unit 3 the atom & light

Unit 3The Atom &

Light

Today…• Turn in:–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

Block A B C D F Ave High Score

1 6 8 6 2 0 83.23 97

2 6 7 4 3 2 79.25 97.5

4 10 6 4 5 0 83.84 100

7 7 7 11 1 1 81.39 98

TOTAL 31% 29% 26% 11% 3%

Crash Course Video – The Atom

• http://www.youtube.com/watch?v=FSyAehMdpyI

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/animations/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=yQP4UJhNn0I

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/HS-Science-Mass-Practice-VHS_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

SublevelsEnergy 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

Types

s 1

p 3

d 5

f 7

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

ElectronsSublevel # 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=8ROHpZ0A70I

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.html

• 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?

1s22s22p63s23p64s1

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.leidenuniv.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.

Examples1. Magnesium

2. Iodine

Try it Out!

1.Carbon• [He]2s22p2

2.Iron• [Ar] 4s23d6

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=rcKilE9CdaA

• 4:16 – 7:33

Review – Which element? (p. 11)

1. 1s22s22p63s2

2. 1s22s22p63s23p64s23d8

3. 1s22s22p63s23p64s23d9

4. [Ar]4s23d4

5. Write Lead (noble gas notation)

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=fAVPRDnzSpE

• https://www.youtube.com/watch?v=P3ABix1LJAI

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 wavelength of 5.00 x 10-8 m?

• (6.00 x 1015 s-1)

Properties of Light

•Electromagnetic Spectrum - made up of all the forms of electromagnetic radiation

Electromagnetic Spectrum• 7 types of Electromagnetic Radiation1. Gamma Rays 2. X-Rays3. Ultraviolet Light4. Visible Light 5. Infrared Radiation6. Microwaves7. 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 = hνE=Energy

ν= frequencyh= Planck’s Constant = 6.626 x 10-34 J·s

Energy and Frequency

E = hν

High ν = High ELow 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/.../publications/ tnl/35/light3.html

Continuous Spectrum

•Continuous Spectrum – emission of a continuous range of frequencies of electromagnetic radiationExample: 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 atomEach 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 atomEach 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=uxzpE7N0B4Y

• 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 & ConstantsE = hν

h= Planck’s Constant = 6.626 x 10-34 J·s

c = λν

c = 2.998 x 108 m/s

Review1. 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=rcKilE9CdaA

Review Formulas & ConstantsE = hν

h= Planck’s Constant = 6.626 x 10-34 J·s

c = λν

c = 2.998 x 108 m/s

Version Problem #1 Problem #2

1 4.11 x 10-23 J 9.52 x 1015 s-1

2 5.43 x 10-19 J 1.39 x 1014 s-1

3 1.46 x 10-21 J 1.09 x 1015 s-1

4 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