Covalent Bonding
Molecular Formula, heissen die
Verbindungen zwischen Geometries :
zwei nicht Metallen Die .
Verbingungen zwischen einem bent (104 . 59 :
linear (1800 :
trigonal planar (120%
CT
-d -
Metall und nicht Metall Empirical o o
0
heisst
;
For mula
HH c
=
=
,
=
.
Non-Metals
form bonds to archieve Noble gas
configuration
->
2/p + 2 bonds -I bonds , Olp ->
3bonds , Olp
trigonal pyramidal (107 . 89) tetrahedal
5
%:
by "sharing"
:
an electron The shared electrons are concentraded (109 .
.
FE
in the
region between the two nuclei, which attractes them
#N -
-F
stabilizes 3bonds 1Ip bonds
formation hydrogen the -> 4
->
The the
of molecule atoms, ,
so is released as the bond is formed The bond
energy .
the between the two Lewis Structure Skeletal Formula
length distance
:
is a measure of
:
bonded nuclei where the
energy is at its minimum The
·
unpaired electrous F -
IEI
-
.
H
Na
-
described
bond
streugh is
usually in terms
of bond
energy
lone
pairs Na -
stablette
4t
?
-
and is measure
of the required to break bond if have an ion 02 - -
energy
a a you
."
xe" Ye
or the
energy
that is released when a bond is
formed .
(KI/mol -
lone pairs are not drawn
it
E
for H-H bond is
435KJ/mol that is released
during the
the
formation of Imol of He bonds . Polarized Covalent bonds :
bigger the equal
the
bigger the bond
length electrous shared attracts
radius the the not electron the other more
-> atomic are
mostly ba One
:
.
polarized diffrent negativity =0 .
5
two
higher the
ers the bonds between with electron
difference
:
The sand wore atoms an
non-polar bond same atom, electrons shared
·
equal
:
+St
S
the
higher
the intermolecular force (IMF) ,
the
higher the AEN :
The diffrence of
the EN , beschriften
St
boiling point the
higher the core
charge, the
higher
- nur oder eine polarize Verbindung hat
-
.
wenn es
Ipolar
!
attraction the
%
the EN . the more shells atoms have ,
VIT
#
st
st St
London ! X + st
-
the lower the E N More .
Atoms, higher force 8&g
+
ST
d
Molecules DD-Force
Dipole
:
:
-> a molecule is
dipole when the centre of positive charge and centre of negative charge
are ->
dipole molecules attract each other (from one and o
from
-
/ . .
not place the other
on the same .
Draw an arrow
from positive
to
negative . molecule
->
O-
1I
N +13 EN; H
=
.
2
1
E
-
N 1 / .. EN 0
. London
N
force
= :
8 Hg+ ;
- . 3
I
/ ↑⑪# -
H
St · with all molecules
St
short moment
AEN=0 .
9
only
->
for a
very very
Electrons are
always
in motion ,
so they can be found near one atom
for a short
Ethanol CzHG moment This partial and the other
partial positiv
:
atom gets
.
negative charge
Lewis Structure 3D structure skeletal
charge
: :
formula
:
H2
St
H H ·
HOH
H-
*
-
H
↑
I
C
/
-
c
-
C
I
pr
C
-> the
larger the contact area between the molecules, the Stronger the London
higher
↳
so
needs
we
4
have
bonds ,
3 C-H
force -
boiling point
bonds
- "Standart", where
if 3D is important, for
I
n ↑
&
biomolecules
111 mallenta
all
you
can see bonds
Example in a
fasteasy -
IIIIII
like
enzymes large
eine XX
Contact
area
only tetrahedal
- or
trigonal pyramidal
Molecular Formula, heissen die
Verbindungen zwischen Geometries :
zwei nicht Metallen Die .
Verbingungen zwischen einem bent (104 . 59 :
linear (1800 :
trigonal planar (120%
CT
-d -
Metall und nicht Metall Empirical o o
0
heisst
;
For mula
HH c
=
=
,
=
.
Non-Metals
form bonds to archieve Noble gas
configuration
->
2/p + 2 bonds -I bonds , Olp ->
3bonds , Olp
trigonal pyramidal (107 . 89) tetrahedal
5
%:
by "sharing"
:
an electron The shared electrons are concentraded (109 .
.
FE
in the
region between the two nuclei, which attractes them
#N -
-F
stabilizes 3bonds 1Ip bonds
formation hydrogen the -> 4
->
The the
of molecule atoms, ,
so is released as the bond is formed The bond
energy .
the between the two Lewis Structure Skeletal Formula
length distance
:
is a measure of
:
bonded nuclei where the
energy is at its minimum The
·
unpaired electrous F -
IEI
-
.
H
Na
-
described
bond
streugh is
usually in terms
of bond
energy
lone
pairs Na -
stablette
4t
?
-
and is measure
of the required to break bond if have an ion 02 - -
energy
a a you
."
xe" Ye
or the
energy
that is released when a bond is
formed .
(KI/mol -
lone pairs are not drawn
it
E
for H-H bond is
435KJ/mol that is released
during the
the
formation of Imol of He bonds . Polarized Covalent bonds :
bigger the equal
the
bigger the bond
length electrous shared attracts
radius the the not electron the other more
-> atomic are
mostly ba One
:
.
polarized diffrent negativity =0 .
5
two
higher the
ers the bonds between with electron
difference
:
The sand wore atoms an
non-polar bond same atom, electrons shared
·
equal
:
+St
S
the
higher
the intermolecular force (IMF) ,
the
higher the AEN :
The diffrence of
the EN , beschriften
St
boiling point the
higher the core
charge, the
higher
- nur oder eine polarize Verbindung hat
-
.
wenn es
Ipolar
!
attraction the
%
the EN . the more shells atoms have ,
VIT
#
st
st St
London ! X + st
-
the lower the E N More .
Atoms, higher force 8&g
+
ST
d
Molecules DD-Force
Dipole
:
:
-> a molecule is
dipole when the centre of positive charge and centre of negative charge
are ->
dipole molecules attract each other (from one and o
from
-
/ . .
not place the other
on the same .
Draw an arrow
from positive
to
negative . molecule
->
O-
1I
N +13 EN; H
=
.
2
1
E
-
N 1 / .. EN 0
. London
N
force
= :
8 Hg+ ;
- . 3
I
/ ↑⑪# -
H
St · with all molecules
St
short moment
AEN=0 .
9
only
->
for a
very very
Electrons are
always
in motion ,
so they can be found near one atom
for a short
Ethanol CzHG moment This partial and the other
partial positiv
:
atom gets
.
negative charge
Lewis Structure 3D structure skeletal
charge
: :
formula
:
H2
St
H H ·
HOH
H-
*
-
H
↑
I
C
/
-
c
-
C
I
pr
C
-> the
larger the contact area between the molecules, the Stronger the London
higher
↳
so
needs
we
4
have
bonds ,
3 C-H
force -
boiling point
bonds
- "Standart", where
if 3D is important, for
I
n ↑
&
biomolecules
111 mallenta
all
you
can see bonds
Example in a
fasteasy -
IIIIII
like
enzymes large
eine XX
Contact
area
only tetrahedal
- or
trigonal pyramidal
