Classical mechanics successfully describes macroscopic objects but fails for microscopic objects like atoms and molecules. Quantum mechanics was developed to account for these microscopic objects, which exhibit both wave-like and particle-like properties. It describes that electrons can have distinct quantum states defined by quantum numbers like principal (n), azimuthal (l), magnetic (m), and spin (s). The values of these quantum numbers determine properties of atomic orbitals like shape, size, and energy.

1. Made by :-
Name :- Pranav Ghildiyal
Class :- XI B

2.  Classical mechanics, based on Newton’s laws of motion, successfully
describes the motion of all macroscopic which have essentially a
particle-like behaviour However it fails when applied to microscopic
objects like electrons, atoms, molecules etc. This is mainly because of
the fact that classical mechanics ignores the concept of dual behaviour
of matter especially for sub-atomic particles and the uncertainty
principle. The branch of science that takes into account this dual
behaviourof matter is called quantum mechanics.
 Quantum mechanics is a theoretical science that deals with the
study of the motions of the microscopic objects that have both
observable wave like and particle like properties.
 Quantum mechanics was developed independently in 1926 by
Werner Heisenberg and Erwin Schrödinger. The fundamental
equation of quantum mechanics was developed by Schrödinger and
it won him the Nobel Prize in Physics in 1933. This equation which
incorporates waveparticle duality of matter was proposed by de Broglie

3. Types of Quantum NumbersTypes of Quantum Numbers

4.  The principal quantum number ‘n’ is a positive
integer with value of n = 1,2,3... .The principal quantum
number determines the size and to large extent the
energy of the orbital. For hydrogen atom and hydrogen
like species (He + , Li, .... etc.) energy and size of the
orbital depends only on ‘n’. The principal quantum
number also identifies the shell.the increase in the value
of ‘n’, the number of allowed orbital increases and are
given by the following letters .
n = 1 2 3
4
Shell = K L M N .

5.  Size of an orbital increases with increaseofSize of an orbital increases with increaseof
principalprincipal
quantum number ‘quantum number ‘n’.n’. Each shell consists of one orEach shell consists of one or
moremore
sub-shellsor sub-levels. The number of sub-shellsinsub-shellsor sub-levels. The number of sub-shellsin
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principal shell is equal to the value value of n.Forprincipal shell is equal to the value value of n.For
example in the first shell (example in the first shell ( nn = 1), there is only one= 1), there is only one
sub-sub-
shell which corresponds l = 0. Each sub-shell isshell which corresponds l = 0. Each sub-shell is
assigned an azimuthal quantum number. Sub-shellsassigned an azimuthal quantum number. Sub-shells
corresponding to different values ofcorresponding to different values of ll areare
representedrepresented
in the following tablein the following table
Value for l 012345...........
.
notation for sub-
shell
spdf
gh............

6. n L SubShell
notations
1 0 1s
2 0 2s
2 1 2p
3 0 3s
3 1 3p
3 2 3d
4 0 4s
4 1 4p
4 2 4d
4 3 4f

7.  Magnetic orbital quantum number. ‘m’ gives information about the spatial orientation ofMagnetic orbital quantum number. ‘m’ gives information about the spatial orientation of
thethe
orbital with respect to standard set of co-ordinate axis. For any sub-shell (defined by ‘l’orbital with respect to standard set of co-ordinate axis. For any sub-shell (defined by ‘l’
value)value)
2l+1 values of m are possible and these values are given by : m2l+1 values of m are possible and these values are given by : m11 = – l, – (l –1), – (l –2)... 0,1...= – l, – (l –1), – (l –2)... 0,1...
(l – 2), (l–1), l.(l – 2), (l–1), l.
 for l = 0, the only permitted value of mfor l = 0, the only permitted value of mll = 0, [2(0)+1 = 1, one s orbital]. For can be –1, 0 and= 0, [2(0)+1 = 1, one s orbital]. For can be –1, 0 and
+1 [2(1)+1 = 3, three orbitals]. For l = 2, m = –2, –1, 0, +1 and +2, [2(2)+1 = 5, five d orbitals]. It+1 [2(1)+1 = 3, three orbitals]. For l = 2, m = –2, –1, 0, +1 and +2, [2(2)+1 = 5, five d orbitals]. It
should be noted that the values of mshould be noted that the values of mll are derived from that the value of l are derived fromare derived from that the value of l are derived from
n.n.
Value of l 0 1 2 3 4 5
Subshell notation s p d f g h
number of orbitals 1 3 5 7 9 11

8.  In 1925, George Uhlenbeck and Sameul Goudsmit proposed theIn 1925, George Uhlenbeck and Sameul Goudsmit proposed the
presense of the fourth quantum number known as electron spinpresense of the fourth quantum number known as electron spin
quantum number. An electron spins around its own axis, much inquantum number. An electron spins around its own axis, much in
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Similar way as earth spins around its own axis while revolvingSimilar way as earth spins around its own axis while revolving
aroundaround
the sun. Spin angular momentum of the electron — a vectorthe sun. Spin angular momentum of the electron — a vector
quantity,quantity,
can have two orientations relative to the chosen axis. These arecan have two orientations relative to the chosen axis. These are
the twothe two
spin states of the electron and are normally represented by twospin states of the electron and are normally represented by two
arrows, ↑ (spin up) and ↓ (spin down). Two electrons that havearrows, ↑ (spin up) and ↓ (spin down). Two electrons that have
differentdifferent mm values (one+ and the other –) are said to havevalues (one+ and the other –) are said to have
oppositeopposite
spins. An orbital cannot hold more than two electrons and thesespins. An orbital cannot hold more than two electrons and these
twotwo

9.  ‘‘n’ defines the shell, determines the size of the orbital and alson’ defines the shell, determines the size of the orbital and also
to ato a
large extent the energy of the orbitallarge extent the energy of the orbital
 There areThere are n subshells in then subshells in the nnthth shell, ‘l’ identifies the subshellshell, ‘l’ identifies the subshell
andand
determines theshape of the orbital.There are (2determines theshape of the orbital.There are (2 l+1) orbitals ofl+1) orbitals of
eacheach
type in atype in a subshell, that is,onesubshell, that is,one s orbital (l = 0), Three p orbitals (l =s orbital (l = 0), Three p orbitals (l =
1)1)
and five d orbitals (l = 2)and five d orbitals (l = 2) per subshell. To some extent ‘per subshell. To some extent ‘ l’ alsol’ also
determines the energy of the orbital in a multi-electron atom.determines the energy of the orbital in a multi-electron atom.
 MMll designates the orientation of the orbital. For a given value ofdesignates the orientation of the orbital. For a given value of
l,l,
mm has (2has (2l+1)l+1) values, the same as the number of orbitals pervalues, the same as the number of orbitals per

11.  The orbital wave function or ψ for an electron in an
atom has no physical meaning. It is simply a
mathematical function of the coordinates of the
electron. However, for different orbitals the plots of
corresponding wave functions as a function of r (the
distance from the nucleus) are different
According to the German physicist, Max Born, the
square of the wave function (ψ2 ) at a point gives the
probability density of the electron at that point. For
1s orbital the probability density is maximum at the
nucleus and it decreases sharply as we move

12. 1s {n=1, l= 0 } 2s {n=2, l=0}
1s orbitals 2s orbitals

13. For 2p
orbitals
For 2p
orbitals
For 3d
orbitals
For 3d
orbitals

14.  The filling of electrons into the orbitals of different atoms
takes place according to the aufbau principle which is
based on the Pauli’s exclusion principle, the Hund’s rule
Of maximum multiplicity and the relative energies of the
orbitals.

16.  The distribution of electrons into orbitals of an
atom is called its electronic configuration. If one
keeps in mind the basic rules which govern the
filling of different atomic orbitals, the electronic
configurations of different atoms can be written very
easily.