chem aip art integration PR ject of class.ppt

This Ppt is based on orbitals and it's shapes and other stuffs

1. THE QUANTUM NUMBERS
&
SHAPES OF ORBITALS
CHAPTER # 2
ATOMIC STRUCTURE

2. Team members
•Tharun kumar (roll no:-26)
•Dishaa challani (roll no :-33)
•Gauri (roll no:-34)
•Suhas (roll no:24)

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DRAWBACKS OF BOHR’S
ATOMIC MODEL
•Objections were being made on Bohr’s
atomic model about:
–the movement of electrons in 3D space
–spectra of poly electronic atoms.
•Bohr’s atomic model failed to justify
these objections.

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Erwin Rudolf Schrödinger
oIn 1926, Erwin Rudolf
Schrödinger, gave the
idea that of wave
motion of electron
oNobel Prize in Physics
in 1933

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Schrödinger Equation
oHe formulated an equation called “the
Schrödinger equation”, in which
electrons are treated as moving with
wave like motion in 3D space around
the nucleus.
oThe solution of Schrödinger Equation
gave a set of numerical values.

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“The Quantum Numbers”
oExplained the arrangement and
movement of electrons, spectral lines of
poly electronic atoms and gave an
acceptable model of an atom.

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The 4 Quantum Numbers -
An Electron’s
Address
oPrincipal Quantum Number (n)
oSpecifies the main energy level (orbit)
oAzimuthal Quantum Number (l)
oInformation about the sub energy level
(orbital)
oMagnetic Quantum Number (m)
oSpatial orientations of an orbital
oSpic Quantum Number (s)
oSpin movement of electrons

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Principal Quantum Number
(n)
oSize & Energy of an
orbit/shell
on=1, 2, 3, 4,….
oGreater value of n
represents Bigger
orbits with high
energies
oDistance from the
nucleus also increases.

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Principle Quantum Number
(n)
Total No. of Electrons in an orbit = 2n
2
Value of n
Name of
Shell
Total No. of
Electrons 2n
2
n=1 K 2(1)
2
= 2
n=2 L 2(2)
2
= 8
n=3 M 2(3)
2
= 18
n=4 N 2(4)
2
= 32

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Azimuthal Quantum Number
(l)
oEach energy level is divided into sub
levels.
ol defines the shape of sub energy
level/orbital
l
Sub
level
Name
No. of
electrons
0 s Sharp 2
1 p Principal 6
2 d Diffused 10
3 f Fundamental 14

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Relationship between n & l
l = 0  (n-1)
Orbit n l Orbitals
No. of
electrons
K 1 0 1s 2
L 2 0, 1 2s, 2p 2+6 = 8
M 3 0, 1, 23s, 3p, 3d 2+6+10= 18
N 4 0, 1, 2, 3
4s, 4p, 4d,
4f
2+6+10+14=32

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n=1 , K shell
n=2 , L shell
n=3 , M shell
n=4 , N shell
1s (2 electrons)
2s (2 electrons)
2p (6 electrons)
3s (2 electrons)
3p (6 electrons)
3d (10 electrons)
4s (2 electrons)
4p (6 electrons)
4d (10 electrons)
4f (14 electrons)
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Magnetic Quantum Number
(m)
oExplains the effect of an orbital in
magnetic field i.e. the orientation of an
orbital
oOrbitals split up into degenerate
orbitals (having same energy & size) in
a magnetic field
oEach degenerate orbital can hold up to
2 electrons

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Relationship between l & m
m = -l  0  +l
l m
Degenerate
orbitals
No. of
electrons
l = 0, s 0 1 2
l = 1, p-1, 0, +1 3 2+2+2 = 6
l = 2, d
-2, -1, 0, +1,
+2
5
2+2+2+2+2
= 10
l = 3, f
-3, -2, -1, 0,
+1, +2, +3
7
2+2+2+2+2
+2+2 = 14

15. n=1 , K shell
n=2 , L shell
n=3 , M shell
n=4 , N shell
l=0, 1s
l=0, 2s
l=1, 2p
l=0, 3s
l=1, 3p
l=2, 3d
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m=0
m=0
m=0
m=0
m=-
1
m=+
1
m=0
m=-
1
m=+
1
m=0
m=-
1
m=+
1
m=0
m=-
1
m=+
1
m=0
m=-
2
m=+
2
m=-
1
m=+
1
m=0
m=-
2
m=+
2
m=-
1
m=+
1
m=0
m=-
2
m=+
2
m=-
3
m=+
3
l=0, 4s
l=1, 4p
l=2, 4d
l=3, 4f
n l m

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Spin Quantum Number (s)
oDirection of spin of an electron
oElectron which rotates around the
nucleus also rotates around its own axis
oThis is called self rotation
oEither Clockwise (50%) or anticlockwise
(50%)
os = -1/2 ( ) for clockwise
↑
os = +1/2 ( ) for anticlockwise
↓

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Spin of electron
Associated with magnetic field

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Orbital Diagrams
oWe often represent an orbital as a square
and the electrons in that orbital as arrows.
oThe direction of the arrow represents the spin
of the electron.
Orbital with
1 electron
Unoccupied
orbital
Orbital with
2 electrons

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1s
2
2s
2
3s
2
4s
2
2p
6
3p
6
4p
6
3d
10
4d
10
4f
14
K shell
N shell
M shell
L shell

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Orbit
oThe circular path of
an electron around
the nucleus is
called an orbit.
oThe orbit or shells
are denoted by K, L,
M, N etc

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Electron Cloud
A cloud showing
the probability of
finding the
electron in terms
of charged cloud
around the
nucleus is called
Electron Cloud.

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Atomic Orbitals: s, p, d, f
oAtomic orbitals are regions of space
where the probability of finding an
electron about an atom is highest.
os orbital spherical shape
op orbital dumb-bell shape
od orbital clover leaf shape
of orbital double clover leaf

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s orbital - spherically symmetric
l= 0 and m = 0

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p orbital - dumbbell shaped
l = 1m = -1,0,+1

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d orbital shapes
l= 2m = -2,-1,0,+1,+2

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f orbital shapes
 = 3 m
= -3,-2,-1,0,+1,+2, +3

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The End