# Electron Quantum NumbersPage 1

#### WATCH ALL SLIDES

Slide 1 ## Electron Orbitals

Cartoon courtesy of lab-initio.com

Slide 2 ## Quantum Mechanical Model of the Atom

Mathematical laws can identify the regions outside of the nucleus where electrons are most likely to be found.

These laws are beyond the scope of this class…

Slide 3 ## Heisenberg Uncertainty Principle

The more certain you are about where the electron is, the less certain you can be about where it is going.

The more certain you are about where the electron is going, the less certain you can be about where it is.

“One cannot simultaneously determine both the position and momentum of an electron.”

Werner

Heisenberg

Slide 4 ## Quantum Numbers

Each electron in an atom has a unique set of 4 quantum numbers which describe it.

Principal quantum number

Angular momentum quantum number

Magnetic quantum number

Spin quantum number

Slide 5 ## Electron Energy Level (Shell)

Generally symbolized by n, it denotes the probable distance of the electron from the nucleus. “n” is also known as the Principle Quantum number

Number of electrons that can fit in a shell:

2n2

Slide 6 ## Electron Orbitals

Orbital shapes are defined as the surface that contains 90% of the total electron probability.

An orbital is a region within an energy level where there is a probability of finding an electron.

The angular momentum quantum number, generally symbolized by l, denotes the orbital (subshell) in which the electron is located.

Slide 7 ## Orbital shape

The s orbital

(l = 0) has a spherical shape centered around

the origin of the three axes in space.

s

Slide 8 There are three dumbbell-shaped p orbitals (l = 1) in each energy level above n = 1, each assigned to its own axis (x, y and z) in space.

p orbital shape

Slide 9 Things get a bit more complicated with the five d orbitals (l = 2) that are found in the d sublevels beginning with n = 3. To remember the shapes, think of “double dumbells”

…and a “dumbell

with a donut”!

d orbital shapes

Slide 10 Go to page:
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