(g) 80%1
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Ctb
Bunsen flame
created by : Emma Le
Exams
many graphics : Save
My
,C1 Particulate nature of matter
My
.
→ KE
-
states :
•
particle separation
? fixed ?)
arrangement ( regular
°
•
motion f
V, shape , f
atoms , compounds ions
-
,
H Mg 504 A-
Heating / cooling curve
•
melting points +
boiling points
are
unique to
pure substances
KINETIC THEORY
•
substance 1^1-0
= absorb thermal e. →
K
movement
→
structure ? motion ?
→ vibrates →
expands
→ structure breaks
KE >
intermolecular
forces
between 32
things
, DIFFUSION
-
states :
liquid # ,
random motion requires energy ?
-
*
-
[ h_ ] → [ -1 ]
until
evenly spread out
* make faster ?
-
relative molecular mass ( Mr )
•
faster in than
•
same to ,
different rates
→
Mr d → of
C2 .
Experimental techniques
C2 1
.
.
Measurements
unit equipment
liquids
2
-
time s stopwatch , stopcock
-
to 0C thermometer ( traditional /
digital )
mass
g. kg digital balance
-
'
volume ?m3 [ ]
accuracy
-
⇐
em
-
✗ precise :
variable V accurate :
3 fixed V
O -
50cm
⇒ minions -
10cm
}
3
-
25cm
gases
↳
, Criteria of
c. 2.2 .
purity
why do we need purity ?
only substance
•
one
pure
=
food additives not ? ?
in
drugs * what happens if impurities
•
,
how ?
↳
melting and
boiling point analysis * → data tables
g. pure water b.
e. :
p
:
I
.
M.p.
:
* if not exact values ?
•
mixtures melt / boil over a
range of to
*
why ?
ww
Paper chromatography
•
separate substances w/ different solubilities
(
in a solvent
•
solvent travels via
capillary action
>
dif rates
•
Retention factor ( Rf ) values
identify components of mixtures
→
-
compare Rf ( unknown) with Rf ( Known )
under same conditions
/ I.
7
ratio
/ )
units )
Rf = d moved
by compound ¥ ( no
d solvent
Cmf
" "
£1
?
highest / lowest solubility
-
-
pure / impure ?
'
vi.
¥÷÷ihemmiÉÉÉÉÉ÷%¥%÷
"
f-¥ .
II.
⑨ a
?¥ ¥0m
*
÷÷
" "
gÉN;¥¥÷¥÷
" lattice
structure
tetrahedron Coordinated Sciences
¥:}
⇒
*
.
if 0654
cttb ¥±
*
th ←
¥0s
Its
-
are,
Ctb
Bunsen flame
created by : Emma Le
Exams
many graphics : Save
My
,C1 Particulate nature of matter
My
.
→ KE
-
states :
•
particle separation
? fixed ?)
arrangement ( regular
°
•
motion f
V, shape , f
atoms , compounds ions
-
,
H Mg 504 A-
Heating / cooling curve
•
melting points +
boiling points
are
unique to
pure substances
KINETIC THEORY
•
substance 1^1-0
= absorb thermal e. →
K
movement
→
structure ? motion ?
→ vibrates →
expands
→ structure breaks
KE >
intermolecular
forces
between 32
things
, DIFFUSION
-
states :
liquid # ,
random motion requires energy ?
-
*
-
[ h_ ] → [ -1 ]
until
evenly spread out
* make faster ?
-
relative molecular mass ( Mr )
•
faster in than
•
same to ,
different rates
→
Mr d → of
C2 .
Experimental techniques
C2 1
.
.
Measurements
unit equipment
liquids
2
-
time s stopwatch , stopcock
-
to 0C thermometer ( traditional /
digital )
mass
g. kg digital balance
-
'
volume ?m3 [ ]
accuracy
-
⇐
em
-
✗ precise :
variable V accurate :
3 fixed V
O -
50cm
⇒ minions -
10cm
}
3
-
25cm
gases
↳
, Criteria of
c. 2.2 .
purity
why do we need purity ?
only substance
•
one
pure
=
food additives not ? ?
in
drugs * what happens if impurities
•
,
how ?
↳
melting and
boiling point analysis * → data tables
g. pure water b.
e. :
p
:
I
.
M.p.
:
* if not exact values ?
•
mixtures melt / boil over a
range of to
*
why ?
ww
Paper chromatography
•
separate substances w/ different solubilities
(
in a solvent
•
solvent travels via
capillary action
>
dif rates
•
Retention factor ( Rf ) values
identify components of mixtures
→
-
compare Rf ( unknown) with Rf ( Known )
under same conditions
/ I.
7
ratio
/ )
units )
Rf = d moved
by compound ¥ ( no
d solvent
Cmf
" "
£1
?
highest / lowest solubility
-
-
pure / impure ?
