CHEMICAL BONDING #Types of bonds Electrovalent bond Covalent bond Coordinate bond Metallic bond

1. SAVITRIBAI PHULE UNIVERSITY
(INORGANIC CHEMISTRY)

2. • Name- Amruta Suhas Vaidya
• Year- FYBsc.Bed (2020-21)
• Subject code- BSC 221
• Topic Name- Chemical bonding
• Teacher- Dr.Sudarshan Tapsale sir.

3. CHEMICAL BONDING
• The force of attraction holding the atoms together in a molecule is called chemical
bond.
Types of bonds-
• Electrovalent or ionic bond
• Covalent or electron pair bond
• Co-ordinate or dative bond
• Metallic bond

4. IONIC BOND
• The formation of ionic bond involves transfer of one or more electrons from one
atom to another to complete their octet.

5. COVALENT BOND
1. The bond formed by sharing of one or more pairs of electrons between two
atoms is called a covalent bond.

6. CO-ORDINATE BOND
• The co-ordinate Bond formed between two atoms by a pair of electrons provided
entirely by one of the combining atoms but shared by both.

7. METALLIC BOND
• The force that binds a metal ion to mobile electrons within its sphere of influence is
known as a metallic bond.
• The metallic bond can explain
Characteristic properties of metal
Such as luster, ductility, malleability,
And conductivity.

8. IONIC BOND
BORN –LAND EQUATION FOR CALCULATION OF LATTICE
ENERGY
• The lattice energy is the energy change when 1 mole of Crystal is formed from its component ions in
the gaseous state.
• For NaCl lattice energy is -781kj per mol
• Two methods are use to calculate lattice energy
• Theoretical equation Experimental methode
• By using born land equation by using born haber cycle

9. BORN HABER CYCLE

10. Application of Born-Haber cycle
• It can be used to calculate any of the Other quantity when all
other quantities are known
• It is also useful in knowing the nature of bonding in the
compound
• It can be used to calculate the energy of hydration of ions
• It can be used as a check on calculated energies

11. SOLUBILITY OF IONIC SUBSTANCES IN WATER
• Solubility of one substance in another substance depends on the inter ionic or a
intermolecular forces between the two substances .The solubility of ionic
substance in water involves the the consideration of of forces between the ions
(lattice energy) and the forces between the ion and water molecules (solvation
energy)
• If the solvent is water then solvation energy is called as hydration energy
• Solubility of ionic solid depends upon the
1) The lattice energy of the ionic solid
2) Solvation energy of the solvent

12. POLARISING POWER AND POLARIZABILITY FAJANS
RULE

13. IN 1924 FJANAS STATED FOUR RULES RELATING
IONIC CHARGE AND SIZE OF THE ION
• Large charge either on anion or on cation favour covalency -this is due to fact
that a high charge increase this the amount of polarization
• Small cation favours covalency- a small cation has greater polarization effect
upon and anion than a large cation this is because of the greater concentration of
positive change
• Large anion favours covalency- it is well known fact that the the large anion
would be more polarisable than the smaller anion

14. • Cation with non inert gas configuration- the cation with 18 electron structures
have been found to to effect greater anion distortion then doors with inert gas
structure (8 electron structure) even if the same size and charged or taken
because of this the melting point of anhydrous chloride of copper silver and gold
(18 electron structure) are lower than those of sodium Potassium (8 electron
structure)

15. IONIC CHARACTER OF COVALENT BOND
• Covalent bond between an atom A and an atom B involves sharing
of electrons it is known as A*x B.
• An ionic Bond involves complete transfer of electron it is shown as
[A]+ [x*B]-

16. • The degree of polarity of a polar molecule is expressed in term
of dipole moment which is equal to the product of electric
charge and the distance in angstrom between the positive and
negative centers.
• =e×d
• Thus Greater the value of the dipole moment of a molecule
greater is the polarity of the bond between the atoms.

17. VALENCE BOND THEORY
• Covalent bond is formed by overlapping of atomic orbital (atoms should come very
close)
• Only half field orbitals with electronic opposite spin overlap
• Overlapping must be less than 50 degree
• Extent of overlapping decides strength of of Bond
• Two types of overlapping her possible
1) Axial overlapping or head on overlapping >>> Sigma bond
2) Parallel overlapping or sidewise overlapping>>>Pi bond
• The overlapping orbitals must have same sign

19. HYBRIDISATION
• The process of mixing and recasting of atomic orbitals of slightly
different energies in an isolated atom to form a set of new orbitals
having equal energy is called hybridization and the the new orbitals
are called as hybrid orbitals.

20. CHARACTERISTICS OF HYBRIDIZATION
• Orbitals Of the same atom or ion can undergo hybridization
• The orbitals which slightly differ in their energy can take part in hybridization
• Atomic orbital undergo hybridization usually when atom is in excited state
• Hybrid orbital of one atom can overlap atomic orbitals or hybrid orbitals of other
atoms and form covalent bonds
• The shape of the molecule and bond angle are suggested by the type of
hybridization and orientation of Orbitals

21. TYPES OF HYBRIDISATION AND GEOMETRY OF THE MOLECULE
HAYBTIDIZATION USING ‘S’ AND ‘P’ ORBITALS
• Diagonal or linear sp hybridisation
• The mixing of one s and one p orbital to form two new equivalent hybrid orbitals of
identical energy and shape is known as sp hybridisation, Due to Linear shape it is
called as diagonal hybridization.
• Bonding in BeH2 molecule

23. TRIAGONAL SP2 HYBRISISATION
• The mixing of 1S and 2P orbitals to form three new equivalent hybrid orbitals of
identical energy and shape is known as SP2 hybridization
Bonding in BF3 Molecules

25. TETRAHEDRAL SP3 E HYBRIDIZATION
• The mixing of One S and three p orbitals to form four new
equivalent hybrid orbitals of identical energy and shape is known as
SP3 hybridization due to the tetrahedral shape of the molecule it is
called as tetrahedral hybridization the molecules in which the
central atom shows SP3 hybridization are are methane, ethane, etc.

26. SP3 HYBRIDISATION OF METHANE

27. HYBRIDISATION USING D ORBITALS

28. SQUARE PLANAR DSP2 HYBRIDISATION
• The mixing of one d One s and 2P orbital to form four new
equivalent hybrid orbitals of equal energy and shape is known as
dsp2 hybridization due to the square planar shape of the molecule
it is called as square planar hybridization

30. TRIGONAL BIPYRAMIDAL DSP3 OR SP3D
HYBRIDISATION
• The mixing of 1S 3p and 1D orbitals to form on non equivalent set of 5 hybrid orbitals is called
DSP 3 hybridization. Due to Trigonal bipyramidal shape of molecule it’s called trigonal
bipyramidal hybridization
• Bonding in Fe(CO)5

32. OCTAHEDRAL SP3D2 TO HYBRIDIZATION
• The mixing of 1S 3p and 2 d orbital to form a set of 6 equivalent
hybrid orbital it’s called sp3d2 hybridization.DueTo the the
octahedral shape of the molecule it is called octahedral
hybridization

35. V S E P R THEORY
(VALENCE SHELL ELECTRON PAIR REPULTION
THEORY)
• This theory can explain the shape of simple molecules having bonded or non-
bonded localised electron pair.
• 1) Electron pair are always ripelling each other and tries to remain far apart.
• 2)Different electron pair have different order of repulsion.
• 3)If lone pair is zero then geometry is shape.
• 4)Geometry is depends upon Bond pair and lone pair.
• 5)Shape is depends upon surrounding atom.

36. BONDING AND SHAPE OF CLF3 MOLECULE

37. • Bonding and ahape of Cl2O molecule
• Stucture –Tetrahedron
• Lone pair- 2
• The bond angle not equal to tetrahedral angle of 109 degree 28 ‘
It is 111 degree.

38. BONDING AND SHAPE BRF5 MOLECULE

39. BONDING AND SHAPE OF XENON TRIOXIDE

40. BONDING AND SHAPE OF XENON OXYFLUORIDE

41. LIMITATIONS OF VSEPR THEORY
• Shapes of highly polar molecules cannot be explained by VSEPR theory.
• Shapes of molecules with extensive delocalised electrons system cannot
be explained by VSEPR theory.
• VSEPR theory cannot explain shapes of certain molecules having inert
pairs of electrons.
• VSEPR theory is unable to Predicts shapes ofsome transition metal
complexes.