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Unit 8

Atomic Theory and Periodicity

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Chemistry Unit 8: Atomic Theory and Bonding

|Assignment |WB Page Number |Score |Out of |

|Podcast 8.1 (CB 1-7) |Online + CB Pages | | |

|Video Clip + Discussion with your teacher: |In Class | | |

|Mindwalk | | | |

|Worksheet A | | | |

|Podcast 8.2 (CB 9-13) |Online + CB Pages | | |

|Black Box Lab |Teacher Handout | |100 |

|Demo: Spectral Tubes + Discussion with Teacher |In Class | | |

|Demo: Let their be light + Discussion with your |In Class | | |

|teacher | | | |

|Take Home Lab: Let their be Light |Pg 7 | |100 |

|Lab: Flame Tests |Pg 8-9 | |100 |

|Worksheet B |Pg 16-17 | | |

|Podcast 8.3 (CB 15-27)—This is a long one |Online + CB Pages | | |

|Lab-Activity: Periodic Trends |Pg 11-12 | |100 |

|Technology Lab |Teacher Handout | |100 |

|Worksheet C |Pg 18 | |100 |

|Worksheet D |Pg 19-20 | | |

|Lab: Model Building |Teacher Handout | |100 |

|Podcast 8.4 (CB 29-35) |Online and CB Pages | | |

|Worksheet E |Pg 21 | | |

|Molecular Modeling Computer Activity |Online: See Teacher | |100 |

|Worksheet F |Pg 22 | | |

|Unit 8 Exam |In Class | |100 |

(You must score 85/100 on all assignments with a number to move to the next unit. For those assignments with a check, you need to do it to the satisfaction of your teacher)

Unit 8: Atomic Theory: Chapter 13-14

Section 13.1: Models of the Atom

|1 |History of the Atomic Theory (pg 361-363) |

| |Read the section: “The Evolution of Atomic Models” and describe—or draw pictures—of the models presented by |

| |Dalton |

| |Thompson |

| |Rutherford |

| |Bohr |

|3 |The Quantum Mechanical Model, Atomic Orbitals (pg 363-366) |

| |Define: Quantum Mechanical Model, Atomic Orbitals |

| |Cut out and paste into your composition book the following: |

| |[pic] |

| |[pic] |

| |[pic] |

Section 13.2: Electron Arrangement in Atoms

|5 |Electron Configurations (pg 367-369) |

| |Summarize Each of the Following: Aufbau Principle, Pauli Exclusion Principle, Hund’s Rule |

| |Place the following Diagram on page 5 of your composition book |

| |[pic] |

|7 |More Electron Configurations (Leave Blank for teacher Notes) |

13.3: Physics and the Quantum Mechanical Model

|9 |Light & the Atomic Spectra (pg 372-375) |

| |Sketch: Figure 13.8 on page 372 |

| |Define: Electromagnetic Radiation, Amplitude, wavelength, frequency |

| |Sketch: Figure 13.10 on page 373 |

| |Sketch: Figure 13.11 on page 374 |

|11 |The Quantum Concept and the Photoelectric Effect (pg 376-378) |

| |Define: photon |

| |Copy: Planck’s Equation: Label all variables and copy down the value and units for Planck’s Constant |

| |Read and Summarize: Read the entire section and summarize what it means for energy to be quantized |

|13 |An Explanation of the Atomic Spectra (pg 379-381) |

| |Sketch: Figure 13.17 on page 380 |

Section 14.2: Periodic Trends

|15 |Atomic Size (pg 398-401) |

| |Define: Atomic Radius |

| |Cut and Paste: (The figure below) |

| |[pic] |

| |Sketch: Figure 14.9 on page 400 |

|17 |Ionization Energy (pg 401-402) |

| |Define: Ionization Energy |

| |Cut and Paste |

| |6[pic] |

|19 |Electronegativity (pg 405-406) |

| |Define: Electronegativity |

| |Cut and Paste |

| |[pic] |

|21 |Valence Electrons (pg 413-414) & Bonding Summary |

| |Sketch: Figure 15.1 on page 414 |

| |Define: Octet rule |

| |Place the following table on page 21 |

| |[pic] |

|23 |Ionic Bonding Summary (pg 419-425) |

| |Sketch: the formation of NaCl found on page 419 |

|25 |Metallic Bonding Summary (pg 427-429) |

| |Sketch: Figure 15.13 on page 427 |

| |Define: malleable, ductile, alloy |

|27 |Covalent Bonding Summary |

| |Leave Blank for teacher notes |

|29 |Lewis Structures |

| |Leave Blank for teacher notes |

|31 |Molecular Shapes |

| |A sheet will be provided for you to paste into page 31 |

|33 |Bond and Molecular Polarity |

| |Leave Blank for teacher notes |

|35 |Intermolecular Forces (pg 463-466) |

| |Define: van der Waals Forces, Dispersion forces, hydrogen bonding |

| |Sketch: Figure 16.23 on page 464 |

Take Home Lab

Parent/Student Experiment

Title: And Then There Was Light....

Subject/Concept: Chemistry - Photon Emission

Purpose:

❑ The purpose of this activity is to observe the emission of photons in your own home! Don’t worry, this happens all the time!

Materials:

❑ several commercial bandage strips (3” x .75” with pull-apart packaging - no strings!)

❑ CURAD™, KING SOOPERS™, OR SAFEWAY™ brands work well

❑ regular Wintergreen LifeSavers™ candies or Wintergreen LifeSavers™ Holes

Procedure:

In an absolutely pitch dark room (bathrooms often work), do the following:

❑ Pull apart the bandage strip packaging with very quick pulls of about a half inch or so. You should see the emission of a small purple photon!

❑ While your partner looks on, crush the wintergreen candy between your teeth and your partner will see the emission of a small photon!

Questions:

1. What is the source of the emitted photon?

2. Make a drawing of the Rutherford-Bohr model of an atom showing the movement of an electron during the process of light emission.

For Credit:

To receive credit, complete the questions for this lab on a separate piece of paper. Also, your parent or guardian must write a short note confirming that you performed the experiment for them and explained the results to their satisfaction using the concept of photon emission and electron energy levels. Attach your note to the back of this sheet.

Flame Test Lab

Chemists began studying colored flames in the 18th century and soon used "flame tests" to distinguish between some elements. Different elements burn with different colored flames. Although some of the flames you will be seeing will appear similar in color, their light can be resolved (separated) with a prism into distinctly different bands of colors on the electromagnetic spectrum (ROYGBIV). These bands of colors are called atomic line spectra, and they are UNIQUE to each element. Niels Bohr studied the line spectrum for hydrogen, and wondered what the specific line spectrum had to do with the structure of the atom. He postulated that an electron can have only specific energy values in an atom, which are called energy levels. Bohr believed that the energy levels for electrons were quantized, meaning that only certain, specific energy levels were possible. How does an electron move between energy levels? By gaining the right amount of energy, an electron can move, or undergo a transition, from one energy level to the next. We can explain the emission of the light by atoms to give the line spectrum like this:

1. An electron in a high energy level (excited state) undergoes a transition to a low energy level (ground state).

2. In this process, the electron loses energy, which is emitted as a photon (a particle which behaves like a wave)

3. The energy difference between the high energy level and the low energy level is related to the frequency (color) of the emitted light.

Pre-lab questions:

1. Bohr's important discovery was that energy levels of electrons are quantized (only existing in certain, specific levels). In what year was this discovery made? _____________

2. What happens to an electron when energy is added?

3. What is released when an electron loses energy?

4. What determines the frequency (color) of photons?

5. Why do you think the frequencies (color) for a specific element is always the same?

Procedure: In this lab, you will be observing the colors of the flames for 7 different elements: lithium, sodium, potassium, calcium, strontium, barium, and copper. Each element is dissolved in a solution of its chloride salt. There is a different solution at each lab station. You will go around to all 7, perform the flame test, and make CAREFUL observations of the colors. You will then be given an unknown solution, for which you will have to use your notes below to determine which unknown you were given.

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Post- Lab Questions:

1. If you had 2 colors that seemed identical, how could you tell them apart more accurately?

2. Albert Einstein determined this equation:

energy (in joules) of a photon is equal to Planck's constant times the frequency of the light:

E = h • ( • Frequency (() has units of 1/sec (which is a Hertz, or Hz)

• Planck's constant (h) = 6.63 x 10-34 J·sec

a) If the frequency of a red spectrum line is at 1.60 x 1014 Hz, how much energy does each photon of this light have?

b) If the frequency of a violet spectrum line is at 2.50 x 1014 Hz, how much energy does each photon of this light have?

c) On the far ends of the visible spectrum of light, there exists ultraviolet (UV) radiation and infrared (IR) radiation.

- UV radiation is dangerous. UV radiation is located just past violet on the spectrum.

• IR radiation is harmless. It is located just past red on the spectrum.

• Based on what you calculated in parts a & b, explain -why- UV is more dangerous than IR:

Molecular Shapes

|“clouds” | | | | | |

|2 |[pic] Linear Triatomic, Usually | |Linear Diatomic | |In molecules where the|

| |nonpolar CO2, HCN | |[pic] | |outside molecules are |

| | | |Polarity depends upon | |different, shapes that|

| | | |electronegativity | |tend to be nonpolar |

| | | |difference | |usually become polar. |

| | | |Polar if >0.5 | | |

| | | |Nonpolar if 0.5 | | |

| | | |Nonpolar if Ionic > Metallic

18. Classify each of the following compounds as either: Ionic, Covalent, Metallic.

a. H2O Covalent

b. NaCl Ionic

c. MgSO4 Ionic

d. CsCl Ionic

e. Fe Metallic

f. Hg Metallic

g. He None

h. Ca3(PO4)2 Ionic

i. NH4Cl Ionic

j. NH3 Covalent

k. P2O5 Covalent

l. Ag Metallic

m. AgNO3 Ionic

n. AgCl Ionic

o. Titanium Metallic

p. Barium Phosphate Ionic

q. Sulfur Dioxide Covalent

r. Bromine Covalent

s. Tungsten V Bromide Ionic

WS E: Lewis Structure Worksheet: Name _________

• Draw the Lewis Structures

• Determine the shape

• Determine the polarity of the molecule

1.HCl

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1. Br2

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2. SeBr2

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3. CF4

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4. PI3

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Pyrimidal

Polar

5. O2

[pic]

6. N2

[pic]

7. H2

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8. OI2

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9. CS2

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Linear Triatomic

Non Polar

10. SiBr4

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11. F2

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12. HCN

[pic]

13. NH4 +

[pic]

Tetrahedral

Non Polar

14. NO2 –

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Bent 120

Polar

15. SO3

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Trigonal Planar

Nonpolar

16. SO42-

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Tetrahedral

Nonpolar

17. NO3-

[pic]

Trigonal Planar

Nonpolar

18. PO33-

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Pyrimidal

Polar

19. CN-

[pic]

Linear Diatomic

Polar

20. CO2

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Linear Triatomic

NonPolar

21. CO

[pic]

Linear Diatomic

Polar

22. I2

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Linear Diatomic

Non Polar

23. CO32-

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Trigonal Planar

Nonpolar

24. SO2

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Bent 120

Polar

25. OCN-

[pic]

Linear Triatomic

Polar

26. SCN-

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Linear Triatomic

Polar

27. O3

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For the following structures: You do NOT have to determine the shapes

28. H3CCOOH

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29. CH3CH2OH

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30. H3COCH3

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31. H3CCH3

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32. H2CCH2

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33. HCCH

WS F: Intermolecular Forces Name _______________

| |Predominant Intermolecular Force| |Predominant Intermolecular Force |Substance with Higher Boiling |

|Substance #1 | |Substance #2 | |Point |

|(a) HCl(g) |Dipole |I2 |LDF |HCl |

|(b) CH3F |Dipole |CH3OH |H-Bond |CH3OH |

|(c) H2O |H-bonding |H2S |Dipole |H2O |

|(d) SiO2 |Covalent Network |SO2 |Dipole |SiO2 |

|(e) Fe |Metallic |Kr |LDF |Fe |

|(f) CH3OH |H-Bond |CuO |Ionic |CuO |

|(g) NH3 |H-Bond |CH4 |LDF |NH3 |

|(h) HCl(g) |Dipole |NaCl |Ionic |NaCl |

|(i) SiC |Covalent Network |Cu |Metallic |SiC |

2. Rank the following substances in order from lowest to highest melting point.

CO2, NaCl, Ag, H2O, He, HBr

He < HBr < H2O < Ag < NaCl

3. Rank the following substances in order from lowest to highest freezing point.

H2O, Ca3(PO4)2, Cr, C2H6, OF2

C2H6 < OF2 < H2O < Cr < Ca3(PO4)2

4. Rank the following substances in order from highest to lowest boiling point.

Cl2, Ne, Ca, Cr(OH)3, CH3CH2OH, Diamond

Diamond > Cr(OH)3 > Ca > CH3CH2OH > Cl2 > Ca

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O

H

H

H

Metallic

Covalent

Ionic

Bonding

C

H

H

H

C

O

O

H

C

H

H

H

C

O

O

O

28.

Bent 120

Nonpolar

1-

N

S

C

27.

1-

N

O

C

26.

O

O

O

C

24.

I

I

C

O

O

O

C

21.

N

C

3-

O

P

O

O

-

O

O

O

N

18.

2-

O

O

O

O

S

17.

O

O

O

S

16.

O

O

N

15.

H

H

H

H

N

14.

N

H

Linear Triatomic

Polar

C

13.

12.

Linear Diatomic

Non Polar

F

F

Br

Br

Br

Br

Tetrahedral

Non Polar

Si

11.

C

S

10.

S

I

Bent 104

Polar

O

I

9.

Linear Diatomic

Non Polar

H

H

8.

Linear Diatomic

Non Polar

N

N

7.

Linear Diatomic

Non Polar

O

O

6.

I

P

5.

I

I

F

F

C

4.

Tetrahedral

Non Polar

F

F

Se

3.

Bent 104.5

Polar

Br

Br

2.

Linear Diatomic

Non Polar

Br

Br

1.

Linear Diatomic

Polar

Cl

H

2p

2s

1s

2p

2s

1s

2p

3s

3p

2s

1s

1s

1s

4p

3d

4s

2p

3s

3p

2s

1s

3d

4s

2p

3s

3p

2s

1s

3d

4s

2p

3s

3p

2s

1s

2p

3s

3p

2s

1s

2p

3s

2s

1s

2p

3s

3p

2s

1s

2p

2s

1s

2ap

3s

3p

2s

1s

2p

2s

1s

4s

2p

3s

3p

2s

1s

2p

3s

2s

1s

2s

1s

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