2. The Major Players
• Werner Heisenberg
• Heisenberg Uncertainty Principle
• Electron Density
• Erwin Schrödinger
• Wave functions (Ψ)
• Atomic Orbital
• Quantum Numbers
9. Quantum Numbers
-zip codes for electrons-
4 Types of Quantum #s
1. Principal (n)
• Distance from nucleus
2. Angular Momentum (l)
• Orbital Shape
3. Magnetic (ml)
• Orientation in space
4. Spin (ms)
• Rotational Spin
14. SPIN (ms)
Electron spin ⇒ +½ or -½
–An orbital can hold 2 electrons that
spin in opposite directions.
15. Quantum Numbers
-zip codes for electrons-
4 Types of Quantum #s
1. Principal (n)
• Distance from nucleus
2. Angular Momentum (l)
• Orbital Shape
3. Magnetic (ml)
• Orientation in space
4. Spin (ms)
• Rotational Spin
16. • n = # of sublevels per level
• n2
= # of orbitals per level
• Sublevel sets: 1 s, 3 p, 5 d, 7 f
17. • Orbitals combine to form a spherical
shape, which defines the “electron
cloud.”
2s
2pz
2py
2px
19. Questions
How many orbitals are in the
following sublevels?
3p
2s
4p
3d
4f
3: px, py, pz
1: s
3: px, py, pz
5: dxy, dyz, dxz, dx2-y2, dz2
7: Don’t worry, just know it
20. Questions
How many sublevels are
contained in each of the
following energy levels?
n = 1
n = 2
n = 3
n = 4
1, the s sublevel
2, the s and p sublevels
3, the s, p, and d sublevels
4, the s, p, d, and f sublevels
21. Questions
What is the maximum number of
electrons that can go into each
of the following sublevels?
4s 3p 4s 3d
4p 5s 4f 5p
2e-
6e-
2e-
10e-
6e-
2e-
14e-
6e-
Notas del editor
Werner Heisenberg – tried to locate a subatomic particle that behaves like a wave (Particle Duality). He formulated. . . .
Heisenberg Uncertainty Principle – it is impossible to know simultaneously both the momentum (p = mass *velocity) and position of a particle with any certainty.
Although you don’t know exactly where a wave is, you can explain where you are most likely to find it.
Electron Density – defines the probability of finding an electron in a particular region of an atom.
Erwin Schrödinger – Used complicated math, taking equations from wave motion and particle motion to create wave functions ()
Wave functions () are used to describe the probability of finding an electron around a nucleus.
Atomic orbital – the wave function of an electron in an atom.
This idea gave birth to quantum numbers:
Quantum numbers – describe the distribution of electrons in atoms. There are four
1. Principal (n)
2. Angular Momentum (l)
3. Magnetic (ml)
Spin (ms)
n – describes electron’s distance from the nucleus (as n increases, the e- moves further from the nucleus)
l – describes orbital shape
0 = s
1 = p
2 = d
3 = f
4 = g
ml – describes orientation of orbital in space
what plane: X,Y,orZ
ms – describes rotational spin
Expressed as whole value starting at +1
Describes an electron’s distance from the nucleus
Boundary surface diagram – encloses 90% of the total electron density in an orbital
Possible value = (n-1)
Describes orbital shape.
Describes orientation of orbital in space. That is, what plane: X,Y,Z
Quantum numbers – describe the distribution of electrons in atoms. There are four
1. Principal (n)
2. Angular Momentum (l)
3. Magnetic (ml)
Spin (ms)
n – describes electron’s distance from the nucleus (as n increases, the e- moves further from the nucleus)
l – describes orbital shape
0 = s
1 = p
2 = d
3 = f
4 = g
ml – describes orientation of orbital in space
what plane: X,Y,orZ
ms – describes rotational spin
