a metal element is reacting to form a compound then it is being oxidised. metals atoms are losing electron to form a ion.
Reduction
it is the gain of electrons
Redox reactions
When both oxidation and reduction are taking place.
Displacement reactions
these are examples of redox reaction as one species is being oxidised while the other is being reduced.
Electrolysis of an ionic compound
- negative ions lose electrons at the positive electrode (oxidation)
- positive ions gain electrons at the negative electrode (reduction)
A simple electrochemical cell
can be produced by dipping two different metals into a electrolyte and connecting them via wires and a voltmeter
