MONDAY
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20.1 Oxidation numbers | |
File Size: | 347 kb |
File Type: | ppt |
Oxidation numbers practice | |
File Size: | 23 kb |
File Type: | docx |
TUESDAY
2 april
20.2 Redox
20.3 Half-Reactions
20.3 Half-Reactions
20.2,3 Redox & Half reactions | |
File Size: | 882 kb |
File Type: | ppt |
WEDNESDAY
3 april
21.1 Voltaic Cells
Due: ch20 WA
Due: ch20 WA
21.1 Voltaic Cells | |
File Size: | 1017 kb |
File Type: | ppt |
ch21 Guided notes | |
File Size: | 445 kb |
File Type: | docx |
ch 21 practice problems | |
File Size: | 78 kb |
File Type: | docx |
THURSDAY
4 april
21.1 Cell Potential
21.1 Cell Potential | |
File Size: | 359 kb |
File Type: | ppt |
FRIDAY
5 april
21.1 Complete equations
21.2,3 Batteries, electrolysis
21.2,3 Batteries, electrolysis
21.1-3 Complete equations, batteries, electrolysis | |
File Size: | 1302 kb |
File Type: | ppt |
8 aprilReview ch 20, 21
Due: -ch21 practice problems -WA ch 21
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9 aprilCh 20, 21 EXAM
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10 aprilCh 2: Units (density), Rounding, Scientific Notation
HW: Rounding & Scientific Notation Practice
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11 aprilCh 2: Precision v. accuracy (significant figures, percent error)
Due: Rounding & Scientific Notation Practice HW: Significant Figures practice
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12 aprilch2: Unit Conversions & Dimensional Analysis
Due: Significant Figures Practice HW: Conversions practice
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15 aprilDimensional Analysis/Factor Label Practice
Due: -Conversions Practice -WA ch 2
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16 aprilch11 The Mole
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17 april15.2 Solutions
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18 april1) finish worksheets
2) work on WA ch11 or ch15 |
19 aprilWork day!
HW: Stoichiometry practice Due: -The Mole Practice -Solutions Practice -WA ch 11 |
22 aprilReview ch 2, 11, 15
Due: WA ch 15 |
23 aprilEXAM CH 2, 11, 15
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24 aprilch12: STOICHIOMETRY
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25 aprilPractice Stoich
Parent Teacher Conference |
26 aprilComp day
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29 aprilQUIZ: stoichiometry
ch16: Energy Conversions and Specific Heat HW: Energy Conversions and Specific Heat Practice
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30 aprilch 16 Calculating Energy
HW: Energy Calculations practice
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Questions asked:
WA ch 20
Always include + or - when writing oxidation numbers
2. Write it as it looks on the reactant side.
15a. Cr = +3
15b. Au = +3
WA ch 21
WebAssign has some of the numbers incorrectly inputed - I will take that into account as I grade
DO NOT INCLUDE + FOR POSITIVE CELL POTENTIALS (you will need - for negative ones)
7a. lead oxide
b. lead
c. lead sulfate
8. In a fuel cell, the oxidation of a fuel is used to produce electricity.
Current can be produced and sustained as long as a fuel source is present
WA ch 2
1. volume = (how far the water rose) - 20 mL (where it started)
3. the density of aluminum is 2.7 g/cm3
8. the answer to the second part is "placeholder"
12. volume = (how far the water rose) - 20 mL (where it started)
31. slope = rise/run
WA ch 11
T-charts galore! Writing it down will solve a lot of problems.
3. Remember, 1 mol ZnCl2 = 2 mol Cl
10. 1 dozen = 12 things and 1 mol = _________ things
11. molar mass
19. Density = mass/volume
WA ch 15
Read the instructions!
5. Remember, % mass = g solute/g solution x 100. So set it up this way:
___ % = g NaCl / (g NaCl + ? g H2O) *100 Then solve for g H2O
6-9. Remember, Molarity = mol/liters
9. Don't forget to convert moles to grams
WA ch 12 + 11.4 & 11.5
FOLLOW the STEPS! It really does work.
Stoichiometry: 1) Balance equation
2) Convert grams (or beginning units) to moles
3) Convert moles to moles
4) Convert moles to grams (or needed units)
Ask your 3 questions:
1) Where do you I want to end up?
2) Where do I start?
3) How do I get there? Stoichiometry, equations, conversions, etc
Check your formulas, your units, be so careful!
4. Ni(CN) - add subscripts to this format
7. Na2CO3 = 37.03%
H2O = 62.97%
8. 1 CaSO4 . 2 H2O
name: calcium sulfate dihydrate
9. initial mass of hydrate = (mass of hydrate + crucible) - (mass of empty crucible)
mass of anhydrous solid = 8.57
1 BaCl2 . 2 H2O
barium chloride dihydrate
11-13. Rewrite the equation, reporting particles, then moles, then convert moles to grams
remember: molecules = covalently bonded; formula units = ionicly bonded
14-15. They want to know what step is that converts moles of one thing to moles of another thing
16. Divide each number by the smallest one to find the moles
17-18. mole-mole conversions
19-23. mole-mass and mass-mole conversions
24-30. mass-mass conversions
26. convert kg to g. Your answer will be in scientific notation
31-38. Limiting reactant
Remember to do 2 T-charts, compare the 2 answers you get
38-46. To find excess,
1) take the amount produced from the limiting reactant
2) convert the amount produced back to the excess reactant = amount excess used
3) initial amount - amount used = excess left over
39-45. Percent yield (theoretical yield from stoichiometry - limiting reactant)
44. BONUS! You can skip this one if you want - if you do it correctly, you get the bonus points!
47-50. Mixed principles - use what you know!
Always include + or - when writing oxidation numbers
2. Write it as it looks on the reactant side.
15a. Cr = +3
15b. Au = +3
WA ch 21
WebAssign has some of the numbers incorrectly inputed - I will take that into account as I grade
DO NOT INCLUDE + FOR POSITIVE CELL POTENTIALS (you will need - for negative ones)
7a. lead oxide
b. lead
c. lead sulfate
8. In a fuel cell, the oxidation of a fuel is used to produce electricity.
Current can be produced and sustained as long as a fuel source is present
WA ch 2
1. volume = (how far the water rose) - 20 mL (where it started)
3. the density of aluminum is 2.7 g/cm3
8. the answer to the second part is "placeholder"
12. volume = (how far the water rose) - 20 mL (where it started)
31. slope = rise/run
WA ch 11
T-charts galore! Writing it down will solve a lot of problems.
3. Remember, 1 mol ZnCl2 = 2 mol Cl
10. 1 dozen = 12 things and 1 mol = _________ things
11. molar mass
19. Density = mass/volume
WA ch 15
Read the instructions!
5. Remember, % mass = g solute/g solution x 100. So set it up this way:
___ % = g NaCl / (g NaCl + ? g H2O) *100 Then solve for g H2O
6-9. Remember, Molarity = mol/liters
9. Don't forget to convert moles to grams
WA ch 12 + 11.4 & 11.5
FOLLOW the STEPS! It really does work.
Stoichiometry: 1) Balance equation
2) Convert grams (or beginning units) to moles
3) Convert moles to moles
4) Convert moles to grams (or needed units)
Ask your 3 questions:
1) Where do you I want to end up?
2) Where do I start?
3) How do I get there? Stoichiometry, equations, conversions, etc
Check your formulas, your units, be so careful!
4. Ni(CN) - add subscripts to this format
7. Na2CO3 = 37.03%
H2O = 62.97%
8. 1 CaSO4 . 2 H2O
name: calcium sulfate dihydrate
9. initial mass of hydrate = (mass of hydrate + crucible) - (mass of empty crucible)
mass of anhydrous solid = 8.57
1 BaCl2 . 2 H2O
barium chloride dihydrate
11-13. Rewrite the equation, reporting particles, then moles, then convert moles to grams
remember: molecules = covalently bonded; formula units = ionicly bonded
14-15. They want to know what step is that converts moles of one thing to moles of another thing
16. Divide each number by the smallest one to find the moles
17-18. mole-mole conversions
19-23. mole-mass and mass-mole conversions
24-30. mass-mass conversions
26. convert kg to g. Your answer will be in scientific notation
31-38. Limiting reactant
Remember to do 2 T-charts, compare the 2 answers you get
38-46. To find excess,
1) take the amount produced from the limiting reactant
2) convert the amount produced back to the excess reactant = amount excess used
3) initial amount - amount used = excess left over
39-45. Percent yield (theoretical yield from stoichiometry - limiting reactant)
44. BONUS! You can skip this one if you want - if you do it correctly, you get the bonus points!
47-50. Mixed principles - use what you know!