Transcript Unit 3 The Atom & Light

Unit 3
The Atom &
Light
• Turn in:
Today…
–Goal Sheet – fill out & turn in
• Our Plan:
–New Calendar
–Inquiry Part 1 (10 minutes) + Video
–Start Part 2
–Wrap Up – Build sulfur online
• Homework (Write in Planner):
–Part 1 must be done by next class
A B C D F
Ave
High
Score
1 6 8 6 2 0
2 6 7 4 3 2
4 10 6 4 5 0
83.23
97
79.25
97.5
83.84
100
7 7 7 11 1 1
81.39
98
Block
TOTAL
31%
29%
26%
11%
3%
Crash Course Video – The Atom
• http://www.youtube.com/watch?v=FSyAeh
MdpyI
Work Time
• Complete Part 1 individually
and begin Part 2 as a team.
Have Mrs. C check at each
appropriate spot. Part 1 is
due at the beginning of next
class.
POGIL Jobs
• Leader – In charge of the group, reads the
questions, summarizes what should be
written
• Task Master – Makes sure the group is on
task and keeps track of time
• Quality Control – Makes sure that
everyone has close to the same answers
recorded
• Motivator – encourages the group and
makes sure that everyone is participating
and that all ideas are heard
Wrap Up – Exit Ticket
• Go to the website
www.kscience.co.uk/ani
mations/atom.htm and
build a Sulfur atom.
Show it to Mrs. C.
Today…
• As you come in:
– Get a notebooklet and worksheet packet
• Our Plan:
– TED Video
– Review – Find Someone Who
– Inquiry Part 2 & 3
– Wrap Up – Online Exit Ticket
• Homework (Write in Planner):
– Finish Inquiry Packet
…
TED Video Review
• https://www.youtube.com/watch?v=yQP4U
JhNn0I
Find Someone Who
• Move around the classroom and
find students who can answer the
questions on p. 2 of your
notebooklet. Be sure to get their
signature or initials.
POGIL Jobs
• Leader – In charge of the group, reads the
questions, summarizes what should be
written
• Task Master – Makes sure the group is on
task and keeps track of time
• Quality Control – Makes sure that
everyone has close to the same answers
recorded
• Motivator – encourages the group and
makes sure that everyone is participating
and that all ideas are heard
Wrap Up
• Clicker Review
• OR
• http://www.learningliftoff.com/wp-content/uploads/2014/05/HSScience-Mass-PracticeVHS_CHEM_S1_02_03_108_atomic_number_mass_practice.swf
Today…
• Turn in:
– Guided Inquiry Packet
– Have your area clear except for WS Packet &
something to write with
• Our Plan:
– Hog Hilton
– Notes – orbitals & electron configurations
– Online Orbital Activity
– Electron Configurations
– Worksheet #1
• Homework (Write in Planner):
– Worksheet #1
Bohr
• He said that electrons
travel around the atom in
defined orbits or energy
levels
• The energy levels are
like rungs of a ladder
Bohr’s Model
Schrödinger
• He developed the modern
theory of the atom
• Came up with mathematical
equations to predict the
locations of electrons
• Quantum mechanical model –
based on probability
Analogy – p.130
• Similar to the motion of a rotating
propeller blade.
–Cannot tell its precise location
at any instant (The Heisenberg
Uncertainty Principle)
–The cloud is more dense where
the probability of finding an
electron is high
Atomic Orbitals
• Electrons are found in
energy sublevels (atomic
orbitals)
• The sublevel
corresponds to an orbital
of a different shape
Atomic Orbitals
• Orbitals are located inside
energy levels just like
subdivisions are located
inside cities.
Orbitals
•Region of space in
which there is a high
probability of finding
an electron
Sublevels
Energy Level
Names of sublevels that
exist in the energy level
1st Energy Level
s
2nd Energy Level
s and p
3rd Energy Level
s, p, and d
4th & 5th Energy Level
s, p, d, and f
Label Your PT
Sublevel
# of Types of
Orbitals
Possible
s
1
p
3
d
5
f
7
Types
Orbitals
• Only 2 electrons can fit in each
orbital.
• That means that any s orbital can
only hold 2 electrons, and any d
orbital can only hold 2 electrons
• Since there are 5 d orbitals, it can
hold 10 electrons total
Electrons
Sublevel
# of Electrons
s
2
p
6
d
10
f
14
Label Your PT
Quantum Number
•Indicates the
probable location of
an electron in an
atom
•LIKE AN ADDRESS!
Principle Quantum
Number
• Symbol = n
• Indicates – energy level
• Possible Values – 1-7
• STATE
Orbital Quantum #
• Indicates – sublevel
(orbital shape)
• Possible Values – s, p, d, f
• CITY
Magnetic Quantum
Number
• Indicates – the orientation in
space of an orbital of a
given energy and shape
(which room is it in)
• STREET
Spin Quantum Number
• Indicates – 2 possible spin
states
• Possible Values – Clockwise,
Counterclockwise
• HOUSE NUMBER
TED Video – uncertain location
of electrons
• https://www.youtube.com/watch?v=8ROH
pZ0A70I
Break Time!
• Do the front of WS#1
through problem 7.
Break Time
• Get out your chromebook and go
to
http://www.learner.org/interactives
/periodic/elementary_interactive.h
tml
• Complete all four elements listed
and show Mrs. C when you are
done.
Challenge
• This is the electron
configuration for potassium.
What do you think each
number and letter means?
2
2
6
2
6
1
1s 2s 2p 3s 3p 4s
The Blocks of the PT
The Blocks of the PT
• Whichever block an element is in
corresponds to the orbital that
it’s valence electrons are
located.
• Valence electrons are the
outermost electrons in an atom
Electron Configuration
•Shows how many
electrons an atom has
in each of its
sublevels.
Remember
• s holds 2 electrons
• p holds 6 electrons
• d holds 10 electrons
• f holds 14 electrons
Aufbau Principle
• An electron occupies the
lowest energy level that is
available
• Additional electrons keep
“building up” to new
levels
Hund’s Rule
• Every orbital in a subshell is
singly occupied with one
electron before any one
orbital is doubly occupied,
and all electrons in singly
occupied orbitals have the
same spin.
•
http://www.strw.leide
nuniv.nl/~thi/lecture3/
aufbau4.gif
Hund’s Rule
•
library.tedankara.k12.tr/ carey/ch1-1depth.html
Electron Configurations
• All of these principles allow
us to write an electron
configuration for each
element
• Electron configurations
show the location of each of
an atoms’ electrons.
Examples
•Oxygen
Examples
•Potassium
Examples
•Bromine
Try it Out!
• Lithium
–1s22s1
• Sulfur
–1s22s22p63s23p4
• Cobalt
–1s22s22p63s23p64s23d7
Noble Gas Notation
• Instead of writing the
whole electron
configuration, you can
just write the ones since
the nearest noble gas.
Examples
1. Magnesium
2. Iodine
Try it Out!
1.Carbon
2
2
• [He]2s 2p
2.Iron
2
6
• [Ar] 4s 3d
Let’s take a break to visualize
what’s going on in the atom…
• Go to the website
http://keithcom.com/atoms/ and watch
what happens as you add electrons. Be
prepared to describe/explain what you see.
Want to try the f orbital?
• The first f orbital is the 4f,
the second is the 5f (one
number behind the d orbital)
• You say the f before you
say the d orbital (just like it
fits in on the periodic table).
Example
• Bismuth
• Uranium
•Do you feel
smart yet?
STOP!
• Complete Worksheet #1
by next class
Wrap Up – Exit Ticket (p. 9)
• Identify the Element:
1. 1s22s22p63s23p4
2. 1s22s22p63s23p64s23d3
3. 1s22s22p63s23p64s23d104p2
4. [Ar]4s23d6
Today…
• Turn in:
– Get out WS #1 to Check
• Our Plan:
– Crash Course Clip
– Review + Try It Out from Notes
– Quiz – WS#1
– Notes – Light, Wavelength, & Spectra
– Worksheet #2
– Wrap Up – Wintergreen Video
• Homework (Write in Planner):
– WS#2 – due next class
Crash Course Review
• http://www.youtube.com/watch?v=rcKilE9
CdaA
• 4:16 – 7:33
Review – Which element? (p. 11)
1. 1s22s22p63s2
2. 1s22s22p63s23p64s23d8
5. Write Lead
(noble gas
notation)
3. 1s22s22p63s23p64s23d9
4. [Ar]4s23d4
6. Write Krypton
(long form)
Review– Battleship
• Obtain a Battleship board and a dry erase marker. On the bottom
section, mark where you want to put your ships by blocking out
boxes on the Periodic Table.
–
–
–
–
–
Destroyer – 4 Blocks
Carrier – 5 Blocks
Submarine – 3 Blocks
Patrol Boat - 2 Blocks
Battleship - 3 Blocks
• Try to guess where your partner has placed their boats by
asking them energy level, orbital, and how many electrons.
For example, you might say 5s2. Your partner will say hit or
miss. Play alternates and you continue until all ships are
sunk.
Quiz Time!
Daily Challenge
• What are the 6 types of
radiation that make up
the electromagnetic
spectrum?
Properties of Light
•Light behaves as
both a PARTICLE
and a WAVE.
•This is known as a
duality.
Wave Particle Duality Explained
• https://www.youtube.com/watch?v=fAVPR
DnzSpE
• https://www.youtube.com/watch?v=P3ABi
x1LJAI
Parts of a Wave
Amplitude – height of a wave
Parts of a Wave
Wavelength – distance between
waves from peak to peak or
trough to trough
Parts of a Wave
Frequency – number of waves
in a given unit of time
Formula
• The wavelength and
frequency of light are
inversely proportional to
each other (opposites).
• c = λν
• c = 2.998 x 108 m/s
Important Note
• All wavelengths must be in m to
use the constant, so you may
have to convert.
• Hz and s-1 are the SAME THING
Practice Problem
• Calculate the wavelength of the yellow
light emitted by a sodium lamp if the
frequency of the radiation is 5.10 x 1014Hz.
5.88 x 10-7 m
Try It Out!
• What is the frequency of
radiation with a
-8
wavelength of 5.00 x 10
m?
• (6.00 x 1015 s-1)
Properties of Light
• Electromagnetic
Spectrum - made up of
all the forms of
electromagnetic
radiation
Electromagnetic Spectrum
•
1.
2.
3.
4.
5.
6.
7.
7 types of Electromagnetic Radiation
Gamma Rays
X-Rays
Ultraviolet Light
Visible Light
Infrared Radiation
Microwaves
Radio Waves
Electromagnetic Spectrum
Visible Light
• Visible light is the part of
Ultraviolet Radiation that we
can SEE!
• To remember the colors in
order of increasing
frequency, remember
ROYGBIV!
Visible Light
Frequency vs. Wavelength
geography.uoregon.edu/.../geog101/ lectures/lec01/lec01.htm
E = hν
E=Energy
ν= frequency
h= Planck’s Constant = 6.626 x 10
-34
J·s
Energy and Frequency
E = hν
High ν = High E
Low ν = Low E
High E = dangerous!
Challenge
Which waves are most
dangerous?
http://hyperphysics.phy-astr.gsu.edu/hbase/mod3.html
Sample Problem
• Find the amount of energy given off by a
wave whose frequency is 1.6 x 1012 Hz.
(Remember h = Planck’s constant = 6.626
x 10-34 J·s)
• 1.1 x 10-21 J
Try It Out!
• Find the amount of energy given off by a
wave whose frequency is 3.9 x 1018 Hz.
• 2.6 x 10-15 J
Light as Particles
• Quantum – minimum
amount of energy that can
be lost or gained by an atom
• Each particle of light carries
a quantum of energy. The
particles are called
PHOTONS.
Light Emission
• Ground State – Lowest
energy state of an electron
• Excited State – When an
electron has more energy
than in it’s ground state
Light Emission
• When an excited electron moves
to its ground state it GIVES OFF
ENERGY (IN THE FORM OF
ELECTROMAGNETIC
RADIATION).
• When an electron moves from its
ground state to an excited state it
REQUIRES ENERGY.
Think of it like this..
• The energy levels are like
rungs of a ladder
• When you climb up or down a
ladder, you must step on a rung
(you can’t be between rungs)
• It requires energy to go up the
ladder and gives off energy
when you go down
Light Emission
• The more energy levels the electron
moves, the more energy it emits
(quantum leap)
• The amount of energy is consistent
with the frequency (color) of light that
is given off.
• That’s why different elements give off
different colors of light.
Bohr’s Model of the Atom
www.astrosociety.org/.../publicatio
ns/ tnl/35/light3.html
Continuous Spectrum
• Continuous Spectrum –
emission of a continuous
range of frequencies of
electromagnetic radiation
Example: Rainbows
and White Light
Continuous Spectrum
Did you know?
• White light is a mixture of all
colors of visible light
• When sunlight passes
through raindrops, it is
broken into the colors of the
rainbow
Line Emission Spectra
• Line-emission Spectrum –
bands of light emitted by an
atom
Each element has its own
distinct spectrum
Emission spectrum can be
used to identify unknown
samples
Line Emission Spectrum
Absorption Spectrum
• Bands of light absorbed
by an atom
Each element has its own
distinct spectrum
Absorption spectrum can be
used to identify unknown
samples
Absorption Spectrum
STOP!
• Complete Worksheet #2 – due
next class
Wrap Up
• Wintergreen Commercial from 1990 http://www.youtube.com/watch?v=uxzpE7N
0B4Y
• Why does this work?
Today…
• Turn in:
– Worksheet #2
• Our Plan:
– Review Problems – p. ___ booklet
– Quiz over Light
– Flame Test Lab
– Light My Candy Reading/Activity
– Wrap Up – Lab Analysis
• Homework (Write in Planner):
– Finish Reading
Review Formulas & Constants
E = hν
h= Planck’s Constant = 6.626 x 10-34 J·s
c = λν
c = 2.998 x 108 m/s
Review
1. Find the amount of energy given off
by a wave whose frequency is 3.4 x
1016 s-1. (Remember h = Planck’s
constant = 6.626 x 10-34 J·s)
2.3 x 10-17 J
2. Calculate the wavelength of the
yellow light emitted by a sodium
lamp if the frequency of the radiation
is 8.10 x 1012s-1 3.70 x 10-5 m
Wrap Up
What are some problems with
using a flame test as your only
method for identifying a substance?
Today…
• Turn in:
–Flame Test Lab/Candy Reading
• Our Plan:
–Review – Find Someone Who
–Spectroscopy Reading & Activity
–Wrap Up – Clicker Review
• Homework (Write in Planner):
–Finish Reading/Activity
Find Someone Who
• Move around the classroom and
find students who can answer the
questions on p. 18 of your
notebooklet. Be sure to get their
signature or initials.
Wrap Up
• Clicker Review
Today…
• Turn in:
– Spectroscopy Reading/Activity
• Our Plan:
– Math Review
– Academic Conversations
– Test Review & Work Time
– Wrap Up – Quiz, Quiz, Trade
• Homework (Write in Planner):
– Test Review due next class
– TEST NEXT CLASS PERIOD
Crash Course Review
• https://www.youtube.com/watch?v=rcKilE9
CdaA
Review Formulas & Constants
E = hν
h= Planck’s Constant = 6.626 x 10-34 J·s
c = λν
c = 2.998 x 108 m/s
Version
1
2
3
4
Problem #1 Problem #2
4.11 x 10-23 J
9.52 x 1015 s-1
5.43 x 10-19 J 1.39 x 1014 s-1
1.46 x 10-21 J 1.09 x 1015 s-1
2.78 x 10-24 J 3.68 x 1012 s-1
Wrap Up
• Quiz, Quiz, Trade
Today…
• Turn in:
– Test Review – get out to check
– Missing Work in Basket
• Our Plan:
– Scavenger Hunt
– Hand in Review
– Test
– PT Basics Activity (just make the table)
• Homework (Write in Planner):
– Periodic Table Basics