BAB 2 Orbital dan perannya pada Ikatan Kovalen FROM LEWIS DIAGRAMS TO MOLECULAR SHAPE VSEPR THEORY.
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Transcript of BAB 2 Orbital dan perannya pada Ikatan Kovalen FROM LEWIS DIAGRAMS TO MOLECULAR SHAPE VSEPR THEORY.
![Page 1: BAB 2 Orbital dan perannya pada Ikatan Kovalen FROM LEWIS DIAGRAMS TO MOLECULAR SHAPE VSEPR THEORY.](https://reader038.fdocuments.us/reader038/viewer/2022110320/56649ca35503460f94963a70/html5/thumbnails/1.jpg)
BAB 2BAB 2
Orbital dan perannya pada Ikatan Kovalen
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FROM LEWIS DIAGRAMS TO MOLECULAR SHAPE
VSEPR THEORYVSEPR THEORY
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H. H.
H. H.
H H
IKATAN KOVALENIKATAN KOVALEN
Tumpang tindih orbital
Pembentukan Ikatan
Atom yang terpisah
atomsmovecloser
( Model tumpang tindih orbital)
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QUESTIONQUESTION
…….. LET’S TRY IT FOR H.. LET’S TRY IT FOR H22OO
Can we predict the shapes of molecules simply bycombining the atomic orbitals available on each atom?
H O
H
:..
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O
y
x
z
..2s
.
2p
.2p
oxygen = [He]2s22p4
OXYGENOXYGENORBITALSORBITALS
[ cartoon ]
2p Orbital saling tegak lurus (90o)
2p22p12p1
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O
y
x
z
.
... ..
2s
2p
2p
2p
OXYGENOXYGENORBITALSORBITALS
oxygen = [He]2s22p4
unpaired
unpaired
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O
y
x
z
H. .
.
H.
.. ..
Combining atomicorbitals to form H2O.
Incorrectlypredicts a90o angle.
2s
2p
2p
2p
1s
1s
oxygen = [He]2s22p4
hydrogen = 1s1
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H
H
O
105o
The actual H-O-H anglein water (measured byelectron diffraction) is 105o
EXPERIMENTAL RESULTEXPERIMENTAL RESULT
This is not very good agreement with the atomic orbital model!
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VSEPRVSEPR TheoryTheoryValenceShellElectronPairRepulsionBased on the simple idea that
groups of electrons repel each otherPredicts molecular shapes quite
well
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A better result is predicted by VSEPR theory
consider the completedvalence shell to be aspherical volume aroundthe nucleus
try to minimize repulsionsby maximizing the distancebetween all pairs ofelectrons
electron pairs (4 pair)repel each other
in the final solution, theyshould all be equidistant
valenceshell
nucleus
TETRAHEDRAL
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Basic Shapes of MoleculesBasic Shapes of Molecules
A B A
A
BA A
B A
A
Aor
A
BAA
A
B A
A
AA
A
A
B
AA A
A A
LINEAR
TRIGONAL PLANAR
TETRAHEDRAL
TRIGONAL BIPYRAMID OCTAHEDRAL
Bond angle = 180°
Bond Angles = 120°
Bond angles = 109° 28'
Bond angles = 120°, 90° Bond angles = 90°
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VALENCE SHELL ELECTRON PAIR REPULSION
VSEPR THEORY
4 pair tetrahedral 109o28’ sp3 (pyrimidal, angular )
3 pair trigonal planar 120o sp2
2 pair linear 180o sp
pairs geometry angles hybridization
For most molecules, these predictions are correct to within a few degrees (5o).
6 pair octahedral 90o d2sp3
5 pair trigonal bipyramid 120o, 90o dsp3
ORGAN IC
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OrbitalsOrbitals
The region of space around an atom in which an electron is likely to be found is an orbital.
The shape and size of the orbital are determined by a mathematical equation called a wave function.
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OrbitalsOrbitals
When atoms combine to form molecules, they do so by combining the wave functions for the individual atomic orbitals.
We say that the orbitals “overlap.”The region of space defined by this
combination of orbitals is the molecular orbital.
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Sigma BondsSigma BondsHead-on overlap of atomic
orbitalsElectron density is a symmetrical
cylinder around the bond axis
Atomic orbital combinations that give bonds:s s p p ps
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Pi BondsPi BondsSide-on overlap of atomic orbitalsElectron density is above and below a
nodal plane on the internuclear axis
Atomic orbital combinations that give bonds:
p p p d
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HYBRIDIZATIONHYBRIDIZATION
HOW ARE THE OBSERVED BOND ANGLES ACHIEVED?
“Vision is the art of seeing things invisible.”
Jonathan Swift
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atomicorbitals
hybrid atomic orbitals
molecular orbitals
HYPOTHETICAL BONDING PROCESS
2s2px,2py,2pz
sp,sp2py,2pz , , ,n
These orbitals are for the atom - we can’t expect that they are suitable for the molecule.
WHY DOESN’T THE ATOMIC ORBITAL APPROACH WORK ?WHY DOESN’T THE ATOMIC ORBITAL APPROACH WORK ?
During bonding ….new orbitals form thatare more suitable for making bonds.
After bonding (overlap)we get a totallynew solution for thenew molecule.
overlap
NOTE. Formally LCAO theory and Molecular Orbital theory are two completely different approaches. You do not need to use hybid orbitals to derive the molecular orbitals, combinations of any type of function will do. Nevertheless, the abstraction presented above is quite useful, as we will see quite soon.
LCAO
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O
tetrahedral geometry
2s
2p
sp3 hybrid orbitals
hybridization
109o28’
(cartoon)
FORMATION OF TETRAHEDRAL HYBRID ORBITALSFORMATION OF TETRAHEDRAL HYBRID ORBITALS
4 pair
sp3(1)
(1) (2) (3) (4)
sp3(3)
sp3(4)sp3(2)
New orbitals pointto the corners of atetrahedron.
FILLED VALENCESHELL
occurs when orbitalsare full and have finished bonding
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X
unhybridized atom
2s
2pz
2py
2px
2s
2p
FORMATION OFFORMATION OFSPSP33 HYBRID ORBITALS HYBRID ORBITALS
X
sp3 hybridized atom
(1) (2) (3) (4)
FORMATION OFFORMATION OFSPSP33 HYBRID ORBITALS HYBRID ORBITALS
These orbital shapes arecartoons - actual shapesare shown on the nextslide. [animation]
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sp3
SPSP33 HYBRID ORBITAL HYBRID ORBITAL
The hybrid orbitalhas more density in the bonding lobethan a p orbital andforms stronger bonds.
( cross section )
The shape shown is calculated fromquantum theory.To avoid confusion the
back lobe is omitted from the cartoons, already shown, and thefront lobe is elongatedto show its direction. omitted
Courtesy ofProfessor George Gerhold
… and its cartoon
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2s 2p
add together, divide in four
sp3 hybrid orbitals(1) (2) (3) (4)
each new orbital is1/4 s + 3/4 p (25% s, 75% p)
S1P3 = SP3
( 1+3 ) = 4 parts total
ORIGIN OF THE SPORIGIN OF THE SP33 DESIGNATION DESIGNATION
hybridization
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+
+
-
2s orbital
2p orbital
x
HYBRIDIZATION
x +-
sp3 hybrid orbital
HYBRIDIZATION
signs are mathematicalcoordinates, not electronic charge
RECALL:
ORIGIN OF THE SPORIGIN OF THE SP33 ORBITAL SHAPE ORBITAL SHAPE
[animation]
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Ikatan padaIkatan pada
Alkana sp3
Alkena sp2
Alkuna sp
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C
Carbon has 4 valence electrons, 2s22p2
.. ..
Carbon can form single, double or triple bonds
sp, sp2 and sp3 hybrid orbitals.
Let’s do sp3 first.
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2p
2s
hybridize sp3
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H
H
H
H
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CC H
H
HH
H
H
C C
H HH
H H
H
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Multiple Bonds and hybridization
Ethylene C CH
H
H
H
Each carbon is hybridized sp2 . The hydrogens are 1s. One of the double bonds is sp2 - sp2. The other one isp - p.
2p
2s
hybridize
2p
sp2
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C C
Note that a double bond consists of a and a type bond
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C C
H
H
H
H
C C
H
H
H
H
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What about acetylene?
C CH HEach carbon atom is sp hybridized. The hydrogens areunhybridized, 1s orbitals.
2p
2s
hybridize
2p
sp
Note that a triple bond consists of a and 2 bonds. Thetwo bonds use unhybridized p orbitals.
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CCH H
C C HH
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COMPARISON OF SPCOMPARISON OF SPxx HYBRID ORBITALS HYBRID ORBITALS
more “p” character
more “s” character
sp3 sp2 sp
bigger“tail”
more electrondensity in thebonding lobe
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BOND STRENGTHS - MULTIPLE BONDSBOND STRENGTHS - MULTIPLE BONDS
CC bond bond bond energy molecule bond type length per mole measured
Kcal (KJ)
C-C sp3-sp3 1.54 Å 88 (368) CH3- CH3
C=C sp2-sp2 1.34 Å 145 (607) CH2=CH2
C=C sp - sp 1.21 Å 198 (828) HC=CH= =
increasings-character
and p - p
and two p-p
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Bond EnergyBond Energy
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Molecular Distortions: Molecular Distortions: VSEPR Revisited VSEPR Revisited
Four situations:
1) electron pair repulsion
2) effect of electronegative atoms
3) double bond and electronegativity
4) steric repulsion
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C
H
H HH
:
:....
symmetrical moleculeall repulsions are equal
perfect tetrahedral
all angles 109o28’
NH H:
....
H
.. anglebecomeslarger
larger repulsion
repulsionsmaller angle becomes
smaller
not all pairs are equivalent
the unshared pairs repel morestrongly than the bonded pairs
Electron Pair RepulsionElectron Pair Repulsion
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Effect of double bond and electronegativity
C CHH
H H
C OH
H
C CH2
H
H
C CH2
Cl
Cl
C CH2
F
FC O
F
F
C OCl
Cl
C OH
H
117o
121.5o
121.5o
123o
125o
117o
114o
110o
116o
122o
116o
124.5o
126o
111o
108o
122o
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Most pi bonds have a bond energy of
50 - 60 Kcal / mole( 210 - 250 Kj / mole )
MOLECULES WITH PI BONDSMOLECULES WITH PI BONDS
When the total energy of a multiple bond is given,you must subtract the energy of the pi bonds toobtain the sigma bond energy.
C=C 145 Kcal/mole C-C = 95 Kcal/mole
( 145 - 50 = 95 )bothbonds
thus:
TOTAL BOND ENERGY
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Non Bonded Electrons (unshared pairs) do not significantly change their energyin going from an atom to a bonded molecule
MOLECULES WITH UNSHARED PAIRSMOLECULES WITH UNSHARED PAIRS
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OC
H
H
H
H
2s2p
sp3 hybrids
hybridization C OHH
H
Hsp3 sp3 Metanol
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2s2p
sp2
hybridization
2p
2p
C O
H
HC
HO
H
used for
bond
used for
bonds
sp2
sp2
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2s2p
sp hybrids
hybridization
2p
2p
NCH
C NHsp sp
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C CC
H
H
H
H
C C CH
H
H
Hallena
sp2
sp2sp
CH
HH H
endview
molecule has a twist in the center
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Start with theLewis Diagram
Determine thegeometry ofeach atom
Use the correct hybid in eachcase
Assemble themolecule fromthe hybrids.
C N
H
H
H
H
H :
C = 4 pair = tetrahedralN = 4 pair = tetrahedral
C = sp3 N = sp3
VSEPR
C N
C NH
H
H
H
H
ASSEMBLY METHODASSEMBLY METHOD
..
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Sample ProblemsSample Problems
Predict the hybridization, geometry, and bond angle for each atom in the following molecules:
Caution! You must start with a good Lewis structure!– NH2NH2
– CH3-CC-CHO
CH3 C
O
CH2
_