Unit 3 Chemistry: The Electron Flashcards
(31 cards)
How electrons are distributed within an atom:
Electron configurations
Describes the average distance of an electron from the nucleus
Principal energy levels
Correspond to the different areas an electron can be located in an atom:
Sublevels
S sublevel shape
Spherical
P sublevel shape
Dumbbell
D sublevel shape
Clover
F sublevel shape
Double clover
What are sublevels represented by?
Letters: s, p, d, f, g, h…
Each sublevel is oriented differently inv 3-D space and each orientation is called….
An atomic orbital
How many electrons can atomic orbitals hold?
Only 2
What are the principal energy levels?
n= 1, 2, 3, 4, etc.
How many orbitals are in each type of sublevel?
s=1
p=3
d=5
f=7
Electrons enter sublevels with the lowest energy first.
Aufbau Principle
Uses circles to represent atomic orbitals with a label underneath to indicate sublevel and energy level.
Orbital notation
Atomic orbitals can hold only two electrons at most and they must have opposite spin.
Pauli Principle
In a sublevel with more than one orbital, put one electron into each orbital before putting 2e- into any one orbital.
Hund’s rule
Order of energy levels:
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
Electrons that are located in the outermost energy level.
Valence electrons
Used to describe the distribution of electrons in atoms.
Quantum numbers
What does n=
Principal quantum number
What does l=
Angular momentum quantum
What does ml=
Magnetic quantum number
What does ms=
Electron spin quantum number
Described as the average distance of electrons to the nucleus (energy level0
Principal quantum number
