HYBRIDIZATION : SP3, SP2 & SP
HYBRID ORBITAL
INTRODUCTION
EMPOWERING
ENHANCING
CLOSURE
VIDEO
What is hybridization?Please watch this video to know more..
INTRODUCTION
EMPOWERING
THEORY
QUIZ
CH CH
methane ethylene acetylene
What can you see from these 3 compounds??
All of the three compound is
covalently bonded with each other
Carbon in methane is bonded with four hydrogen atoms and
has single bond
Each carbon in ethane is bonded with three
other groups and the carbon is connected by
the double bond
Carbon in acetylene is bonded with only two groups and the carbon
is connected by the triple bond
• We can see that the central atom, which is carbon is covalently bonded with other groups in the compound.
• But, how does the bonding occur??
Valence Bond Theory
Hybrid Orbital Theory
Lets take a closer look
towards these two theory
Valence bond theory describes covalent bonding as the overlap of two atomic orbitals with the electron pair in the resulting bond being shared by both atom.From this theory, carbon can only form two bonds because on its valence shell only has two unpaired electron and the resulting molecule is CH2.
Carbon :1s 2s 2p
-CH2 is a very reactive molecule and cannot exist outside the molecular system-So, how does the bonding occur???-now, lets take a look at the hybrid orbital theory
hybrid orbital
New orbital that results from the combination of
two or more atomic orbitals
According to the hybrid orbital theory, an electron form 2s orbital is excited to the 2p orbitalNow, the carbon is in the excited stateThe bonding of molecule now is called hybridisation Hybridisation is the combination of two or more atomic orbitals to form the same number of atomic orbitals
Carbonground state :1s 2s 2p
Carbonexcited state :
2s 2p
So now, we can proceed to the next part on how are we going to determine type of hybridisation
How To Determine Type Of Hybrid Orbital?
CH CH
methane ethylene acetylene
Back to the structure that we see at the beginningThe obvious differences between the three molecule is the type of bonding that they have where methane has single bond, ethylene double bond and acetylene triple bondThe type off bonding will determine their type of hybridisation.
METHANE, CH3
Carbonexcited state :2s 2p
Now, lets take a look again at the carbon in excited stateSince carbon is bonded to four hydrogen atom, four hybrid orbitals is usedThe hybridization now is called as the sp3 hybrid orbitals Carbonhybridized :
sp3 sp3 sp3 sp3
WHY SP3 HYBRID ORBITALS?
Because it is formed from 1 s orbital and 3 p orbitals forming the sp3 hybrid orbitalsMixing the spherical 2s orbital and three dumbbell shaped 2p orbital produces four orbital having large lobe and small lobe
s orbital p orbital
sp3 hybrid orbital
hydrogen atom overlaps with the four sp3
hybridized orbital form four sigma bond
The geometry is tetrahedral
The bond angle is 109.5o
ETHYLENE, C2H4
Carbonexcited state :
2s 2p
We can see that carbon molecule in ethylene is bonded to three groups only which is carbon and two hydrogen This means that, only three hybrid orbitals is used Thus, forming the sp2 hybridization sp2 sp2 sp2
2pCarbonhybridized :
But now, what will happen to the 2p orbital
that is unhybridized?
oThe second C-C bond result from the side-by-side overlapsoSide by side overlaps create electron density above and below plane of sp2 hybrid orbitals.oThis bond is called π bond.o π bonds are weaker and easily broken than sigma bond
How many bonds present in the ethylene
molecule?
There are six bonds in the ethylene molecule
1 sigma bond within C-C and 4 sigma bonds between C-H1 pi bond between C-C molecule
Sigma bonds
Sigma bonds
Pi bond
The geometry of ethylene molecule is trigonal planarThe hybrid orbitals all lie on the same planeIt cannot rotate freely because of the presence of pi bondH-C-H and H-C-C bond angles are about 120o
What is the geometry of this
compound?
CH CHACETYLENE, C2H2
By looking at the Lewis structure of acetylene, can we
describe the molecular
geometry, and the type of
hybridization??
Yes, we canBased on the Lewis structure, each Carbon atom is singly bonded to the Hydrogen atom and triply bonded to each Carbon atom.So, each carbon atom is surrounded by two groups resulting linear geometry and sp hybridized.The bond angle is 180o
Carbonexcited state :2s 2p
sp sp2p 2p
Carbonhybridized :
Since there are only two groups surrounding the carbon atom, only 2 hybrid orbitals is used to form the sp hybrid orbitals which are the C-H
bond and C-C bondThe other two 2p orbital is
unhybridised
What is the difference between hybridized orbital and unhybridised orbital??
Hybridized orbital is the C-H bond and the C-C bond. Both bonds result from the end-to-end overlap of sp hybrid orbital and 1s orbital and also sp hybrid orbital with sp hybrid orbital on each carbonThis result the formation of sigma bondUnhybridized orbital results from the side-by-side overlap between the two sp orbital to the other carbons creating the 2nd and 3rd bond of the C-C triple bond.Both of these bonds are pi bonds
How many sigma and pi bond are
present?
There are three sigma bonds in acetylene which are the C-C bond and two from the C-H bond.Meanwhile, there are 4 pi bonds in these compound
The linear geometry of the acetylene molecule
QUIZ
CHOOSE THE RIGHT ANSWER FOR THE
QUESTION.
1. Which molecule is not linear?
A. BeF2
D. H20C. CO2
B. BeH2
CLICK TO SHOW EXPLANATION
2. Which molecule is linear?
A. NO2
C. CO2 D. H2S
B. ClO2
CLICK TO SHOW EXPLANATION
3. Which of the following molecule has 120o bond angle?
A. IF3
C. HCl D. C2H4
B. PCl3
CLICK TO SHOW EXPLANATION
4. Which of the following hybrid orbitals consist of a pi bond and
sigma bond
I. C2H6
II. BeH2
III. CO2
IV. C2H4
A. I and II
C. II, III and IV D. I, II, III and IV
B. I, II, and III
CLICK TO SHOW EXPLANATION
5. The central atom in a CH4 molecule is in hybrid state. The
shape of molecule will be
A. Trigonal pyramidal
C. Pyramidal
B. Tetrahedral
D. Trigonal Planar
CLICK TO SHOW EXPLANATION
CONGRATULATIONS, THAT IS THE CORRECT ANSWER!!
SORRY, PLEASE TRY AGAIN..
1. ANSWER : D
H2O did not have linear shape
because oxygen atom have two lone
pair electrons
The lone pair repels the two Hydrogen
atom, to bond angle of 104.5o
CONGRATULATIONS, THAT IS THE CORRECT ANSWER!!
SORRY, PLEASE TRY AGAIN..
2. ANSWER : C
the carbon in CO2 is sp
hybridized.
All sp hybridized is linear
CONGRATULATIONS, THAT IS THE CORRECT ANSWER!!
SORRY, PLEASE TRY AGAIN..
3. ANSWER : D
Thus, shape is trigonal
planar The bond angle is 120o
C2H4 is sp2 hybrid
orbitals
CONGRATULATIONS, THAT IS THE CORRECT ANSWER!!
SORRY, PLEASE TRY AGAIN..
4. ANSWER : C II,III, IV
Structure I, C2H6 did not have any pi bond
It undergo sp3 hybridization
CONGRATULATIONS, THAT IS THE CORRECT ANSWER!!
SORRY, PLEASE TRY AGAIN..
5. ANSWER : B
Geometry of CH4 is tetrahedral
Carbon is bonded to four hydrogen atom forming sp3
hybrid orbital
Geometry of sp3 hybrid orbital is
tetrahedral
ENHANCINGACTIVITY 4
ACTIVITY 3
ACTIVITY 2
ACTIVITY 1
SNAKE AND LADDER GAME
Instruction to play this game.
• Roll a dice.• Move the button according to the number on the dice.•When you reach the ladder, you can simply move up the ladder.•But, if you reach the snake, you must choose any number from 1 until 15 and answer the question.•When it is answered correctly, then the game can be continued.
QUESTIONS
CLICK TO CHECK THE ANSWER
THE POWER OF EXPLAINING
Use the hybridization theory to explain the formation of the following molecules, regarding to
• Lewis structure• Ground state• Hybridized state
a) O2
b) ClO3-
c) OF2
d) CH3+
CLICK TO CHECK THE ANSWER
TEST YOUR DRAWING SKILL HERE
Deduce the type of hybridization of each atom, draw the overlap of the orbitals, and state the bond angles for the
following compounds.
• CH3Cl • NO 3
-
• CH3C CCH2OH
CLICK TO CHECK THE ANSWER
G B D S N X Z R T A A A N K F L
P O Y U D V A X M V B S W Q R E
M H Y N F E Z G A D L K T W Q C
P J J O N D I T H U A M F S A E
L E W I S S T R U C T U R E P T
A O L T Q S G H H Y I D A K O H
N I I A Y F S L K J B E R E E Y
A D H Z C K T D S A R E Q W N L
R N M I K E L D R B O N D S Q E
H U Y D E W T Q S F F G I K L N
U I K I J W E Y Z Z X C B V V E
Z C V R N M U E L G N I S C V Z
X A Q B S G H F K E L P O F R E
C U I Y Z V M B D G N H P H F I
F J T H Y M E T H A N E R W A S
C V T E T R A H E D R A L B L R
Let’s find the hidden word..
acetylene bond ethylene hybridization Lewis structure linear methane orbital pi planar sigma single tetrahedral
WORD PUZZLE
CLICK TO CHECK THE ANSWER
G B D S N X Z R T A A A N K F L
P O Y U D V A X M V B S W Q R E
M H Y N F E Z G A D L K T W Q C
P J J O N D I T H U A M F S A E
L E W I S S T R U C T U R E P T
A O L T Q S G H H Y I D A K O H
N I I A Y F S L K J B E R E E Y
A D H S C K T D S A R E Q W N L
R N M I K E L D R B O N D S Q E
H U Y D E W T Q S F F G I K L N
U I K I J W E Y Z Z X C B V V E
Z C V R N M U E L G N I S C V Z
X A Q B S G H F K E L P O F R E
C U I Y Z V M B D G N H P H F I
F J T H Y M E T H A N E R W A S
C V T E T R A H E D R A L B L R
Finally, I got all the answers..
(^_~)
LIST THE DIFFERENCES OF HYBRID ORBITLAS BETWEEN METHANE,
ETHYLENE AND ACETYLENE
CLOSURE
HYBRIDIZATION SP3 HYBRID ORBITALS SP2 HYBRID ORBITALS SP HYBRID ORBITALS
STRUCTURE
GEOMETRY TETRAHEDRAL TRIGONAL PLANAR LINEAR
BOND ANGLE 109.5o 120o 180o
BONDING GROUP 4 BONDING GROUP 3 BONDING GROUP 2 BONDING GROUP
NON-BONDING GROUP 0 NON-BONDING GROUP
1 NON-BONDING GROUP
2 NON-BONDING GROUP
SIGMA BOND FORM 4 SIGMA BOND 3 SIGMA BOND FOR EACH CARBON
2 SIGMA BOND FOR EACH CARBON
PI BOND FORM 0 PI BOND 1 PI BOND 2 PI BOND
From our learning session today, we can
conclude that
There are three types of hybridisation which is sp3, sp2 and sp hybrid orbitals
Geometry for sp3
hybridization is tetrahedral and the bond angle is 109.5o
Geometry of sp2 hybridization is trigonal
planar and the bond angle is 120o Geometry for sp
hybridization is linear and bond angle is 180o
THE END