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Find a seat in which you can learn distraction free• Be ready for the quiz

10/30/2018

1. Housekeeping •Rules, Door, Attention signal

2. Quizzes beginning of class• Must be on time to class – No Excuses; tardies

• Excused ABSENCE? Take it afterschool

3. Class Policies• Journals:

• Pages attached, orderly, due on test day, Review sheet

Date Title Page #

History of The Atom 29

History IP 30

2 Book Learning Assignments 31

Book Learning 32

Book Learning 33

Parts of the Atom IP 34

Parts of the Atoms Notes 35

Book Learning 36

Book Learning 37

Todays Date Bohr Model IP 38

Todays Date Bohr & Light Emission Notes 39

ANNOUNCEMENTS!

Quiz Today

10/30/2018

10 minutes

1. Draw a Bohr Model of Nitrogen

2. Draw a Bohr Model of Nitrogen’s Isotope: N- 16

ObjectivesSWBAT explain the relationship between energy and frequency.SWBAT predict the behavior of and/or calculate quantum and photon energy from

frequency.SWBAT explain how the quantization of energy of an atom relates to the

electromagnetic (EM) spectrum.SWBAT identify and describe the different aspects and electromagnetic radiation of

the EM spectrum.SWBAT use the EM spectrum to calculate wavelength, frequency, and/or energy.SWBAT explain the relationship between energy and frequency; and predict the

behavior of and/or calculate quantum and photon energy from frequency.

Essential QuestionHow does the emission spectrum of atoms provide insight into the structure of an atom?

5 minutes

Use the space on your guided notes or add to history ofthe atom notes:

1. What did Milikin discover?

2. What did the x-rays produce when they struck the oildroplets?

3. How did droplets with a negative charge act?

BELL RINGER (copy questions)

Remember

1. These are your notes

2. They can be used to study for your test

3. Your grade, reflects how much of the material you mastered

4. Write what you see and/or hear on the slide, where you see fit

Ownership of learning & your grade

10/30/2018

The current atom

Electrons “-”

Protons “+”

Neutrons “0”

+

+

+0

0

0

0

Bohr’s Model

•Bohr studied the light produced when atoms were excited by heat or electricity.

•Rutherford's model couldn't explain why unique colors were obtained by atoms of different elements.

Bohr’s Model

•Electrons orbit the nucleus like planets orbit the sun.

•Bohr proposed that electrons are in orbits & when excited jump to a higher orbit. When they fall back to the original they give off light.

10/30/2018

Lower energy level

Higher energy level

Bohr’s Model• The electrons in the outermost shell (ring) are

called valence electrons

• The shell containing electrons that is furthest from the nucleus is called the valence shell

+The number of electron shells is the same as the period number

+The number of valence electrons is the same as the group number

Bohr’s Model• Each electron shell (ring) can hold a certain

number of electrons

• Electron shells are filled from the inside out

+ Noble Gases have full outer electron shells

Argon (Ar)“Noble Gas”

10/30/2018

USE THE PERIODIC TABLE TO CREATE YOUR BOHR MODEL!• Protons, neutrons, electrons• Rings (energy shells)• How you should “fill up” each ring• Valence electrons

CFU #1: Carbon •Total electrons

•How many on ring 1?

•How many on ring 2 (valence)?

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CFU #1: Neon •Total electrons

•How many on ring 1?

•How many on ring 2 (valence)?

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BONUS: Bromine (Br)

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BONUS: Xenon (Xe) • Total electrons

• How many on ring 1?




• How many on ring 5 (valence)?

Non- METALS

METALS

1 2 GROUPS “valence electrons” 3 4 5 6 7 8

1. Sulfur (S)2. Fluorine (F)

3. Aluminum (Al)

HOW MANY VALENCE ELECTRONS?

KEY

CFU #3

Non- METALS

METALS

1. Sulfur (S)2. Fluorine (F)

3. Aluminum (Al)

1

2

3

4

5

SHELLS

HOW MANY SHELLS (RINGS)?

KEY

CFU #2

CFU!

Non- METALS

METALS

1 2 GROUPS “valence electrons” 3 4 5 6 7 8

1

2

3

4

5

SHELLS

CFU!

Which element has 18 valence electrons, 4 shells?CFU!

Which element has 2 valence electrons, 5 shells?CFU! e

Which element has 5 valence electrons, 3 shells?

BONUS

Drawing Bohr Models

1. Draw the nucleus.

2. Write the number of neutrons and the number of protons in the nucleus.

3. Draw the first energy level.

4. Draw the electrons in the energy levels according to the rules below. Make sure you draw the electrons in pairs.

5. Keep track of how many electrons are put in each level and the number of electrons left to use.

You must fill one level before going on to draw the next level!

Guided Practice

• Protons: _____ Neutrons: _____ Electrons: ______

• How many energy shells will this have? ____

• How many valence (outer) electrons does this element

have? ____

• Bohr Model:

11

Na

Sodium

22.990

11 12 113

1

Guided Practice




have? ____

• Bohr Model:

15

PPhosphorous

30.974

15 16 153

5

Guided Practice




have? ____

• Bohr Model:

6

C

Carbon

12.011

6 6 62

4

How is light absorbed and emitted by atoms in interstellar gases or stars?

10/30/2018

MODELS OF LIGHT

LIGHT IS A WAVE LIGHT IS A PARTICLE

So which one is right?

They are both right...and they are both wrong.That’s called W A V E - P A R T I C L E duality

•In some experiments, the wave model works best.•In other experiments, the particle model works best.•Thus, we use both.

10/30/2018

Wavelength vs. Frequency

Wavelength ()

the distance between successive crests of a wave, especially points in a sound wave or electromagnetic wave.

Frequency (f)

the rate at which a vibration occurs that constitutes a wave, either in a material (as in sound waves), or in an electromagnetic field (as in radio waves and light), usually measured per second.

Inverse Relationship

10/30/2018

Light comes in many wavelengths

• When white light passes through a glass prism (or a diffraction grating), it separates into colors.

• These colors have different wavelengths.

• This group of wavelengths is the visible part of the electromagnetic spectrum.

• When you “see” the entire spectrum with no thin dark bands, it is a continuous spectrum.

10/30/2018

Electromagnetic Spectrum

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Add colors to this portion:

• Energy• Frequency • wavelength

Check for Understanding

1. What is the wavelength range for the visible light spectrum?

2. Which color of light has a longer wavelength purple or red?

3. Suppose that a certain medical treatment requires exposing certain tissues to high frequency radiation. Would that radiation likely be gamma rays or radio waves?

10/30/2018

Light is a PARTICLE small region of space

• Albert Einstein proposed that light consisted of photons.

• A photon is a “particle” or “packet” of energy according to Max Planck

• High frequency (low wavelength) photons have high energy; low frequency (high wavelength) photons have low energy.

10/30/2018

Bohr Model

• The Bohr model is a planetary model, where the electron orbits the nucleus like a planet orbits the Sun.

• An electron is only allowed in DISCRETE orbits (n=1, n=2, n=3, etc.)

• The higher the orbit, the higher the energy of the electron.

10/30/2018

Absorption, Emission, and Energy

• When an atom absorbs a photon, it gains energy.

• When an atom loses energy, it emits a photon.

• An atom can only absorb photons or emit photons of “specific” energy.

• Those “right energies” correspond to the DIFFERENCES in energy between the allowed energy levels.

Absorption

photon

Emission

photon

10/30/2018

Hydrogen Energy Spectrum

-13.6 eV

-3.40 eV

-1.51 eV

-0.850 eV

-0.544 eVn=5n=4n=3

n=2

n=1

Energy Level Energy • Only certain energies are allowed

• The change in the energy between two levels corresponds to a certain color photon absorbed or emitted by the atom.

• The lowest energy level is the ground state.

• Higher energy levels are called excited states.

10/30/2018

ground

excited

Absorption Spectrum

• If light of a continuous spectrum is incident on a gas of hydrogen atoms, then electrons will absorb some of the light.

• As a result, bands of the spectrum are missing; these are called absorption lines.

10/30/2018

Emission Spectrum• If excited

hydrogen atoms fall to lower energy states, photons will be emitted.

• The emitted photons will be detected as light of certain bands of frequencies (i.e. colors).

• The collection of bands (or lines) forms an emission spectrum.

10/30/2018


-13.6 eV

-3.40 eV

-1.51 eV

-0.850 eV-0.544 eVn=5

n=4n=3

n=2

n=1

Energy Level Energy

1. If an atom is in the ground state(n=1) and is excited to n=3, whatenergy photon was absorbed?

2. If a hydrogen atom is in thestate n=4, to what level must it“fall” in order to emit a bluephoton?

10/30/2018

Independent Practicepage 30

page 34page 38

Notebook

Page

READ Checking Up Chem 2 Go

31113-116 1-4 1-3

652-655 1,2,3,5,6 1-5

32 123-126 1-3 1-8

33 144-148 1-5 1-7

36 133-136 1-7 1,2,4,7,8,9,11

37 176-182 1-7 1-10

BOOK LEARNING

Sign Tutoring log in Chem binder if you need more help

Quiz Today

10/30/2018

15 minutes

Come in and sit beside your lab partner. Check the list on the wall if you forgot who your partner is.


2. Quizzes beginning of class• Must be on time to class – No Excuses; tardies

• Excused ABSENCE, tardy? Take it afterschool

3. Class Policies• Journals:

• Pages attached, orderly, due on test day, Review sheets

4. Finishing Data Chats

Date Title Page #


History IP 30


Book Learning 32

Book Learning 33



Book Learning 36

Book Learning 37

Bohr Model IP 38

Bohr & Light Emission Notes 39

Todays Date Absorption/Emission Lab 40

Unit 2 review 41

ANNOUNCEMENTS!

refresher1. Giving an atom energy (photon) causes what to happen?

2. Explain Milikin’s oil drop experiment. What did he discover?

3. Name the 3 subatomic particles, their charge, and location.

4. List some atomic characteristics that the periodic table can demonstrate.

5. What is the difference between a valence electron and an electron?

6. What is a valence shell?

7. What are some terms we can use to describe light?

8. Describe the frequency and wavelength of Red light? Blue light?

9. Compare electrons and their orbital placement to the energy they have.

10. When white light passes through a prism, what should you expect to see?

11. Below are two spectrums. Which is represents Absorption , which represents Emission.

15 minutesAdd to notes, highlight, write, listen.. Choose wisely

Absorption Spectrum

• If light of a continuous spectrum is incident on a gas of hydrogen atoms, then electrons will absorb some of the light.

• As a result, bands of the spectrum are missing; these are called absorption lines.

10/30/2018

Emission Spectrum• If excited

hydrogen atoms fall to lower energy states, photons will be emitted.

• The emitted photons will be detected as light of certain bands of frequencies (i.e. colors).

• The collection of bands (or lines) forms an emission spectrum.

10/30/2018


10/30/2018

-13.6 eV

-3.40 eV

-1.51 eV

-0.850 eV-0.544 eVn=5

n=4n=3

n=2

n=1

Energy Level Energy

1. If an atom is in the ground state(n=1) and is excited to n=3, whatenergy photon was absorbed?

2. If a hydrogen atom is in thestate n=4, to what level must it“fall” in order to emit a bluephoton?

Pg.39

Independent Practicepage 30

page 34page 38

Notebook

Page

READ Checking Up Chem 2 Go

31113-116 1-4 1-3

652-655 1,2,3,5,6 1-5

32 123-126 1-3 1-8

33 144-148 1-5 1-7

36 133-136 1-7 1,2,4,7,8,9,11

37 176-182 1-7 1-10

BOOK LEARNING

Sign Tutoring log in Chem binder if you need more help


2. TEST NEXT CLASS Journals due

• Pages attached, orderly, due on test day, Review sheets

Date Title Page #


History IP 30


Book Learning 32

Book Learning 33



Book Learning 36

Book Learning 37

Bohr Model IP 38


Absorption/Emission Lab 40

Todays Date Unit 2 review 41

ANNOUNCEMENTS!

Day of Test:

Journals are DUE & ready to be submitted*?*• Pages attached• In order (correct assignments on correct pages)• Review sheet completed

Absent? Provide documentation of excused absence

Tutoring? Fill out tutoring log in binder

HIGH EXPECTATIONS, NO EXCUSESwww.kinga2.weebly.com

10/30/2018

http://www.kinga2.weebly.com/

Unit 2 Review Due Test Day .• List each scientist & their contribution (including

Millikan)• Know Max Planck’s contribution• Know Daltons 5 postulates

• Illustrate and explain both Cathode Ray & Gold foil experiment.• Name the scientist and their discovery

• Know how to calculate proton, neutrons, and electrons• Including Isotopes

• Know all subatomic particles of the atom & their charges

• Know how to draw a Bohr Model

• Know how to determine energy levels and valence electrons using the PT

• Know: what a photon is and what electrons do when energy is absorbed

• Know: what light is, order energies on EM spectrum

Title Page #


History IP 30


Book Learning 32

Book Learning 33



Book Learning 36

Book Learning 37

Bohr Model IP 38


Absorption/Emission Lab 40

Unit 2 review 41

Spot check, last 20 min of class

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