Objective: To learn about metals and Reactivity
Chapter 4.06
The reactivity series of metals is a chart
listing metals in order of decreasing reactivity. In
general, the more reactive a metal is:
the more vigorously it reacts with other substances.
the more easily it loses electrons to form positive
ions (cations)
.
Parameters to judge reactivity of metals:
i)
ii)



The more readily a metal gives up electrons
to form ions, the more reactive it is.
A metal high up in the Reactivity series
 Reacts vigorously with other chemicals.
 Readily gives up electrons.
 Corrodes easily.
A metal low down in the Reactivity series
Does not react vigorously with other
chemicals.
Does not readily give up electrons.
Does not corrode easily.
Reactions of metals with oxygen

Reactions of iron with oxygen, water and
hydrochloric acid
Sample question/answers:
Q.1) a)Description of the chemical reaction of
iron with hydrochloric acid
A.1) a)The chloride formed
when iron reacts with hydrochloric
acid is iron (II) chloride, also known
as iron dichloride.
Word Equation:
Iron + Hydrochloric acid----------
Ironchloride + hydrogen
Q.1) b)Description of the chemical reaction of
iron with oxygen
A.1) a)The oxide formed when iron reacts
with oxygen is iron oxide which is a black
powder.
Word Equation:
Iron + oxygen---------- Iron oxide
Q.1) c)Description of the chemical reaction of
iron with water
A.1) c) In the absence of air, cold water doesn’t
react with iron. In the presence of air, however
iron reacts with water and produces ironoxide
and hydrogen.
Word Equation:
Iron + water---------- Iron oxide +
hydrogen