# Electron Orbitals and Configurations

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```					Electron Orbitals and
Configurations
Division 2 MST
Directions
 While we go through this PowerPoint, I
will be taking notes on the board

 You should write down what I write on the
board
 You should also have out your periodic
table
Electron Orbitals…
what you need to know
 Electrons orbit the nucleus

 Electrons have energy

 Electrons are arranged in a specific pattern

 Electrons will fill energy levels closest to the
nucleus first, and then fill those further away
ENERGY levels

N=3
 Closest = 1   N=2

N=1

 Next = 2

 Next = 3 ….
ENERGY levels

The only problem with
this model, is that only
the electrons in the s
orbital, circle the
nucleus

So what do the electron orbitals really look like?
Each of the Energy Levels has
different orbitals…
 At Energy level = 1
Only 2
 The only orbital
electrons can
fit in this
s
energy
possible is
level!!!!!
What happens when we have
more than 2 electrons?

 They go to a higher energy level

 At Energy level = 2

 The possible orbitals are   s and p
Energy level = 2
sublevels = s and p

Electrons will fill the S sublevel first
p orbitals
S orbital
What do you notice about p
orbital?
 How many
electrons do
you think the
p orbital
could hold?

Okay, but there are elements with
more than 8 electrons…
 Electrons will then fill Energy level 3
which has 3 possible orbitals…

s
p
d
 How many
electrons do
you think the
d orbitals could
hold?
Electron Configuration
 3 Rules:
 Electrons must occupy the lowest energy
levels FIRST
 An orbital can hold up to 2 electrons, but
they must have opposite spins
 Orbitals of equal energy are each occupied
by 1 electron before others are doubled up.

 Say what?
Let’s take an example
 How many electrons does Carbon have?
 6 electrons
 What would be the first energy level to fill?
N=1
 Now what orbital does the first energy
level have?
s
 How many electrons will fit?
Only 2
 What happens next?
 The N=2 energy level will start to fill
 What are the orbitals in the N=2?
 s and p
 Which one will fill first?
 s….why?
 How many electrons will go into the s orbital?
2
 How many electrons are now left?
2
 Where do they go?
 p orbital
 Our last rule
states that
orbitals of
equal energy
must each be
occupied by
one electron
before others
can double up
 How do we represent this without
using the orbital diagrams?

 Electron Configuration             1s22s22p6
(do you know which element is represented?)

 Orbital Notation
Practice makes perfect!
 Let’s practice some of these….
 Write the electron configuration and orbital
notation for
Helium
 Fluorine
 Chlorine

```
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