norfolk public schools science learning in place plan ... · phase diagram: use the phase diagram...
Post on 03-Aug-2021
1 Views
Preview:
TRANSCRIPT
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
top related