CHEM 1300 Lecture Notes - Lecture 4: Principal Quantum Number
Lecture 4 – Quantum Numbers
The combination of the quantum numbers are arranged in a way that acts like an address to find the
potential position of an e- with a probability of 90% (there is always a 10% chance that the position is
incorrect or somewhere else)
Symbols:
1. Psi
2. Lambda
3. m sub-lambda
4. axes (x,y,z)
5. n = principle quantum number (orbital)
a. positive integer
b. gives the energy level (e1, e2, etc..)
c. gives relationship to size and stability of the atom
c.i. a higher n will be less stable (more reactive) but have a higher energy and be
larger
c.ii. a lower n will be more stable but have lower energy
c.iii. n also gives the radius of the atom (distance of e- from nucleus) and therefore
the size of the atom
c.iv. also known as the principle level or shell
c.v. note Schrödinger’s equation to solve for n
c.vi. n = (-2.18x10-18J)/n2 can also be used to solve
note: when you see these symbols you know it’s an orbital probability question
Azimuthal Quantum Number ( )
●shape of the atom
●sub-level, or sub-shell
●orbital angular momentum quantum number is the direct translation
●positive whole # less than n
o0-1
oDependent on atom in equation
o10% chance uncertainty
oS,p,d,f orbital shapes
▪1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4d, 5s, 5p, 5d, 5f
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