Metallic Elements and Alloys

1. Metallic Elements and Alloys
• Metals are the elements on the left side of the periodic table and non-metals are
those on the right side of the periodic table.
The physical properties differences between metals and non-metals

2. The chemical properties differences between metals and non-metals
A. Properties Of Metal
 Conduct heat and electricity
 Are malleable (can be hammered and made into different
shapes) and ductile (can be drawn into wires)
 Tend to be lustrous (shiny)
 Have high density and usually have high melting points
 Form positive ions through electron loss
 Form basic oxides

3.  General chemical properties of metals
• The chemistry of metals is studied by analysing their reactions with water, dilute acid and oxygen
• Based on these reactions, a reactivity series of metals can be produce
 Reactivity with water
• Some metals react with water, either warm or cold, or with steam
• Metals that react with cold water form a metal hydroxide and hydrogen gas
• metal + water → metal hydroxide + hydrogen
Ca (s) + 2H2O (l) → Ca(OH)2 (aq) + H2 (g)
• Metals that react with steam form metal oxide and hydrogen gas
Zn (s) + H2O (g) → ZnO (s) + H2 (g)
 Reactivity with acids
• Most metals react with dilute acids such as HCl
• When acids and metals react, the hydrogen atom in the acid is replaced by the metal atom to produce a
salt and hydrogen gas, for example iron:
• metal + acid → salt + hydrogen
• Fe (s) + 2HCl (aq) → FeCl2 (aq) + H2 (g)
• Cu (s) + 2HCl (aq) → CuCl2 (aq) + H2 (g)
 Reactivity with oxygen
• Unreactive metals such as gold and platinum do not react with oxygen
• Some reactive metals such as the alkali metals react easily with oxygen
• Copper and iron can also react with oxygen although much more slowly
• When metals react with oxygen a metal oxide is formed, for example copper:
• metal + oxygen → metal oxide
• 2Cu (s) + O2 (g) → 2CuO (s)
• 2Mg (s) + O2 (g)  2MgO (s)

4. • Alloys : mixture of elements (usually metals) designed to have the
properties useful for a particular purpose.
• Alloys often have properties that can be very different from the metals
they contain, for example, they can have more strength (stronger),
hardness or resistance to corrosion or extreme temperatures
• These enhanced properties can make alloys more useful than pure metals
*Common alloys and their uses*
a. Brass is an alloy of copper and zinc , this alloy is hard and is
much stronger than either metal. It is used in musical instruments,
ornaments and door knobs.
b. Stainless steel is hard alloy created specifically to resist corrosion.
a mixture of iron and other elements, for example, chromium, nickel and
carbon.
• Alloys of iron with tungsten are extremely hard and resistant to
high temperatures
• Alloys of iron mixed with chromium or nickel are resistant to corrosion
• Aluminium is mixed with copper, manganese and silicon for aircraft body
production as the alloy is stronger but still has a low density

5. Uses Of Metal
a. Uses of Iron (Fe)
- moderately reactive transition metal
- hardness, strong and malleable
- conduct heat well and magnetic
Use : bridges, construction girders, boat, rail,ships, building
b. Uses Aluminium (Al)
- light, strong metal, good electrical conductivity
- low density, resistant to corrosion, reactive metal
- Aluminium adding manganese and copper = “duralumin” is formed
Use: food packaging, construction : aircraft and high voltage power cable (pylons)
c. Uses Copper
- least reactive metal, very high electrical conductivity, very ductile
- strong but easily bent to shape
Use : water pipes, roofing for building,electrical wiring and cable

6. Solid state  same shape, same volume, can’t compressed, the particle
strongly, fixed shape. E.g : metal
Structure of Metal and Alloy
Ionic atom  charge of cation and anion
A mixture of metal crystals
An Alloy  is not mixture of metal crystal regions but a regular lattice of atoms