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Organic
Module 2
Redox
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The change in oxidation number identifies whether or not a substance has undergone
oxidation
or
reduction
Roman numerals
are used to indicate the oxidation number of
metals
that may have different oxidation states in compounds
Rules for Oxidation Numbers:
all
elements
in their
natural
state
have the oxidation number of
0
oxidation numbers in a compound add up to
0
oxidation numbers of the components in an ion add up to the
charge
on that ion
Order of Priority:
elements
in
group
1,
2
, &
3
, respectively
fluorine
is
-1
hydrogen
is usually
+1
oxygen
is usually
-2
chlorine
is usually
-1
ions with names ending in -ate contain
oxygen
What is the formula for carbon monoxide?
CO
What is the formula for methane?
CH4
What is the formula for nitrogen monoxide?
NO
What is the formula for nitrogen dioxide?
NO2
What is the formula for sulfuric acid?
H2SO4
What is the formula for ammonia?
NH3
What is the formula for nitrogen?
N2
What is the formula for oxygen?
O2
What is the formula for phosphorus?
P4
What is the formula for hydrogen?
H2
All of group 7 elements are
diatomic
molecules
What is the formula for an ammonium ion?
NH4+
What is the formula for a carbonate ion?
C
O
3
2
−
CO3^2-
CO
3
2
−
Define Redox:
A
reaction
where
both
oxidation
and
reduction
take
place
as
one
element
is
oxidised
,
donating
its
electrons
to
the
other
element
that
is
reduced
The oxidising agent becomes
reduced
because it
gains
electrons,
decreasing
its oxidation number
The reducing agent becomes
oxidised
because it
loses
electrons,
increasing
its oxidation number
Give the equation for the oxidising agent:
x
+
x^+
x
+
+
+
+
e
−
−
>
x
e^- -> x
e
−
−
>
x
Give the equation for the reducing agent:
x
−
>
x
+
x -> x^+
x
−
>
x
+
+
+
+
e
−
e^-
e
−
Define Disproportionation:
a
reaction
in
which
the
same
element
is
both
reduced
and
oxidised
NH3 is an
alkaline
gas
The formula for ammonium nitrate:
NH4NO3
Burning a substance means
adding oxygen
to it
Formula for hydrogen carbonate:
HCO3-
Formula for Phosphoric Acid:
H3PO4
Formula for Phosphate ion:
P
O
4
3
−
PO4^3-
PO
4
3
−
The empirical and molecular formula can be the
same
Percentages in empirical formula calculations all add up to
100
%
Using PV=nRT involving density:
g
m
3
gm^3
g
m
3
use v=
1
m
3
m^3
m
3
g
d
m
3
gdm^3
g
d
m
3
use v=
1 x 10^-3
m
3
m^3
m
3
g
c
m
3
gcm^3
g
c
m
3
use v=
1 x 10^-6
m
3
m^3
m
3
Define a Monoprotic Acid:
an acid that donates only one proton
(
H+
)
There's a
1
:
1
ratio;
acid
to
base
Define a Diprotic Acid:
an acid that donates two protons
(
H+
)
There's a
1
:
2
ratio,
acid
to
base
Define a Triprotic Acid:
an acid that donates 3 protons
(
H+
)
There's a
1
:
3
ratio,
acid
to
base
Give three examples of a monoprotic acid:
HCl
HNO3
CH3COOH
Give three examples of a diprotic acid:
H2SO4
H2CO3
H2S
Give an example of a triprotic acid:
H3PO4
What kind of reagent is this equation for:
x
−
>
x
+
x -> x^+
x
−
>
x
+
+
+
+
e
−
e^-
e
−
reducing
What kind of reagent is this equation for:
x
+
x^+
x
+
+
+
+
e
−
−
>
x
e^- -> x
e
−
−
>
x
oxidising
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