Define atomic orbital . Explain the shapes of s, p and d orbitals with the help of diagrams.

Explanation

Atomic orbital : The three - dimensional space around the nucleus in an atom where the probability of finding an electron is maximum is called an atomic orbital.
Shapes of s , p and d orbitals : The shapes of the orbitals are the 'angular distribution curves' , obtained as one of the solutions of Schrodinger wave equation
1) Shape of s - orbital :
i) s orbital is spherical in shape.
ii) As the value of principle quantum number increases , size of s orbital increases.
(iii) An 's' orbital no directional property.

2 ) shape of p -orbital : Shape of p-orbital is dumb-bell . There are three p - orbitals They are `p_(x),p_(y) and p_(z)` orbitals . Each orbital has two lobes . These lobes are oriented along their respective axes. Each p-orbital has one nodal plane .
3) shape of d -orbital : d - orbital has double dumb-bell shape . There are five d-orbitals. They are `d_(xy),d_(yz),d_(x^(2)-y^(2)) and d_(z^(2))` . Each d orbital has 4 lobes . In `d_(xy)` orbital , the lobes are placed in -between the x and y axes , similar is the case with other orbitals , `d_(yz) and d_(xz). "In " d_(z^(2))` orbital , two lobes lie along z axis and there is a ring of electron -cloud around the centre. In `d_(x^(2)-y^(2))` orbital , the lobes lie along x and y-axes . Each d orbital has two nodal planes.