The document discusses hybridization in chemistry, detailing how atomic orbitals combine to form new hybrid orbitals, specifically outlining sp, sp2, and sp3 hybridization with examples. It also describes the molecular geometry of simple inorganic molecules and ions, categorizing them into five main shapes and providing bond angles and examples for each type. References include an NCERT textbook and Byju’s for further reading.

1. COURSE CODE: ED1101
COURSE NAME: ATOMIC STRUCTURE AND BONDING
TOPIC: TYPES OF HYBRIDIZATIONSHAPES OF
SIMPLE INORGANIC MOLECLUES AND IONS.
SUBMITTED BY:
ED24B1019
KIRTI VINAY JAMBHALI
CHEMISTRY MAJOR
ITEP- B.SC, B.ED,
I YEAR
NATIONAL INSTITUTE OF TECHNOLOGY
PUDUCHERRY
SUBMITTED TO:
MR.S. DETCHANAMURTHY
FACULTY OF CHEMISTRY,
DEPARTMENT OF EDUCATION,
NATIONAL INSTITUTE OF TECHNOLOGY
PUDUCHERRY.

2. WHAT IS HYBRIDIZATION ?
 Hybridization combines atomic orbitals to form
new ones for bonding in molecules.
 This intermixing usually results in the formation
of hybrid orbitals having entirely different
energies, shapes, etc.
 The atomic orbitals of the same energy level
mainly take part in hybridization.
 Possible hybrid combinations are sp,sp2
,sp3
,
sp3
d,sp3
d2
.

3. sp3
HYBRIDISATION
 When one s orbital and three p orbitals from the same
shell of an atom mix together to form a new equivalent
orbital then this is called sp³ hybridization.
 For example CH4,NH3,
etc.
Bond Angle = 109.5°

4. sp2
HYBRIDISATION
 When one s orbital and two p orbitals from the same
shell of an atom mix together to form a new equivalent
orbital then this is called sp2
hybridization.
 For example, C2H4 ,BF3 etc. Bond Angle = 120°

5. sp HYBRIDISATION
 When one s and one p orbital from the same shell of an
atom mix together to form a new equivalent orbital then
this is called sp hybridization.
 The molecules which show sp hybridization, have a
linear shape and an angle of 180°.
 For example, BeCl2,BeF2 ,etc.

6. GEOMETRY OF SIMPLE
MOLECULES / IONS
 The study of the three-dimensional arrangement
of the atoms that constitute a molecule is called
Molecular geometry.
 Five main shapes
1)Linear
2)Trigonal planar
3)Tetrahedral
4)Trigonal bipyramidal
5)Octahedral

7. LINEAR
 No. of electron pairs : 2
 Bond angle : 1800
 BeCl2 , HgCl2
 No. of electron pairs : 3
 Bond angle : 1200
 BF3
TRIGONAL PLANAR

8. TETRAHEDRAL
 No. of electron pairs : 4
 Bond angle : 109.50
 CH4
 No. of electron pairs : 5
 Bond angle : 900
&1200
 PCl5
TRIGONAL BIPYRAMIDAL

9. OCTAHEDRAL
 No. of electron pairs : 6
 Bond angle : 900
 SF6

10. TRIGONAL PLANAR
 Molecule type : AB2E
 No. of bonding pairs : 2
 No. of lone pairs : 1
 Shape : Bent
 Angle : 119.50
 Example : SO2
O3

11. TETRAHEDRAL
 Molecule type : AB3E
 No. of bonding pairs : 3
 No. of lone pairs : 1
 Shape : Trigonal pyramidal
 Angle : 1070
 Example :NH3
 Molecule type : AB3E2
 No. of bonding pairs : 2
 No. of lone pairs : 2
 Shape : Bent
 Angle : 1050
 Example :H2O

12. TRIGONAL BI-PYRAMIDAL
 Molecule type : AB4E
 No. of bonding pairs : 4
 No. of lone pairs : 1
 Shape : See saw
 Angle : 900
& 1200
 Example :SF4
 Molecule type : AB3E2
 No. of bonding pairs : 3
 No. of lone pairs : 2
 Shape : T-shape
 Angle : 900
 Example :ClF3

13. OCTAHEDRAL
 Molecule type : AB5E
 No. of bonding pairs : 5
 No. of lone pairs : 1
 Shape : Square pyramid
 Example : BrF5
 Molecule type : AB4E2
 No. of bonding pairs : 4
 No. of lone pairs : 2
 Shape : Square planar
 Example : XeF4

14. CHART

15. REFERENCES
NCERT Textbook for 11th
Part I
Byju’s

16. END