Normal and orthogonal wave function

Normal wave function:

if probability of finding electron in space is unity i.e 100℅ the wave function sie is said to be normalised

or Integration of ꌏ^2 over the whole space must be equal to 1

∫ꌏ^2 dxdydz = 1

if the wave function satisfied the above relation .it is said to be normalised.

Orthogonal wave function :

if ꌏ(1) and ꌏ(2) represent two different acceptable wave function.

the product of two wave functions integrated over the entire space must be equal to zero.

∫ꌏ(1)ꌏ(2) dxdydz = 0

the wave function which obey the above relation is said to be orthogonal.

# if wave function -ve than called imaginary.
# if wave function +ve than called real.

wave function which are both normalised and orthogonal are called orthagonal normalised function.

Comments

Bsc subject chemistry (inorganic sem-1) complete notes

INORGANIC CHEMISTRY BSC SEMESTER -1 section A ...

Electronegativity scales and disadvantage of scales and its nunericals

Electronegativity scales: 1.Pauling scale of electronegativity: in diatomic molecule (A-B) ,the bond formed between two atoms A and B will be intermediate between pure Covalent (A-B) and pure ionic character, the bond between A and B will be strong than bond energy increased. if bond (A-B) has been purily covalent than bond energy can be calculated as average bond energy of bond (A-A) and bond (B-B). that means it is equal to bond energy of bond (A-B) E(A-B) = 1/2[ E(A-A) +E(B-B) ] however experiemental value of bond (A-B) more than this value because of difference in electronegativity of A and B the difference ∆ is given by simple expression ∆ = E(A-B) - 1/2 [E(A-A) +E(B-B) ] where E(A-B) is experimental value of bond energy. if Ҳ(A) and Ҳ(B) are the electronegative of elements A and B than Ҳ(A) - Ҳ(B) = 0.18√∆ for numerical ∆ = E(A-B) -[√(E(A-A) ×E(B-B) )] Disadvan...

Radial probability distribution for p and d orbital, radial wave functions

Radial probability distribution for p and d orbital Radial and Angular wave function: the radial part of wave function depends upon quantum no. n and l and gives the distribution of electron w. r. t distance .it is governed mainly exponential term e^-Zr/na°(a not) here e based on natural log. Z Atomic number r distance from nucleus n principal quantum no. or radial quantum no. a° 0.529A° for hydrogen ( Bohr radii) the exact mathematical expression for radial part of wave function for 1s or 2s and 2p orbitals. n= 1 ,l=0 s orbital R(r) =2× (z/a°) ^3/2 ×(2-zr/a°) ×e^-zr/2a° n= 2 ,l=0 2s orbital R(r) = (z/a°) ^3/2 ×(2-zr/a°) ×e^-zr/2a° n= 2 ,l=1 2p orbital R(r) = 1√3×(z/2a°) ^3/2 ×(zr/a°) ×e^-zr/2a ° the rad...

Chemistry

Search This Blog