topic I 0 I 2 0
HOMOLOGOUS SERIES ACID-BASE PROPERTIES .
don't have avid
☆ most
functional groups -
base properties
pounds with same
general formula
-
um
lath member Ctlz
☆ exceptions
differs by
-
similar chemical 4 Alkanoicaiids weak acids HCOOH HCOO Ht
-
-
-7 +
properties
=
trend in
physical properties at}NH , lHzNHzᵗ
-
-
4 Amines = weak bases + Her -7 + OH
SOLUBILITY BOILING PANTS eat only
only London DF
•
depends on
polarity 1- chain
length •
breaking intr not intramolecular
force
polar ≠ dissolve ( alkane / alkene) c- chain
longer higher
•
non -
•
-
-
all functional
groups except alkyls polar London
•
are
stronger for bigger molecules
•
decreases the ( cuz that part is nonpolar)
•
Solubility longer the c- chain ◦
LDF < dipole dipole < H bond
-
-
•
branched -
_ lower ( spherical sobsscohtaltw/ other molecules = lasaltraited )
ALKANES undergo free-radical substitution reactions
low Free radical substitution
reactivity
•
Non-polar •
light
UV
alkanet
4 C-C & C-H bonds are
strong (unreactive ) halogen →
halogensalkanet HCI
low polarity ( C- C--0 ) ( C- H= ) Ayat lb ,
↳ 0.4 neutral Utsa g) +
Haig)
4
only react in persona of strong source
of energy
↑
→ stable undermost conditions A- g- At a- a H a H G
-
H !
,
hydrogen"
be stored, "
→ can
transported compressed safely
+
chiorowetnane
""
l details next page )
•
Unbutton
↳
comptdt exothermic 1021-11-20 =
greenhouse gases
Cltytllz -7 fEtLHz0 \ CO poisonous gas
CONSEQUENCES →
=
4in¥te
9+4+-31-7 +2¥ , released
unburned Clsoot)= as
particulates
☆ same # of water but less Ozvsed
negative health effect on
respiratory system
catalysts informing smog
, D INITIATION
.ci?-F.i.:-:&i..t:&i
w
Ck → a. + crime
I
Radia's
elective unpaired
① : .
UV light has to be present µnÑ""H
µ
µ I
+ H C/ -
homolytic same# étoemhatom after bond breaks
② [¥ (/ → H C .
fission
• -
-
+
µ _
1
of Cl Cl-
,
bond
µ H
② PROPAGATION radical used + formed veryreoutivespaiesinmixtvre-heepsreoution-g.org It H
I I ¢ 9
.
→H at
CH , -7 CH } HCl Cltgatck Cltzaztcl
. -
+
•
→ µ
-
+ . -
.
I
H
H
Cltjtllz 011-3011-4 cttcltzcl -204201 HCl
.
-7 . t
Band fluorocarbon
③
art CT →
92
③ TERMINATION two radicals combine used the terminates reaction H
species
F
+ up removes +
a. to
-
→ Ck
H - dirt % →
A- c-
'
a
1 It
H
Choi 1- a. → CAN
( Hoitllti -7 CzH6(ethane ) H H
*
'
↑
A- dont
a. d- H → A- c- C- µ
I 1
1 It It It
H
ALCOHOLS OXIDATION
•
combustion -
complete oxidation
•
Redox
241-3011-(111-30219) -7202 (g) +44201g) 04% -726.16J.moH Context Oxidation Reduction
-
gainoftxygen Loss of oxygen
2414101+41+1502191-7106021g) +12420cg, 011-4=-913331.mil =
Oxygen
More exothermic bond
forming release Hydrogen loss of hydrogen gain of
hydrogen
more
energy
-
_
* loss of electrons electrons
gain
also lands
incomplete combustion Electrons
Alcohols
•
Primary
"
""'
"" °
loss of
"
gain
't •
Distillation vs Reflux
%
µ µ H
1
"°
Ct
I [07 heat I
A- C- C- OH
+
+101 heat I " "
" "" "A REFLUX
µ c-_
C H H y¥¥g µ
H µ
1+1!
'
OH
.
'
oxidizing 1 reflux 1 1 I 1-101 ,heat ° I °
+101, heat "
art * H
ethanoicaoid A- C- C- OH -7 A- d- H C -
c
ethanol ethanol
¥×
-
\, '
l 1 OH
ALDEHYDE I ,
ALCOHOL CARBOXYLIC ACID
µ H
µ µ
+ [ 0 ]=H7Crµ ) acidified dichromate crzo -2
,
BP 78% 20°C VINEGAR
cold wine / not closed properly )
WINE
4 allows reaction to happen / changes from orange > green)
sinaitbaomescr.TT! )
refwxywbe.int "
¥¥Y%y
aldehyde does
not evaporate
Sllsndary Alcohol aksholgas gets
•
array
and tandems mown,
cold
→ oxidized to ketone
It wine
µ
¥ It it
'
[D. heat
d- Ht H2O
+
A- c- c- c- It A- c- c-
→
1 I Mtm 1 U I
I
OHH It 0 it
µ
propanone orange green
propan -2-01 HYCRIVI ) -7 CHI)
HOMOLOGOUS SERIES ACID-BASE PROPERTIES .
don't have avid
☆ most
functional groups -
base properties
pounds with same
general formula
-
um
lath member Ctlz
☆ exceptions
differs by
-
similar chemical 4 Alkanoicaiids weak acids HCOOH HCOO Ht
-
-
-7 +
properties
=
trend in
physical properties at}NH , lHzNHzᵗ
-
-
4 Amines = weak bases + Her -7 + OH
SOLUBILITY BOILING PANTS eat only
only London DF
•
depends on
polarity 1- chain
length •
breaking intr not intramolecular
force
polar ≠ dissolve ( alkane / alkene) c- chain
longer higher
•
non -
•
-
-
all functional
groups except alkyls polar London
•
are
stronger for bigger molecules
•
decreases the ( cuz that part is nonpolar)
•
Solubility longer the c- chain ◦
LDF < dipole dipole < H bond
-
-
•
branched -
_ lower ( spherical sobsscohtaltw/ other molecules = lasaltraited )
ALKANES undergo free-radical substitution reactions
low Free radical substitution
reactivity
•
Non-polar •
light
UV
alkanet
4 C-C & C-H bonds are
strong (unreactive ) halogen →
halogensalkanet HCI
low polarity ( C- C--0 ) ( C- H= ) Ayat lb ,
↳ 0.4 neutral Utsa g) +
Haig)
4
only react in persona of strong source
of energy
↑
→ stable undermost conditions A- g- At a- a H a H G
-
H !
,
hydrogen"
be stored, "
→ can
transported compressed safely
+
chiorowetnane
""
l details next page )
•
Unbutton
↳
comptdt exothermic 1021-11-20 =
greenhouse gases
Cltytllz -7 fEtLHz0 \ CO poisonous gas
CONSEQUENCES →
=
4in¥te
9+4+-31-7 +2¥ , released
unburned Clsoot)= as
particulates
☆ same # of water but less Ozvsed
negative health effect on
respiratory system
catalysts informing smog
, D INITIATION
.ci?-F.i.:-:&i..t:&i
w
Ck → a. + crime
I
Radia's
elective unpaired
① : .
UV light has to be present µnÑ""H
µ
µ I
+ H C/ -
homolytic same# étoemhatom after bond breaks
② [¥ (/ → H C .
fission
• -
-
+
µ _
1
of Cl Cl-
,
bond
µ H
② PROPAGATION radical used + formed veryreoutivespaiesinmixtvre-heepsreoution-g.org It H
I I ¢ 9
.
→H at
CH , -7 CH } HCl Cltgatck Cltzaztcl
. -
+
•
→ µ
-
+ . -
.
I
H
H
Cltjtllz 011-3011-4 cttcltzcl -204201 HCl
.
-7 . t
Band fluorocarbon
③
art CT →
92
③ TERMINATION two radicals combine used the terminates reaction H
species
F
+ up removes +
a. to
-
→ Ck
H - dirt % →
A- c-
'
a
1 It
H
Choi 1- a. → CAN
( Hoitllti -7 CzH6(ethane ) H H
*
'
↑
A- dont
a. d- H → A- c- C- µ
I 1
1 It It It
H
ALCOHOLS OXIDATION
•
combustion -
complete oxidation
•
Redox
241-3011-(111-30219) -7202 (g) +44201g) 04% -726.16J.moH Context Oxidation Reduction
-
gainoftxygen Loss of oxygen
2414101+41+1502191-7106021g) +12420cg, 011-4=-913331.mil =
Oxygen
More exothermic bond
forming release Hydrogen loss of hydrogen gain of
hydrogen
more
energy
-
_
* loss of electrons electrons
gain
also lands
incomplete combustion Electrons
Alcohols
•
Primary
"
""'
"" °
loss of
"
gain
't •
Distillation vs Reflux
%
µ µ H
1
"°
Ct
I [07 heat I
A- C- C- OH
+
+101 heat I " "
" "" "A REFLUX
µ c-_
C H H y¥¥g µ
H µ
1+1!
'
OH
.
'
oxidizing 1 reflux 1 1 I 1-101 ,heat ° I °
+101, heat "
art * H
ethanoicaoid A- C- C- OH -7 A- d- H C -
c
ethanol ethanol
¥×
-
\, '
l 1 OH
ALDEHYDE I ,
ALCOHOL CARBOXYLIC ACID
µ H
µ µ
+ [ 0 ]=H7Crµ ) acidified dichromate crzo -2
,
BP 78% 20°C VINEGAR
cold wine / not closed properly )
WINE
4 allows reaction to happen / changes from orange > green)
sinaitbaomescr.TT! )
refwxywbe.int "
¥¥Y%y
aldehyde does
not evaporate
Sllsndary Alcohol aksholgas gets
•
array
and tandems mown,
cold
→ oxidized to ketone
It wine
µ
¥ It it
'
[D. heat
d- Ht H2O
+
A- c- c- c- It A- c- c-
→
1 I Mtm 1 U I
I
OHH It 0 it
µ
propanone orange green
propan -2-01 HYCRIVI ) -7 CHI)
