2. Presentation Ikatan Kimia (Rev)

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

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

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)

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

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

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

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

+

+

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

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

Covalent Bond :

a. H2

H HHH

b. O2

OO

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

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)

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.

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

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

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

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

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

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

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

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

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

Tetrahedron of sp3 hybridization of CH4

CH

H

H

H

Hexahedron of sp3d hybridization of PCl5 P

Cl

Cl

Cl

Cl

Cl``

Octahedron of sp3d2 hybridization of SF6

SF F

F

F

F

F

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)

Complete this blanc like the example

Molecule Polarity

BF3 non pol.

NH3

PCl5

CH4

CH3Cl

H2SO4

CO2

HCl

H2O

BeCl2

cov. bond Polarity Polarity