Chemistry/Y4/Metal Reactivity

General Trends
More reactive metals will displace the cations of less reactive metals from their aqueous solution.

e.g. Zn (s) + Cu2+ (aq) &rarr; Zn2+ (aq) + Cu (s)

Table 3: General Trends

Remembering the General Trends

 * The only thing that you need to memorise is that more reactive metals will loose its electrons easier than less reactive metals.
 * Ionisation Energy: Since, more reactive metals looses electrons easily, less energy is required to remove electrons (I.E.) than less reactive metals. Thus, I.E. increases down the reactivity series.
 * Ease of Oxidation: OIL - Oxidation Is Loss of electrons. Since, more reactive metals looses electrons easily, it is easier for more reactive metals to oxidise.
 * Strength as Reducing Agents - Reducing Agents itself gets oxidised. Since, more reactive metals oxidise easier, more reactive metals are stronger reducing agents than lesser reactive metals.

Oxide Layers
Al oxide layers can be anodized to make them thicker and hence better protect the metal. Anodizing involves the introduction of dyes, hence also colouring it.

Electric Cells (a.k.a. Galvanic cells)
An electric (or galvanic cell) comprises two electrodes (metals of different reactivities) immersed in an electrolyte containing free mobile ions (doesn’t matter what kind). Due to the differing reactivity (and hence ease of electron gain/loss) of the two electrodes, a potential difference is set up.

Examples of Galvanic Cells

 * Seriously, any mobile ions in solution will do for an electrolyte
 * Salt bridges (typically filter paper dipped in KNO3 or) maintain electrical neutrality that was previously caused by e- flow (ions of salt bridge flow to areas of charge imbalance)