Download 3 section 4.2

How is an electron able to change
energy levels?
Day 1 1-7
Objective /
Essential Question
How do we define / describe an
electron’s location in the atom?
Notes
Revisiting
the
Electron
Cloud
Page 7
Electron Position:
probability
orbitals
uncertainty
Electron Distribution
element
Properties of
How can the whereabouts of an
electron compare to an
apartment building?
Floor/story of
building
Energy level
Sublevel
Suite/apartment
Orbital for e- couple
Bedroom
Spin
Female / Male
The Address of the Electrons
Just like people in an apartment, electrons have an
address. The most probable location of an electron is
described using quantum numbers. Each electron has
4 quantum numbers which each relays a different
piece of information about the electron’s possible
whereabouts in the atom.
The Address of the Electrons
Pauli exclusion- no 2 electrons
can have the same address!!! –
same 4 quantum numbers
Describing Atomic Structure
Energy level – regions of space
where there is a high probability of
finding electrons
Energy levels - break into -
Sublevels - break into Orbitals
Describing Atomic Structure
Sublevels
3
2
1
First sublevel –
2 electrons
Second sublevel
– 6 electrons
Third
sublevel – 10
electrons
Describing Atomic Structure
– Building an Address
Energy levels – designated by - #
1st Level = 1, 2nd Level = 2, etc. …
Sublevels – designated by – letter
(s, p, d, f) 1st Sublevel = s
2nd Sublevel = p
3rd Sublevel = d
4th Sublevel = f
Describing Atomic Structure
# of energy level = # of sublevels
in that energy level
Energy level 1 = 1 sublevel
Energy level 2 = 2 sublevels
Energy level 3 = 3 sublevels
…
Describing Atomic Structure
E n e r g y
Sublevels
f
d
p
s
Energy still Increases away from the nucleus
Day 2 1-8
1. Why is it impossible to
determine the speed and
location of an electron at the
same time?
The New Atom?
Do you think Bohr was
right or wrong?
Pauli exclusion?
Energy levels - break into Sublevels - break into -
Orbitals
Electron Arrangement
Energy level
1, sublevel s,
orbital 1s
2
1
3
Energy level 2,
has two
sublevels s and
p, 2s orbital and
2p orbitals
Energy level 3, 3
sublevels s, p, and
d, 3s orbital, 3p
orbitals, and 3d
orbitals
Electron Arrangement
Quantum #s – specify the properties of
atomic orbitals and the properties of
electrons in those orbitals
Principle quantum # (n) – main energy
level = 1, 2, 3…
Angular momentum quantum # (l) –
shape of the orbital = 0, 1, 2… (n-1)
0 = s, 1 = p, 2 = d, 3 = f
Magnetic quantum # (ml) – orientation of
the orbital around the nucleus
Electron Arrangement
Quantum #s – specify the properties of
atomic orbitals and the properties of
electrons in those orbitals
Magnetic quantum # (ml) – orientation of
the orbital around the nucleus
Spin quantum # – indicate the two
possible spin states (+1/2, -1/2)
Electron Arrangement
Energy levels – designated by - # (n
the principle quantum #)
s=0
p=1
d=2
f=3
E n e r g y
Sublevels –
designated by –
letter (s, p, d, f) (l the
angular momentum
quantum #)
Energy still Increases away from the nucleus
Electron Arrangement
How many electrons in an orbital?
2 electrons fit in an orbital one
spinning in the +1/2 orientation and
one spinning in the -1/2 orientation
1. What is an atomic emission
spectra (use your lab handout
if necessary)?
Day 3 1-11
NO ATB today. Sit with your
partner(s) for lab and get out
your lab. Wait for instructions.
Day 5 1-13
LAB
Day 3 111
Day 4 112
Day 6 113
Quantum Theory
Quanta’s Ability:
Light energy hits the electrons in
metal- the light must be powerful
enough.
Electrons in the metal absorb the
energy.
The electrons become excited,
and they jump out of the metal.
Quantum Theory
The electrons become excited,
and they jump out of the metal.
The electrons fall down again, and
create a spark or current.
Examples: The luster of a shiny
metal, Photoelectric cells (solar
power)
Q of the Day
1. How many electrons fit in an
orbital?
 How is their movement
different (from each other)?
Day 1 1-15
Q of the Day
1. How many sig figs:
4020
4020.00
0.004020
Day 2 1-19
Q of the Day
1. There are 4 quantum numbers for
each electron. Each one tells you
something about the electron’s
location within the atom. What do
they tell you?
Energy level, sublevel, orbital, spin
Day 4 1-21
Electron Arrangement
How many orbitals in each sublevel?
s=1
p=3
d=5
f=7
Electron Arrangement
How many sublevels
in each energy level?
1 = _____ (__)
3
2 = _____ (____)
3 = _____ (______)
4 = _____ (__________)
2
1
Electron Arrangement
4
xx xx xx xx
xx xx xx xx xx
3
xx xx xx xx
xx xx xx xx xx
2
xx xx xx xx
d
xx xx xx xx xx xx xx
f
p
1
xx
s
Each x = an electron
Each xx = an orbital
Review
Energy levels  number
Sublevel  letter
s, p, d, f
Taking a Look at Orbitals
S
D
P
Notes Page 10
Taking a Look at Orbitals
Taking a Look at Orbitals
p – orbitals always
occur in 3’s (one for
each dimension)
Q of the Day
1. Get out your electron acrostic
from yesterday. You have 2
minutes to finish!!!
Today’s ATB =
What shape is an s sublevel? What
shape is a p sublevel?
Day 5 1-22
Electron Acrostic
E
L
E
C
T
R
O
N
Electron Arrangement
Recall that atoms like to stay in their
most stable (lowest energy) state.
- Sublevels fill from the nucleus
outward
3
2
1
Electron Arrangement
Recall that atoms like to stay in their
most stable (lowest energy) state =
electron configuration
electron configuration – notation
used to show electron placement
within sublevels
Electron Arrangement
electron configuration – notation
used to show electron placement
within orbitals
electron Configuration for:
Si
1s22s22p63s23p2
C
1s22s22p2
Electron Configurations Practice:
S
1s22s22p63s23p4
F
1s22s22p5
1s22s22p63s23p3
P
http://www.youtube.com/watch?v=Vb6kAxwSWgU
http://www.youtube.com/watch?v=rcKilE9CdaA
The most likely location of an
electron is described by a wave
of probability. This type of wave
is actually a set pattern that
forms a 3-D shape within the
space of the atom. This wave
pattern does not overlap itself
and is known as a standing wave.
http://www.youtube.com/watch?v=-gr7KmTOrx0
http://www.youtube.com/watch?v=3BN5-JSsu_4
http://www.youtube.com/watch?v=18BL7MKjtZM
Define:
quantized
Plank’s constant
wavelength
Bohr
electron cloud model
excited state
radiant energy
electromagnetic radiation
Speed of light
Objective /
Essential Question
How do we define / describe an
electron’s location in the atom?
Quick Talk
Ground state
radiant
energy
Bohr
photon
frequency
Compton
quanta
excited state
continuous
particle or wave
Electron Acrostic
E
L
E
C
T
R
O
N
Electron Acrostic
E
L
E
C
T
R
O
N
Element
Mn
C
Electron Configuration
Noble Gas
Notation
# of Valence
electrons