hybridization ppt

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


3. Which of the following molecule has 120o bond angle?

A. IF3

C. HCl D. C2H4

B. PCl3


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


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


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

2. ANSWER : C

the carbon in CO2 is sp

hybridized.

All sp hybridized is linear

3. ANSWER : D

Thus, shape is trigonal

planar The bond angle is 120o

C2H4 is sp2 hybrid

orbitals

4. ANSWER : C II,III, IV

Structure I, C2H6 did not have any pi bond

It undergo sp3 hybridization

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+


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


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


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

hybridization ppt

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