CHEMISTRY
, Stoichiometry
Element
Nochfiabondabondsf.jo/7/7:. .F: /romi: simi ar/
:
one
type of atoms
Molecules : Atoms that are
chemically bonded ¥ompoumd
Compounds : Two or more
different types of atoms
e.
⑦ ••
••• •• ¥ to the
original to the
original
mixture mixture of
To"fYp%%b compound
compounds deterrents
particulate Nature
Three states of solid
:
> Liquid admiration
µi is
L ]
sublimation
so. - Gas
-
Deposition
TYPES OF MATTER HOMOGENEOUS -_ All components in
/ \ phase e.g saltwater
same
HETEROGENEOUS -_ components are in
pumrensnvbgtfnfff Mixture
different phases e.
g oil and water
Element Compound Homogeneous Heterogeneous
Physical change
→
No new substances made Creversibk)
Chemical
change
→
Atoms are
rearranged to form new substances
, PHASE CHANGES :
endothermic absorbs heat from the environment
exothermic releases heat into the environment
chemical
1. synthesis ( At B →
c)
changes
2. Decomposition ( breaking down )
3. 2kUt )
single replacement ( Clzt KBR → Bra
4 .
Double replacement (Cvs Out NA0H -4404/2 t
Naa 504
)
5. Combustion
( burning) must result H20
present
=
in
COMPOUND OF RULE
+
Lit Nat ,
Kt or NH4 Always soluble
,
02
-
soluble
Cz H3 Always
-
N03 ,
" 't
-
Pb
I
Agt Hgz
-
d- Br Insoluble with soluble with other ion
,
or
, ,
or
, any
't
5042 Bay Agt , Hgz
"
sr2t
-
soluble with all ions except ,
Pb
,
( 032 PO43 NH4Y
-
Lit kt ,
-
soluble with Nat insoluble with other ion
any
or or
,
.
,
52 CA4 5RY BAY hit
-
Kt,NHyt
-
OH or soluble with Nat, insoluble with other ion
any
-
.
,
Double
Replacement EXPERIMENT
CUCOIH)z
Cu sou t
NaOH → t Naz 504
Biuepercipitate countless solution
BLUE PERCIPITATE because of rule :
OH 52 with Catt
"
Batt Lit Nat kt Ntlyt insoluble
-
Sr
-
or soluble -
, , , , , ,
with other ion
any
.
COLOURLESS SOLUTION because of rule :
"
sr2t
Agt , Hgz
't
5042 soluble with all ions except Bast Pb
-
, or
, ,
, Stoichiometry DEFINITIONS
M0K The of the amount of substance , 6.02×1023 (avogadro 's constant ) of atoms
=
measure 1 mole =
ions or molecules .
Molar Mass atomic in periodic table
= The mass
(g) Of one mole of molecules → mass
given
Relative atomic mass =
The
weighted average mass of all the naturally occurring isotopes of an
element compared to the standard of carbon -12
The atomic masses the atomic in
Relative formula of the relative of species as
given
=
mass sum
the formula of an ionic
compound .
Compared to carbon -12
Avogadro constant → 6.02×1023, is the amount of particles in I mot of substance
ATOM ECONOMY →
looks at the level of efficiency of chemical reactions
by comparing the molecular mass of atoms
in the reactants with the molecular mass of useful compounds .
PERCENTAGE ATOM ECONOMY :
molewlarmassofatomsofusefulproducts-XIOO.li
molecular mass of atoms in reactants
The Mole
All chemical substances made
up of elements that composed of their constituent atoms Chemists to
equal amounts of
are are . use a
system measure
different elements
regardless of how
big their atoms are .
The mole is defined as a fixed amount ,
n
, of a substance .
Avogadro's constant
called and has 6. 02 × 1023 MOI
- "
This fixed amount is a number of particles Avogadro 's Constant it a value of
of particles
MY Calculations
number
Avogadrosconstant-Q.ee
amount in moi =
I
calculate the amount in mot ) of CO2 in Q: calculate the number of carbon atoms contained
a sample of 1. go × 1oz , molecules 1. gomo , g. µ , o
in of glucose ,
,
ncor-o.oIII.IT .IT?eIIbsooI5tt
more
↳ ↳
If :[Is
✓
'
emo , of
glucose contains :
6 0 atoms
So C
=
0.249 mot in 1.5 mots there is 9 mots of atoms
number of amount in Mol
atoms x
avogadro s constant
=
= 9 × 6.02×1023
=
5.42×1024 ( atoms
, Stoichiometry
Element
Nochfiabondabondsf.jo/7/7:. .F: /romi: simi ar/
:
one
type of atoms
Molecules : Atoms that are
chemically bonded ¥ompoumd
Compounds : Two or more
different types of atoms
e.
⑦ ••
••• •• ¥ to the
original to the
original
mixture mixture of
To"fYp%%b compound
compounds deterrents
particulate Nature
Three states of solid
:
> Liquid admiration
µi is
L ]
sublimation
so. - Gas
-
Deposition
TYPES OF MATTER HOMOGENEOUS -_ All components in
/ \ phase e.g saltwater
same
HETEROGENEOUS -_ components are in
pumrensnvbgtfnfff Mixture
different phases e.
g oil and water
Element Compound Homogeneous Heterogeneous
Physical change
→
No new substances made Creversibk)
Chemical
change
→
Atoms are
rearranged to form new substances
, PHASE CHANGES :
endothermic absorbs heat from the environment
exothermic releases heat into the environment
chemical
1. synthesis ( At B →
c)
changes
2. Decomposition ( breaking down )
3. 2kUt )
single replacement ( Clzt KBR → Bra
4 .
Double replacement (Cvs Out NA0H -4404/2 t
Naa 504
)
5. Combustion
( burning) must result H20
present
=
in
COMPOUND OF RULE
+
Lit Nat ,
Kt or NH4 Always soluble
,
02
-
soluble
Cz H3 Always
-
N03 ,
" 't
-
Pb
I
Agt Hgz
-
d- Br Insoluble with soluble with other ion
,
or
, ,
or
, any
't
5042 Bay Agt , Hgz
"
sr2t
-
soluble with all ions except ,
Pb
,
( 032 PO43 NH4Y
-
Lit kt ,
-
soluble with Nat insoluble with other ion
any
or or
,
.
,
52 CA4 5RY BAY hit
-
Kt,NHyt
-
OH or soluble with Nat, insoluble with other ion
any
-
.
,
Double
Replacement EXPERIMENT
CUCOIH)z
Cu sou t
NaOH → t Naz 504
Biuepercipitate countless solution
BLUE PERCIPITATE because of rule :
OH 52 with Catt
"
Batt Lit Nat kt Ntlyt insoluble
-
Sr
-
or soluble -
, , , , , ,
with other ion
any
.
COLOURLESS SOLUTION because of rule :
"
sr2t
Agt , Hgz
't
5042 soluble with all ions except Bast Pb
-
, or
, ,
, Stoichiometry DEFINITIONS
M0K The of the amount of substance , 6.02×1023 (avogadro 's constant ) of atoms
=
measure 1 mole =
ions or molecules .
Molar Mass atomic in periodic table
= The mass
(g) Of one mole of molecules → mass
given
Relative atomic mass =
The
weighted average mass of all the naturally occurring isotopes of an
element compared to the standard of carbon -12
The atomic masses the atomic in
Relative formula of the relative of species as
given
=
mass sum
the formula of an ionic
compound .
Compared to carbon -12
Avogadro constant → 6.02×1023, is the amount of particles in I mot of substance
ATOM ECONOMY →
looks at the level of efficiency of chemical reactions
by comparing the molecular mass of atoms
in the reactants with the molecular mass of useful compounds .
PERCENTAGE ATOM ECONOMY :
molewlarmassofatomsofusefulproducts-XIOO.li
molecular mass of atoms in reactants
The Mole
All chemical substances made
up of elements that composed of their constituent atoms Chemists to
equal amounts of
are are . use a
system measure
different elements
regardless of how
big their atoms are .
The mole is defined as a fixed amount ,
n
, of a substance .
Avogadro's constant
called and has 6. 02 × 1023 MOI
- "
This fixed amount is a number of particles Avogadro 's Constant it a value of
of particles
MY Calculations
number
Avogadrosconstant-Q.ee
amount in moi =
I
calculate the amount in mot ) of CO2 in Q: calculate the number of carbon atoms contained
a sample of 1. go × 1oz , molecules 1. gomo , g. µ , o
in of glucose ,
,
ncor-o.oIII.IT .IT?eIIbsooI5tt
more
↳ ↳
If :[Is
✓
'
emo , of
glucose contains :
6 0 atoms
So C
=
0.249 mot in 1.5 mots there is 9 mots of atoms
number of amount in Mol
atoms x
avogadro s constant
=
= 9 × 6.02×1023
=
5.42×1024 ( atoms
