Norfolk Public Schools Science Learning in Place Plan: Chemistry Lessons

Week 10: May 18 – 22, 2020 (Unit 10)

Monday Tuesday Wednesday Thursday Friday

Unit 7.10: Experimental

Unit 1.10: Elements and the Periodic Table Unit 2.10: Compounds and Bonding Unit 3.10: Kinetic Theory Unit 4.10: The Mole and Stoichiometry Unit 5.10: Chemical Reactions Unit 6.10: Solutions Unit 7.10: Experimental U10: Mastery Knowledge

Unit 10 Packet pages 9 – 10 Greatest Scientists in Chemistry Unit 10 Practice

Unit 10 Packet page 11 Unit 10 Review Continued

Unit 10 Packet pages 12 – 13 Unit 10 Review

Week 11: May 25 – 29, 2020 (Review Part 1)

Monday Tuesday Wednesday Thursday Friday

Unit 1.10: Elements and the Periodic Table Unit 2.10: Compounds and Bonding Unit 5.10: Chemical

Reactions

Review Packet pages 1 – 2 Review Packet pages 3 – 4 Review Packet page 5

Week 12: June 1 – 5, 2020 (Review Part 2)

Monday Tuesday Wednesday Thursday Friday

Unit 3.10: Kinetic Theory Unit 6.10: Solutions Unit 4.10: The Mole and Stoichiometry

Review Packet pages 6 – 7 Review Packet page 8 Review Packet pages 9 – 10

9

10

11

12

13

Helium

4.00260

Mercury

200.59

Cadmium

112.41

Zinc

65.39

Gold

196.967

Silver

107.868

Copper

63.546

Platinum

195.08

(269?)

Palladium

106.42

Nickel

58.69

Thallium

204.383

Indium

114.82

Gallium

69.72

Lead

207.2

Tin

118.71

Germanium

72.59

Bismuth

208.980

Antimony

121.75

Arsenic

74.9216

Polonium

(209)

Tellurium

127.60

Selenium

78.96

Astatine

(210)

Iodine

126.905

Bromine

79.904

Radon

(222)

Xenon

131.29

Krypton

83.80

Aluminum

26.98154

Silicon

28.0855

Phosphorus

30.97376

Sulfur

32.06

Chlorine

35.453

Argon

39.948

Boron

10.81

Carbon

12.0111

Nitrogen

14.0067

Oxygen

15.9994

Fluorine

18.998403

Neon

20.179

Lutetium

174.967

Lawrencium

18

He2

Rn86

Xe54

Kr36

Ar18

Ne10

Lu71

Lr103

(260)

Ytterbium

173.04

Nobelium

17

At85

I53

Br35

Cl17

F9

Yb70

No102

(259)

Thulium

168.934

Mendelevium

16

Po84

Te52

Se34

S16

O8

Tm69

Md101

(258)

Erbium

167.26

Fermium

15

Bi83

Sb51

As33

P15

N7

Er68

Fm100

(257)

Holmium

164.930

Einsteinium

14

Pb82

Sn50

Ge32

Si14

C6

Ho67

Es99

(252)

Dysprosium

162.50

Californium

13

Tl81

In49

Ga31

Al13

B5

Dy66

Cf98

(251)

Terbium

158.925

Berkelium

12

Hg80

Cd48

Zn30

Tb65

Bk97

(247)

Gadolinium

157.25

Curium

11

Au79

Ag47

Cu29

Gd64

Cm96

(247)

Europium

151.96

Americium

10

Pt78

110

Pd46

Ni28

Eu63

Am95

(243)

Mass numbers in parentheses are those ofthe most stable or most common isotope. Metals Nonmetals

Si

Silicon

14

28.0855Atomic mass

Symbol

Atomic number

Name

Potassium

39.0983

Calcium

40.08

Sodium

22.98977

Magnesium

24.305

Lithium

6.941

Beryllium

9.01218

Hydrogen

1.00794

Scandium

44.9559

Titanium

47.88

Vanadium

50.9415

Chromium

51.996

Manganese

54.9380

Iron

55.847

Cobalt

58.9332

Rubidium

85.4678

Strontium

87.62

Yttrium

88.9059

Zirconium

91.224

Niobium

92.9064

Molybdenum

95.94

Technetium

(98)

Ruthenium

101.07

Cesium

132.905

Barium

137.33

Lanthanum

138.906

Hafnium

178.49

Tantalum

180.948

Tungsten

183.85

Rhenium

186.207

Osmium

190.2

Francium

K19

Na11

Li3

1

H1

Group1

Rb37

Cs55

Fr87

(223)

Radium

Ca20

Mg12

Be4

2

Sr38

Ba56

Ra88

226.025

Actinium

Sc21

3

Y39

La57

Ac89

227.028

Ti22

4

Zr40

Hf72

Rf104

(261) (262) (263) (262) (265) (266?)

Praseodymium

140.908

Protactinium

Cr24

6

Mo42

W74

Sg106

Pr59

Pa91

231.036

Neodymium

144.24

Uranium

Mn25

7

Tc43

Re75

Bh107

Nd60

U92

238.029

Promethium

(145)

Neptunium

Fe26

8

Ru44

Os76

Hs108

Pm61

Np93

237.048

Samarium

150.36

Plutonium

(244)

Rhodium

102.906

Iridium

192.22

2

3

4Per

iod

5

6

7

1

Transition Elements

Lanthanoid Series

Actinoid Series

Periodic Table of the Elements

Cerium

140.12

Thorium

V23

5

Nb41

Ta73

Db105

Ce58

Th90

232.038

Co27

9

Mt109

Sm62

Pu94

Rh45

77I r

Revised May 2011

Rutherfordium MeitneriumHassiumBohriumSeaborgiumDubnium

Copyright © 2011 by the Commonwealth of Virginia Department of Education

Periodic Table of the ElementsFor Assessments Based on the 2010 Chemistry Standards of Learning

Background: We need to use the periodic table to identify elements and compounds.

How to identify these:

Staircase: The staircase is a zigzag pattern that leads down in a stair shape starting at Boron. Metals: Any element to the left of the staircase, except H (H is a nonmetal)

Nonmetals: Any element to the right of the staircase

Metalloids: The elements that fall on the staircase: Symbols: B, Si, Ge, As, Sb, Te, At

Element: Is identified by only a single capital letter in the symbol. The symbol can have a single capital alone or it can have a lowercase letter as well. Compound: Is identified by two or more different capital letters in a symbol.

Ionic compounds: made of a metal and a nonmetal

Covalent compounds: made of only nonmetals.

Polyatomic Ions: can be present when there are 3 capital letters.

Use your periodic table to identify the following:

Formula Element or Compound

If element, what type?

If compound, Ionic or Covalent

Polyatomic Ion present?

Yes or no

H2O

Mo

CaCO3

CO2

Xe

NaOH

U

NH3

Ge

LiBr

1. What type of compounds have polyatomic ions? _________________________

2. Explain the difference between Co and CO.

Page 1

Review Topic 1: Elements and PTOE

Part 1. Directions: In the chart, fill in the following information for each element:

Element Group Period # of Valence

electrons

Electron

Configuration

Lewis Dot

structure

C

P

Xe

Ba

Al

Cl

K

He

Part 2. Directions: Match the following. Each element can have more than one match.

a. Li ______1. Smallest

b. Ne ______2. Highest ionization energy

c. F ______3. Highest electronegativity

d. Cs ______4. Lowest ionization energy

e. I2 ______5. Largest

______6. Lowest electronegativity

______7. Most reactive metal

______8. Least reactive metal

______9. Least reactive nonmetal

______10. Most reactive nonmetal

Page 2

Review Topic 2: Compounds and Bonding Name each of the following:

1. Mg3P2 _______________________________ 6. Fe(OH)3 _______________________________

2. CO2 _______________________________ 7. CCl4 _______________________________

3. (NH4)2SO4 _______________________________ 8. HNO3 _______________________________

4. HBr _______________________________ 9. Cu3PO4 _______________________________

5. Ca3(PO4)2 _______________________________ 10. P4O10 _______________________________

Write the formula for the following compounds: 1. Aluminum hydroxide _______________________________ 2. Sodium oxide _______________________________

3. Calcium phosphide _______________________________ 4. Magnesium nitrate _______________________________

5. Copper (II) chloride _______________________________ 6. Ammonium sulfate _______________________________

7. Potassium fluoride _______________________________ 8. Chromium (III) nitride ______________________________

9. Carbon dioxide _______________________________ 10. Dinitrogen monoxide ______________________________

11. Sulfur hexafluoride _______________________________ 12. Tetraphosphorus decoxide _________________________

Give an example of the following kinds of compounds:

1. ionic compound

2. base

3. acid (inorganic)

4. organic alcohol

5. diatomic molecule

6. organic acid

7. polar covalent compound

8. covalent compound that has polar bonds but is a non-polar molecule

Page 3

Review Topic 2: Compounds and Bonding Draw the Lewis dot structures for the following molecules and identify the shape and type of intermolecular force.

1. H2 6. O2

2. CO2 7. NH3

3. CH3COOH* 8. N2

4. H2O 9. CH4

5. HCN 10. CHF3

Page 4

Review Topic 5: Types of Chemical Reactions

Balance and classify the following types of chemical reactions: 1. Cl2 + KI → KCl + I2

2. Al(OH) 3 + H2SO4 → Al2 (SO4) 3 + H2O

3. KClO3 → O2 + KCl

4. Na + P → Na3P

5. C3H8 + O2 → CO2 + H2O

6. Na2SO4 + BaCl2 → NaCl + BaSO4

7. C5H12 + O2 → H2O + CO2

8. HNO3 + Mg(OH) 2 → H2O + Mg(NO3) 2

9. Na + BaF2 → NaF + Ba

10. Fe + O2 → Fe2O3

Write a balanced equation for the following:

1. the synthesis of sodium chloride

2. the neutralization of sulfuric acid and sodium hydroxide

3. the D.R. reaction between aluminum hydroxide and calcium chloride

4. the S.R. reaction between copper(II) sulfate and potassium metal

5. the combustion of octane (C8H18)

6. the decomposition of water

7. the dissociation of barium chloride

Page 5

Review Topic 3: Kinetic Theory Phase Diagram: Use the phase diagram to answer the following questions.

1. What is the triple point of this substance?

2. What does A, B, & C represent? How do you know?

3. What phase change will occur at 0.30 atm, if the temperature is increased from -25 oC to 50 oC?

4. What phase change will occur at 75 oC, if the pressure is decreased from 1.0 atm to 0.5 atm?

5. What phase change will occur at standard atmospheric pressure, if the temperature is decreased from 50 oC to -25 oC?

6. What phase change will occur when pressure is dropped from 0.75 atm to 0.25 atm at 270 K?

Heating Curve: Use the following heating curve for water to answer the following questions.

E

D

C

B

A

1. On the lines provided, indicate the states of matter represented by A, C, and E. Then indicate the changes in state that are occurring at B and D.

2. On the y-axis, label the appropriate temperatures of the melting and boiling points.

3. Explain what is happening to the average kinetic energy of the molecules during B and D.

4. To the righ of the heating curve, draw a picture of what a cooling curve would look like.

5. How much energy (in joules) are necessary to raise the temperature of 200 g of water from 20oC to its boiling point?

Tem

pera

ture

(oC

)

Time

Page 6

Review Topic 3: Kinetic Theory

Potential Energy Diagram: Use the following potential energy diagram to answer the following questions:

E

B

C

A

D

1. Write a balanced equation for the reaction depicted. (be sure to include the energy)

2. Is the forward reaction endothermic or exothermic? How do you know?

3. What letter represents the H? Calculate its value.

4. What letter represents the activation energy of the forward reaction?

5. How would a catalyst affect this reaction? Redraw the diagram to show a catalyst’s effect.

Vapor Pressure Curve: Use the vapor pressure curve provided to answer the following questions.

1. Which of the substances has the highest vapor pressure at 30 oC?

2. Which of the substances has the highest boiling point at standard pressure?

3. Which one these substances have the strongest intermolecular attractions? Why?

Reaction Progress

70 kJ

125 kJ

KCl + O2

KClO3

Pote

ntial E

nerg

y

Page 7

Review Topic 6: Solutions and Equilibrium Solubility Curve: Use the solubility curve provided to answer the following questions. (topic 6)

1. What is the relationship between the solubility of a solid and temperature? and of a gas and temperature? 2. What substances on the graph are gases and how do you know?

3. What substance is the most soluble at 50 OC? Which is the least soluble at 80 oC?

4. What is the solubility of the sodium nitrate in 100 grams of water at 70 oC?

5. What is the solubility of ammonia in 200 grams of water at 50 oC?

Le Chatelier’s Principle: 1. Define and use an example to explain equilibrium.

2. Given the following equation at equilibrium:

N2 (g) + 3H2 (g)→ 2NH3 (g) H=-46kJ

Use an arrow to show the direction in which the reaction will shift for each “stress” in order to reestablish equilibrium.

a) Add NH3 b) Increase the temperature c) Decrease the pressure d) Remove N2 e) Add H2 f) Add a catalyst g) Remove NH3 h) Decrease the temperature

Page 8

Review Topic 4: Random Stoichiometry Show all work!

1. What is the density of an unknown object if its mass was found to be 10.58 g and its volume is 4.6mL? *(Sig Fig’s) 2. What is the pressure of 16 grams of oxygen gas (O2) that has a volume of 5.6 L and a temperature of 45oC?

(R = 0.0821 L atm/mol K) 3. How many grams is one mole of NH4OH? Two moles? 0.25 moles? 4. How many moles is 404 g of KNO3? 5. What is the molarity of a solution in which 0.40 grams of NaOH is dissolved in water so that the final volume of the

solution is 100 mL? What is the resulting solution’s pH? 6. What volume in liters of 12 M HCl must be used to make 500 mL of a 3 M solution?

Page 9

Review Topic 4: Stoichiometry Show all work!

Use the balanced equation to answer the following questions: N2 (g) + 3 H2 (g) → 2 NH3 (g)

a. How many moles of nitrogen would be needed to react completely with 6 moles of hydrogen gas? b. How many moles of nitrogen gas would be needed to make 8.5 g of ammonia gas? c. How many grams of ammonia would be made if 56 grams of nitrogen reacted completely? d. How many liters of hydrogen at STP are necessary to produce 17 grams of ammonia?

Page 10