2. Presentation Ikatan Kimia (Rev)
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Transcript of 2. Presentation Ikatan Kimia (Rev)
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DISCUSS CONTENT:
A. Electron Configuration Stability
1. Octet Rule
2. Lewis Structure
B. Kind of Chemical Bond
1. Ionic
2. Covalent
3. Coordination
C. Hybridization and Molecule Shape
1. sp 4. sp3d
2. sp2 5. sp3d2
3. sp3
D. Complex Ion Hybridization
E. Noble Gas Compound
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A. Electron Configuration Stability
The Stable Configuration is Electron Configuration which owned by the noble gas.
Those Configuration are:
He 2
Ne 2 8
Ar 2 8 8
Kr 2 8 18 8
Xe 2 8 18 18 8
Rn 2 8 18 32 18 8
2 8 18 32 32 18 8
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Octet Rule (Lewis Rule)We have Known that
Except of Ne, The end Noble gas electron configuration is 8 electron,
so, all particle with 8 electrons at the outer shell is stable
because of this fact
All Elements (specially representative group) tend to have 8 electrons at their outer shell
Octet Rule (Lewis Rule)
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Elements Tendency
Metal Tendency Non Metal Tendency
The atoms of Metal element tend
to release the electron
The atoms of Non Metal element
tend to accept/catch the electron
WHY
The Metal element electrons are more than noble gas electron
The Non Metal element electrons are less than noble gas electron
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Fill in The BlankElement Tendency Stable Form
11Na release/accept 11Na+
20Ca
10X
52Y
33A
17Cl
35Br
53X
86X
18Z
Write the electronic formula/Lewis Structure of all particle in the above table.
Note:
Lewis Structure is atomic symbol with the electron valence
release
release20Ca2+
stable 10X
accept 52Y2
accept 33A3
accept 17Cl
accept 35Br
accept
stable
53X
86X
stable 18Z
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Write the electronic formula/Lewis Structure of representative group
Lewis Formula of Sodium
Lewis Formula of Berilium
Lewis Formula of Boron
Lewis Formula of Carbon
Lewis Formula of Nitrogen
Lewis Formula of Oxygen
Lewis Formula of Fluorine
Lewis Formula of Neon
Na
Be`
B
C
N
O
F
Ne
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CHEMICAL BOND
Formed by Transfer of electron from metal to non metal atom
(Ionic bond)
Formed by Sharing of electron between non metal and non
metal atom
Covalent Bond
Coordination Bond
+
+
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Ionic Bond:
11Na 2 8 1 11Na+ 2 8 + e
17Cl 2 8 7 + e 17Cl 2 8 8
Na+ Cl
bonded by attractive force/electrostatic force/ Coulomb force
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Ionic Bond Characteristic :
1. Very High bond strength
2. High melting and boiling point
3. Conductor in melt or solution condition
4. Formed by cationic and anionic
5. Can form cationic and anionic
How ionic mechanism of these following couple :
a. 19K and 8O
b. 20Ca and 9F
c. 31X and 16Y
d. 11X and 7Y
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Covalent Bond :
a. H2
H HHH
b. O2
OO
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b. O2
O O`
C. N2
N NN N
How is the Lewis formula of covalent compound formed of:
(Made by your self)
1. P and O 2. S and H 3. Cl and O
Write the Lewis Formula of ..............
1. Cl2O3 2. CO2 3. P2O3 4. P and Cl
Covalent bond is the binding of single electron orbital of non metal atom with single electron orbital of another non
metal atom
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Coordination BondLet we look N and H binding:
N
H
H
H
If the fourth H atom came to NH3 molecule , Can NH3 accept it ?
No, if the fourth H came as neutral atom, but will be
accepted if H came as H+ ion. WHY ?????
Illustration of binding between NH3 and H+ is
N
H
H
H
H
+
Coordination /dative bond
Coordination bond is binding between lone pair orbital (as electron pair donor) and empty orbital (as electron pair acceptor)
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Exercise :
Write Structure Formula, Lewis Formula of these following substance. Determine how many covalent binding , coordination binding and lone pair elektron of them.
(Do by your self)
1) SO 2) SO2 3) SO3 4) P2O3 5) P2O5
6) H2SO4 7) H3PO48) CO2 9) CO 10) Ca3(PO4)2
NOTE: The Exception of Lewis Rule.
Some molecule not agree to Lewis Rule ( octet rule) these molecule are:
1) BeX2 2) BX3 3) PX5 4) SX6
To prove them, write the electronic structure of them. Seem that each of them are not octet, but they are stable molecule.
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Before one atom binds two or more another atoms, this atom will hybridize orbital (electron valence orbital) which will be used. The kind of covalent molecule hybridization are:
Hybridization Shape bond angle
sp Linear 180o
sp2 planar triangle 120o
sp3 tetrahedron 109.5o
sp3d hexahedron 1200 ; 900 ; 1800
sp3d2 octahedron 900 ; 1800
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1. Hybridization of BeCl2
4Be = (2He) 2s2 2p0
Berilium must have two single electrons for binding two Cl atoms, so electron valence be:
these 2 orbital energy made be equal (hybridization) and called sp hybridization
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2. Hybridization of BF3
5B = (2He) 2s2 2p1
B must have three single electrons for binding three F atoms, so electron valence must be promote to:
these three orbital energy made be equal (hybridization) and called sp2 hybridization
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3. Hybridization of CH4
6C = (2He) 2s2 2p2
C must have 4 single electrons for binding 4 H atoms, so electron valence must be promote to:
these 5 orbital energy made be equal (hybridization) and called sp3 hybridization
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4. Hybridization of PCl5
15P = (10Ne) 3s2 3p3 3d0
P must have 5 single electrons for binding 5 Cl atoms, so electron valence must be promote to:
these 5 orbital energy made be equal (hybridization) and called sp3d hybridization
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5. Hybridization of SF6
14S = (10Ne) 3s2 3p4 3d0
S must have 6 single electrons for binding 6 Cl atoms, so electron valence must be promote to:
these 6 orbital energy made be equal (hybridization) and called sp3d2 hybridization
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6. Hybridization of NH3
7N = (2He) 2s2 2p3
N has 3 single electrons for binding 3 H atoms, so electron valence must be still in initial condition (no promotion):
these 4 orbital energy made be equal (hybridization) and called sp3 hybridization
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7. Hybridization of H2O
8O = (2He) 2s2 2p4
O has 2 single electrons for binding 2 H atoms, so electron valence must be still in initial condition (no promotion):
these 4 orbital energy made be equal (hybridization) and called sp3 hybridization
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Illustration of molecular shape :
Linear Molecule of sp hybridization. Example BeF2
Be`F F1800
B
F F
F
Planar Triangle of sp2 hybridization of BF3
1200
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Tetrahedron of sp3 hybridization of CH4
CH
H
H
H
Hexahedron of sp3d hybridization of PCl5 P
Cl
Cl
Cl
Cl
Cl``
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Octahedron of sp3d2 hybridization of SF6
SF F
F
F
F
F
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Covalent Molecule Polarity
All asymmetric molecule
or
Molecule with lone pair elektron in central atom
POLAR
≠ 0
Non POLAR
= 0
All symmetric molecule (general)
or
Molecule without lone pair in central atom (Note: agree for diatomic molecule only)
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Complete this blanc like the example
Molecule Polarity
BF3 non pol.
NH3
PCl5
CH4
CH3Cl
H2SO4
CO2
HCl
H2O
BeCl2
cov. bond Polarity Polarity