Pre class Readings :
Ch1 , 1 4
.
+ Ch 2 , 2 5-2 6 .
.
14
.
Identifying formal Charges
Formal Charge associated w/ atom that does not exhibit the appropriate number of valence electrons .
any
:
↳If present in Lewis structure , formal Charge must be drawn
↳
determine appropriate # of valence electrons for an atom
determine if atom exhibits appropriate # of electrons
# of valence electrons determined
are
by group on periodic table
-
j:
soxygen has 7 total electrons Oxygen onlyneeds 6
:
so add
I
,
you a
H
4
-
-
H
H
.5
2
Identifying lone Pairs
To determine lone pairs on bond line drawings :
-
determine appropriate # of Valence electrons.
Oxygen -
-
determine if atom shows correct # of electrons
Oxygen atoms have negative formal charge extra electron
-
.
-
one
Bonds for
Oxygen atoms
H
j:
-
:
X Lo
I Bond + 3 lone pairs 2 bonds + 2 lone pairs 3 bonds + 1 lone pair
Key Idea Each atom : most make an octet ,
very electronegative atoms
rarely would be
missing an octet
2 6 Carbon atoms W/
.
formal Charges
-Carbon atoms 4 bonds doesn't have formal
generally have
only when it a charge .
-
When a Carbon atom has a positive or
negative charge -> it will have b bonds rather than 4
C -
Carbon is missing an electron ( ) +
t
Sa V +
&
no
hydrogen
atoms
one
hydrogenTwo hydrogen
atom atoms R
Sp hybridized Sp3 hybridized
C- Carbon has one extra electron () Empty Porbital lone pair in hybrid orbital
-
Will have I bonds and one love pair
S - T
N .
Onehydrogen
Two
no
hydrogen hydrogea
atoms atoms
, Friday Aug 19 Steric# = # of electron bonds
Ch1 .
See 1 7 , 1 10 1 12
.
,
. .
-1 = n -
Spr
Wave mechanics/quantum Mechanics Sp3 = 4 =
109 .
5
·
the nature of matter Spr 3 120
Changed how we view =
=
-
·
Wave equation : describes total energy of a
hydrogen atom Sp = 2 = 180
-
takes the wave like behavior of an electron that is in the electron field of a proton into account
4 : Wavefunction the ,
energy of the electron is quantized
Each Wavefunction is a function of Spatial location
-
X2 : indicates the
probability of finding the electron in that location
Orbital : of space that
region can be occupied by an electron
↳ atomic orbitals - S , P d f
, ,
M
.
t
Genode)
ancre To
Phase of the wave
-
N = > electron
0 -
density =
Aufbar Principle lowest Orbital is filled first
:
energy
Parli exclusion Principle: Each orbital can
occupy a max of 2 elections Wh opp spins - 1/1
Hund's rule : one orbital is placed in each before
pairing them up
2p
Tenergy
- - -
=2
1 10 .
hybrid atomic Orbitals
**
bonds
Carbon
excitement
energy
a bonds all bonds in compound single
-
a are
>
not affected
Ethylene
Hi
, c Sp ⑰ -
3 bonds not 4-sp2
hybridized JP2 carbon atom
off porbital
nord
soft bund
bond
Ch1 , 1 4
.
+ Ch 2 , 2 5-2 6 .
.
14
.
Identifying formal Charges
Formal Charge associated w/ atom that does not exhibit the appropriate number of valence electrons .
any
:
↳If present in Lewis structure , formal Charge must be drawn
↳
determine appropriate # of valence electrons for an atom
determine if atom exhibits appropriate # of electrons
# of valence electrons determined
are
by group on periodic table
-
j:
soxygen has 7 total electrons Oxygen onlyneeds 6
:
so add
I
,
you a
H
4
-
-
H
H
.5
2
Identifying lone Pairs
To determine lone pairs on bond line drawings :
-
determine appropriate # of Valence electrons.
Oxygen -
-
determine if atom shows correct # of electrons
Oxygen atoms have negative formal charge extra electron
-
.
-
one
Bonds for
Oxygen atoms
H
j:
-
:
X Lo
I Bond + 3 lone pairs 2 bonds + 2 lone pairs 3 bonds + 1 lone pair
Key Idea Each atom : most make an octet ,
very electronegative atoms
rarely would be
missing an octet
2 6 Carbon atoms W/
.
formal Charges
-Carbon atoms 4 bonds doesn't have formal
generally have
only when it a charge .
-
When a Carbon atom has a positive or
negative charge -> it will have b bonds rather than 4
C -
Carbon is missing an electron ( ) +
t
Sa V +
&
no
hydrogen
atoms
one
hydrogenTwo hydrogen
atom atoms R
Sp hybridized Sp3 hybridized
C- Carbon has one extra electron () Empty Porbital lone pair in hybrid orbital
-
Will have I bonds and one love pair
S - T
N .
Onehydrogen
Two
no
hydrogen hydrogea
atoms atoms
, Friday Aug 19 Steric# = # of electron bonds
Ch1 .
See 1 7 , 1 10 1 12
.
,
. .
-1 = n -
Spr
Wave mechanics/quantum Mechanics Sp3 = 4 =
109 .
5
·
the nature of matter Spr 3 120
Changed how we view =
=
-
·
Wave equation : describes total energy of a
hydrogen atom Sp = 2 = 180
-
takes the wave like behavior of an electron that is in the electron field of a proton into account
4 : Wavefunction the ,
energy of the electron is quantized
Each Wavefunction is a function of Spatial location
-
X2 : indicates the
probability of finding the electron in that location
Orbital : of space that
region can be occupied by an electron
↳ atomic orbitals - S , P d f
, ,
M
.
t
Genode)
ancre To
Phase of the wave
-
N = > electron
0 -
density =
Aufbar Principle lowest Orbital is filled first
:
energy
Parli exclusion Principle: Each orbital can
occupy a max of 2 elections Wh opp spins - 1/1
Hund's rule : one orbital is placed in each before
pairing them up
2p
Tenergy
- - -
=2
1 10 .
hybrid atomic Orbitals
**
bonds
Carbon
excitement
energy
a bonds all bonds in compound single
-
a are
>
not affected
Ethylene
Hi
, c Sp ⑰ -
3 bonds not 4-sp2
hybridized JP2 carbon atom
off porbital
nord
soft bund
bond
