REDOX REACTIONS
OXIDATION:
Increase in Oxygen numbers
Reduce number of Hydrogens
Increase Oxidation numbers
Remove electrons
REDUCTION:
Decrease Oxygen numbers
Increase Hydrogen numbers
Decrease Oxidation numbers
Add electrons
ASSIGNING OXIDATION NUMBERS
Example:
O2, Na, S8, P4
2. Monoatomic ion oxydation number equal to its charge
Example:
F⁻' = - 1
3. Oxygen and Hydrogen's oxydation numbers are as follows:
O = -2
H = +1 (when it's paired with a non-metal)
H = -1 (when it's paired with a metal)
4. Sum of oxydation numbers:
Compound sum = 0
Polyatomic ion sum = charge of ion
Exercise:
Obtain the oxidation number of the bold element:
P₂O₅
2P + 5O = 0
2P + 5 x -2 = 0
2P -10 = 0
P = +5
Cr₂O₇⁻²
2Cr + 7O = -2
2Cr + (7 x -2) = -2
2Cr - 14 = -2
2Cr = 12
Cr = 6
DISPLACEMENT REACTIONS
(Single Replacement Reactions example of Redox reactions)
ACTIVITY SERIES
Exercise:
Write the products of the following reactions:
Zn + Pb(NO₃)₂ ----> Zn(NO₃)₂ + Pb
Zn > Pb on Activity series, therefore the reaction
occurs.
Cu + Pb(NO₃)₂ ----> NR
Cu > Pb on Activity series, therefore there’s no reaction
Exercise:
Write what compound gets oxidized and which compound get reduced in the following displacement reaction:
Al + 6HBr ----> H2 + AlBr3
Procedure:
No comments:
Post a Comment