Stoichiometry
4.
C 4.1
Stoichiometry
.
atoms
•
combine
Group
Types of chemical
Structural formula
a)
1
11
2
111
3
IV
4
V
3
V1
2
V11
1
VIII
0
formulae
how atoms
:
bonded
are
(displayed formula )
diagram
ethanol
:
GHGOH
Al2O3
Valency
I
full valence shells
→
fixed ratios
in
1.
Deducing formulae by combining power
AI
>
t
3
C
4
Alzsz
S
2
>
<
methane
Cttq
H
1
Deducing formulae of ionic compounds
A1
( simplified
b) written
"
soy
structural formula )
L
2-
2+
"
-
-
504
Cu
L
j
>
CHZCHZCHZCHZ
AlSO4
*
2
formula
Molecular
.
actual
:
#
of atoms
a
CuSO4
balance
Catto
Empirical
3.
formula :
simplest ratio
Cztls
Equations
Names
-
words
:
compounds
of
hydrogen
NM
+
NM
nitrogen
NM
+
+
→
→
sodium chloride
hydrogen
+
+
bromine
→
hydrogen
→
[ lower
Group
#
oxygen
→
•
•
NM ide
•
-
bromide
•
coz
"
NO
carbonate
Cacoz
sulfate
Mgsoq
=
hydroxide
NaOH
=
nitrate
BACNO , )z
=
5042
OH
-
-
Mgocs) +21-11403 ( ag)
→
Mg( NO , )zCaq)
+
H2O (e)
2 Kclcaq )
+
Iraq )
-
=
-
-
,
first ]
nitrogen oxide
Ahozcs) -13 Cuts)
groups
common
:
chlorine
hydrogen
-
2 Alcs) -13 Cuocs) →
m-etal-n-on-m-e.to/-M+NM-ide
sodium -1
-
balanced
+
balanced
equations
state symbols
equations
Ionic
2kt (
aa
) + Clzlaq ) →
21%+21 lag )
-
-
21 (aq )
+
+
Cklaq ) → KÑaq+2Cliaq ) Izcaa)
Cklaq ) →
+
-
2cL Caq )
+
Izlaq )
Ar
relative atomic mass
=
atoms
of
on
scale
where
mass
of
-
a
has
Mr
=
a
formula
# of
specific
6.02
unit
-
12
units
F
mass
1-12504
mass
=
)
covalent molecule
molecule
×
:
particles called
constant
10
"
where does it
-
atom
The mole
.
Avogadro 's
=
ñ
B
C
HCl
compound =/
ionic
C. 4.2
exactly
compound
covalent
"
Ars
relative
=
the
molecular
of
sum
-
(
a
At
occurring
element
an
relative
=
Mr
of naturally
average mass
-
particles
come
( atoms
,
molecules
,
formulae )
from ?
mol
Molar volume :
=
•
=
V
that
1 mole of
any gas will occupy
at
room
1-
24 dm
°
and
3
or
cr.t.is )
pressure
22.4
.
3
am
Calculate % composition
Mr 402)
=
% of 0
Ar ( O )
=
e.
g.
:
Concentration
c-
-
1. 2 d. m3
ng
in
CO2
12+32 =
16
44