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Metals
Physical Properties:
High melting and boiling points due to strong metallic bonds within a lattice structure.
Excellent conductors of heat and electricity because of free-moving delocalized electrons in
the metallic structure.
Malleability and Ductility: Metals can be bent or drawn into wires because metal layers can
slide over each other without breaking bonds.
Shiny (lustrous) appearance due to electron interaction with light.
Chemical Properties:
Formation of Positive Ions (Cations): Metals lose electrons easily, forming cations, due to
low ionization energy.
Oxidation: Metals react with oxygen to form metal oxides, which are mostly basic ,
meaning they neutralize acids to form salt and water.
Reactivity: Metals differ in reactivity, affecting their reactions with water, acids, and
oxygen, and the methods used for their extraction.
Reactivity Series
The reactivity series is an arrangement of metals in order of their reactivity, primarily with
water, acids, and oxygen. This reactivity series determines:
Whether metals will displace others in compounds.
The methods used to extract the metal from its ore.
Suitability for various practical applications (e.g., more reactive metals are not ideal for
construction as they corrode quickly).
Order of Reactivity (Most to Least):
Most Reactive: Potassium (K), Sodium (Na), Calcium (Ca)
Moderately Reactive: Magnesium (Mg), Aluminum (Al), Zinc (Zn), Iron (Fe)
Least Reactive: Copper (Cu), Silver (Ag), Gold (Au), Platinum (Pt)
A helpful way to remember it is this pneumonic
Please Send Cats , Monkeys And Zebras Into Hot Countries , Signed Gordon
Reactivity and Reactions with Water, Acids, and Oxygen: