IB Chemistry SL & HL Summary Notes

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