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The 4 Quantum Numbers
1. Principal Quantum Number, n 2. Azimuthal Quantum Number, l 3. Magnetic Quantum Number, ml 4. Spin quantum Number, ms Principle Quantum Number
1. Main energy level of an orbital. 2. Indicates the relative size of the orbital. 3. An increase in n also means increase in the energy of the electron in the orbital. n= 1, 2, 3.... Azimuthal Quantum Number
1. Also called Angular Momentum Number. 2. Defines the shape of orbital. 3. Values ranges from 0 to n - 1. l = n - 1 Azimuthal Quantum Number
l Sublevel Orbital Shape
0 Sharp - s spherical
1 Principal - p Dumbbell - shaped
2 Diffused - d cloverleaf
3 Fundamental Too complex - f Azimuthal Quantum Number Azimuthal Quantum Number
A sublevel in a particular main energy level is defined by its n and its l values.
n l Kind of sublevel
1 0 1s
3 1 3p Magnetic Quantum Number, m l
1. Describes the orientation of the orbital in space. 2. Values are -l to +l 3. Values per sublevel = 2l + 1 Magnetic Quantum Number, m l
sublevel l ml
s 0 0
p 1 -1, 0, + 1
d 2 - 2, -1, 0, 1, + 2
f 3 - 3, - 2, - 1, 0, + 1, + 2, + 3 Sublevel and Capacity of each main energy level
Max. No Main Energy No . of Identity No. of of Level Subleve of Orbitals( Electrons l Sublevels n2) (2n2) 1 1 1s 1 2
2 2 2s 1 2 2p 3 6
3 3 3s 1 2 3p 3 6 3d 5 10
4 4 4s 1 2 4p 3 6 4d 5 10 4f 7 14 Spin Quantum number
The spin quantum number is the fourth quantum number, denoted by s or ms. The spin quantum number indicates the orientation of the intrinsic angular momentum of an electron in an atom.
The only possible values of a spin quantum number are +½ or -½ Pauli’s Exclusion Principle
The Pauli Exclusion Principle states that, in an atom or molecule, no two electrons can have the same four electronic quantum numbers. Example The correct set of quantum number is
A. n=2, l = 1, m = 0, s=0 B. n=2, l = 2, m = -1, s = - 1/2 C. n=2, l = -2, m = 1, s = + 1/2 D. n=2, l = 1, m = 0, s = +1/2 Example The quantum number which explains about size and energy of the orbit or shell is
A. n B. l C. ms D. ml
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