shape of p, d orbital

Shape of p orbital:

for p sub shell

l=1

m=-1, 0,+1

i. e P subshell has three possible orbital desigrated as named as

These three orbital are of equal energy but differ in orbital or orientation. P orbital is domb-bell shaped and probability of finding the electron in both the lobes are same.
Shape of d orbital:

for d sub shell

l=2

m =-2, -1, 0,+1, +2

since there are five values of m. so there are five possible orientation named as dxy, dyz, dzx, dx^2y^2.

The three orbital dxy ,dyz, dzx, are similar in shape each consisting of four lobes of high electron density lying b/w the axis.

dx^2y^2 orbital also have four lobes High electron density lying along the y axis & x-axis

dz^2 orbital is symmetrical about z-axis and is dombbell shaped. in this orbital the part of orbital lying in the direction of magnetic field is enclosed and part of orbital lying perpendicular to it is contracted

Comments

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 curves

Radial probhjjhajajbability distribution curves: The probability of finding the electron is given by the quantity sie^2.By radial probability us probability of finding the electron within small Radial space around the nucleus. volume of spherical shell between radius r and r+dr =4πr^2 and probability of finding the electron will be 4πr^2dr sie^2. radial probability distribution curves are obtained by plotting radial probability at various distance from the nucleus . 1.Radial probability distribution curves for S orbital n=1, l= 0. distance from nucleus here A° is called angstrom. the probability of finding of electron in a shell is maximum at distance r=r° (r not) which is 0.529 A° for H atom. diagram shows that probability plot for 2s has(two region of high probability) or (two peaks) separated by node. we conclude that no. of high probability region in S orbital = n no. of node = ( n-1)

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