Unit I Safety Unit Analysis Measurement

Lesson Day Date Topic Homework

1. Safety                             1

2. Disssociation and Ionic Formulas 2

3. Balancing and Word Equations 3

4. Physical and Chemical Changes 4

5. Matter and Bonding 5

6. Review and Lab Preparation 6

7. Uncertainty Lab Day 1 Lab Handout

8. Uncertainty Lab Day 2

9. Measurement and Uncertainty 7

10. Significant Figures 8

11. Unit Analysis 1 9

12. Unit Analysis 2 10

13. Reading Scales 11

14. Density Calculations 12

15. Practice Test 13

16. Test

Assignment # 1 Safety

Complete the safety map for the room by indicating the location of the three fire extinguishers, five doors, eyewash, fume-hood, fire blanket, aprons, eye-goggles, broken glass container, spill control pillows, four soap dispensers, three paper towel dispensers, and the soap sprayer. This is like a treasure hunt. Get up and look for everything.

Assignment # 2 Ionic Formulas

Write the ionic formula, name, and dissociation equation for each combination indicated by the cell below.

Note that all ionic compounds (start with metals) are solids at room temperature.

	Li	Mg	Al	NH4	Na
OH	1	2	3	4	5
SO4	6	7	8	9	10
Br	11	12	13	14	15
F	16	17	18	19	20
NO3	21	22	23	24	25
PO4	26	27	28	29	30
S	31	32	33	34	35
C2O4	36	37	38	39	40

1. LiOH Lithium hydroxide LiOH_(s) → Li⁺_(aq) + OH^-_(aq)

2.

3. Al(OH)₃ Aluminum hydroxide Al(OH)_3(s) → Al^3+_(aq) + 3OH^-_(aq)

4.

5. NaOH Sodium hydroxide NaOH_(s) → Na^+_(aq) + OH^-_(aq)

6.

7. MgSO₄ Magnesium sulphate MgSO_4(s) → Mg^2+_(aq) + SO₄^2-_(aq)

8.

9. (NH₄)₂SO₄ Ammonium sulphate (NH₄)₂SO_4(s) → 2NH₄^+_(aq) + SO₄^2-_(aq)

10.

11. LiBr Lithium bromide LiBr_(s) → Li^+_(aq) + Br^-_(aq)

12.

13. AlBr₃ Aluminum bromide AlBr_3(s) → Al^3+_(aq) + 3Br^-_(aq)

14.

15. NaBr Sodium bromide NaBr_(s) → Na^+_(aq) + Br^-_(aq)

16.

17. MgF₂ Magnesium Fluoride MgF_2(s) → Mg^2+_(aq) + 2F^-_(aq)

18.

19. NH₄F Ammonium Fluoride NH₄F_(s) → NH₄^+_(aq) + F^-_(aq)

20.

21. LiNO₃ Lithium nitrate LiNO_3(s) → Li^+_(aq) + NO₃^-_(aq)

22.

23. Al(NO₃)₃ Aluminum nitrate Al(NO₃)_3(s) → Al^3+_(aq) + 3NO₃^-_(aq)

24.

25. NaNO₃ Sodium nitrate NaNO_3(s) → Na^+_(aq) + NO₃^-_(aq)

26.

28. AlPO₄ Aluminum phosphate AlPO_4(s) → Al^3+_(aq) + PO₄^3-_(aq)

29.

30. Na₃PO₄ Sodium phosphate Na₃PO_4(s) → 3Na^+_(aq) + PO₄^3-_(aq)

31.

32. MgS Magnesium sulphide MgS_(s) → Mg^2+_(aq) + S^2-_(aq)

33.

34. (NH₄)₂S Ammonium sulphide (NH₄)₂S_(s) → 2NH₄⁺_(aq) + S^2-_(aq)

35.

36.

37. MgC₂O₄ Magnesium oxalate MgC₂O_4(s) → Mg²⁺_(aq) + C₂O₄^2-_(aq)

38.

39. (NH₄)₂C₂O₄ Ammonium oxalate (NH₄)₂C₂O_4(s) → 2NH₄⁺_(aq) + C₂O₄^2-_(aq)

Assignment #3 Chemical Equations from Word Equation

1. Aqueous potassium hydroxide is reacted with aqueous sulphuric acid producing a solution of potassium sulphate and water.

2KOH_(aq) + H₂SO_4(aq) → K₂SO_4(aq) + 2H₂O_(l)

2. Sodium metal is reacted with zinc iodide in solution. The products obtained are aqueous sodium iodide in and zinc metal.

3. Solid calcium sulphate dihydrate is added to gaseous sulphur trioxide producing solid calcium sulphate and aqueous sulphuric acid.

CaSO₄^.2H₂O_(s) + 2SO_3(g) → CaSO_4(s) + 2H₂SO_4(aq)

4.         Solid calcium phosphate and aqueous sodium nitrate are formed when solutions of sodium phosphate and calcium nitrate are mixed.

          2Na₃PO_4(aq)   +        3Ca(NO₃)_2(aq) ®            Ca₃(PO₄)_2(s)    +   6NaNO_3(aq)

5.         Sodium phosphite reacts with calcium nitrate in solution to produce two new ionic compounds. The calcium compound is solid while the other is aqueous.

            2Na₃PO_4(aq)   +        3Ca(NO₃)_2(aq) ®            Ca₃(PO₄)_2(s)    +   6NaNO_3(aq)

6.         Gaseous sulphur trioxide, a pollutant released into the atmosphere by burning coal reacts with liquid water in the air to make a solution of sulphuric acid (acid rain).

           SO_3(g)    +    H₂0_(l) ®    H₂SO_4(aq)

Assignment # 4 Physical and Chemical Changes Balancing Equations

Classify as a physical or chemical change.

1. Spoiling of food Chemical

2. Vaporization of ice Physical

3. Stretching of a rubber band Physical

4. Dynamite explosion Chemical

5. Shattering of glass Physical

6. Decaying of dead bodies Chemical

7. Extraction of iron from form (Fe₂O₃) Chemical

8. Spontaneous combustion of oily rags Chemical

9. Grinding of wheat Physical

10. Melting snow Physical

11. 2 H₂O → 2 H₂ + O₂ + Energy Chemical

12. E + NaCl_(s) → NaCl_(aq) Physical

13. Determine the physical state of each element at -5 ⁰C (use the Handbook, Textbook, or Net to determine the melting point and boiling point of each).

mp bp physical state

a) Mercury -38.87 ^oC 356.58 ^oC liquid

b) Bromine -7.2 ^oC 58.78 ^oC liquid

c) Chlorine -100 ^oC -34.6 ^oC gas

Classify as a physical or chemical properties.

14. Sugar chars when heated chemical property

15. Yellow color of sulphur physical property

16. Tarnishing ability of sulphur chemical property

17. Flexibility of a spring physical property

18. Thermal conductivity of iron physical property

19. Hardness of a diamond physical property

20. Stability of nitrogen chemical property

21. Describe 11 and 12 as exothermic or endothermic

Write Ionic Formulas

22. Aluminum oxide Al₂O₃

23. Aluminum chloride AlCl₃

24. Ammonium acetate NH₄CH₃COO

25. Barium phosphate Ba₃(PO₄)₂

26. Calcium hydroxide Ca(OH)₂

27. Sodium hydroxide NaOH

28. Strontium phosphate Sr₃(PO₄)₂

29. Iron II phosphate Fe₃(PO₄)₂

30. Cobalt III sulphate pentahydrate Co₂(SO₄)₃^.5H₂O

31. Copper II nitrate hexahydrate Cu(NO₃)₂^.6H₂O

Write an equation

32. Sodium chloride dissolving in water (endothermic).

NaCl_(s) + energy → Na⁺_(aq) + Cl^-_(aq)

33. Lead II nitrate reacting with sodium phosphate to produce solid Lead II phosphate and sodium nitrate (exothermic and three chemicals are aqueous).

3Pb(NO₃)_2(aq) + 2Na₃PO_4(aq) → Pb₃(PO₄)_2(s) + 6NaNO_3(aq)

34. List three chemical and physical properties.

Chemical: reactivity flammability stability

Physical: mass colour density

1. Label each as chemical or physical.

a) Ice cubes turn to water physical

b) Steam forms water droplets in a mirror physical

c) Milk is made into ice milk physical

d) Ice cubes shrink in a freezer physical

e) Perspiration “dries” physical

f) Bromine is liquefied from solid bromine physical

2. What change in physical state occurs during the formation of the following?

a) Rain condensation

b) Snow freezing

c) Frost freezing

d) Steam evaporation

3) A sealed glass bulb is half-filled with water, on which some ice and wood are floating. The remainder of the bulb is filled with air. How many physical states are present? Identify them.

solid: ice and wood

liquid: water

Gas: air and water vapour

4) Classify each of the following as a physical or chemical change.

a) Photosynthesis (CO₂ + H₂O → Sugars + oxygen) Chemical

b) Antifreeze boils out of a radiator Physical

c) A firefly emits light Chemical

d) A nail is magnetized Physical

e) A nail rusts Chemical

f) Leaves turn color in autumn  Chemical

g) Food spoils Chemical

h) Dynamite explodes Chemical

I) Grinding of wheat into flour  Physical

j) Shattering of glass Physical

k) Extraction of iron from iron ore (Fe₂O₃) Chemical

5) Identify the chemical and physical changes in the following sequences:

a) A lump of sugar is ground to a powder Physical and then heated in air Physical. It melts Physical, then darkens Chemical, and finally bursts into flames and burns Chemical.

b) Gasoline is sprayed into the carburetor Physical, mixed with air Physical, converted to vapor Physical, burned Chemical, and the combustion roducts expand the cylinder Physical.

Balancing Equations

1. 2KNO₃ → 2KNO₂ + O₂

2. CaC₂ + 2O₂ → Ca + 2CO₂

3. C₅H₁₂ + 8O₂ → 5CO₂ + 6H₂O

4. K₂SO₄ + BaCl₂ → 2KCl + BaSO₄

5. 2KOH + H₂SO₄ → K₂SO₄ + 2H₂O

6. Ca(OH)₂ + 2NH₄Cl → 2NH₄OH + CaCl₂

7. 5C + 2SO ₂ → CS₂ + 4CO

8. Mg₃N₂ + 6H₂O → 3Mg(OH)₂ + 2NH₃

9. V₂O₅ + 5Ca → 5CaO + 2V

10. 2Na₂O₂ + 2H₂O → 4NaOH + O₂

11. Fe₃O₄ + 4H₂ → 3Fe + 4H₂O

12. Cu + 2H₂SO₄ → CuSO₄ + 2H₂O + SO ₂

13. 2Al + 3H₂SO₄ → 3H₂ + Al₂(SO₄)₃

14. 2Si₄H₁₀ + 13O₂ → 8SiO₂ + 10H₂O

15. 4NH₃ + O₂ → 2N₂H₄ + 2H₂O

16. 2C₁₅H₃₀ + 45O₂ → 30CO₂ + 30H₂O

17. 2BN + 3F₂ → 2BF₃ + N₂

18. CaSO₄ ^. 2 H₂O + 2SO₃ → CaSO₄ + 2H₂SO₄

19. 2C₁₂H₂₆ + 37O₂ → 24CO₂ + 26H₂O

20. C₇H₆O₃ + 7O₂ → 7CO₂ + 3H₂O

21. 9Na + 4ZnI₂ → 8NaI + NaZn₄

22. 3LiAlH₄ + 4BF₃ → 3LiF + 3AlF₃ + 2B₂H₆

23. HBrO₃ + 5HBr → 3H₂O + 3Br₂

24. 15O₂ + 2Al_l4C₃ + 54H₂O → 28Al(OH)₃ + 6CH₄

25. 2Ca(NO₃)₂ ^. 3H₂O + 3LaC₂ → 2Ca(NO₃)₂ + 3La(OH)₂ + 3C₂H₂

26. 1CH₃NO₂ + 3Cl₂ → 1CCl₃NO₂ + 3HCl

27. Ca₃(PO₄)₂ + 3SiO₂ + 5C → 3CaSiO₃ + 5CO + 2P

28. Al₂C₆ + 6H₂O → 2Al(OH)₃ + 3C₂H₂

29. 2NaF + CaO + H₂O → CaF₂ + 2NaOH

30. 4LiH + AlCl₃ → LiAlH₄ + 3LiCl

31. 2CaF₂ + 2H₂SO₄ + SiO₂ → 2CaSO₄ + SiF₄ + 2H₂O

Some Tough Ones

Sorry, you are going to have to figure these out for yourself! Good luck!

___FeCl₂ + ___KNO₃ + ___HCl → ___FeCl₃ + ___NO +___ H₂O + ___KCl

___Cu + ___HNO₃ → ___Cu(NO₃)₂ + ___NO + ___H₂O

___ KMnO₄ + ___ HBr → ___MnBr₂ + ___Br₂ + ___KBr + ___H₂O

___ K₂Cr₂O₇ + ___HCl → ___KCl + ___CrCl₃ + ___H₂O + ___Cl₂

Assignment # 5 Balancing Equations Naming Formulas

6. Classify the following as elements, compounds, or mixtures:

a) Methane (CH₄) compound

b) Pizza mixture

c) Milk shake mixture

d) Zinc element

e) Laughing gas  compound

f) Clean air mixture

g) Chocolate chip cookie mixture

7. A pure blue powder when heated in a vacuum releases a greenish colored gas and leaves behind a white solid. Is the original blue powder a compound or element? Explain.

Compound, because it decomposed into two elements.

8. A shiny, metallic-like substance conducts an electric current without a change in its properties. The substance is heated until it liquefies and then an electric current is passed through the liquid again without a change in properties. Is the substance likely to be an element or compound? Explain.

Element, because it could not be decomposed by electrolysis or heating.

9. Describe the difference between chemical and physical change in terms of what occurs with the atoms involved.

Chemical change involves chemical bonds being broken and new ones being formed.

Physical change involves changes in state (s), (l), (g), and (aq). Chemical bonds are not broken.

1. 2Al + 6HCl → 2AlCl₃ + 3H₂

2. Zn + 2KOH → K₂ZnO₂ + H₂

3. B₂O₃ + 3Mg → 3MgO + 2B

4. 2C₆H₁₁OH + 17O₂ → 12H₂O + 12CO₂

5. 2C₁₂H₂₆ + 37O₂ → 26HOH + 24CO₂

6. 2Na + 2H₂O → 2NaOH + H₂

7. 2PbS + 3O₂ → 2PbO + 2SO₂

8. SiCl₄ + 4Na → Si + 4NaCl

9. 2Mg + CO₂ → 2MgO + C

10. 2Al + 3H₂SO₄ → Al₂(SO₄)₃ + 3H₂

Write Formulas for each

11. Zinc phosphate Zn₃(PO₄)₂

12. Ammonium carbonate (NH₄)₂CO₃

13. Iron III oxalate Fe₂(C₂O₄)₃

14. Copper II tripolyphosphate pentahydrate Cu₅(P₃O₁₀)₂^.5H₂O

15. Cobalt II borate Co₃(BO₃)₂

16. Triphosphorus tetroxide P₃O₄

17. Dicarbon hexachloride C₂Cl₆

18. Trisilicon octafluoride Si₃F₈

19. Sodium tetraborate Na₂B₄O₇

20. Aluminum dichromate Al₂(Cr₂O₇)₃

21. Calcium oxide CaO

22. Silver thiosulphate Ag₂S₂O₃

Write balanced chemical equations and include phase symbols for each formula.

23. Aqueous calcium nitrate is reacts with a solution of sodium phosphate producing solid calcium phosphate and aqueous sodium nitrate.

3Ca(NO₃)_2(aq) + 2Na₃PO_4(aq) → Ca₃(PO₄)_2(s) + 6NaNO_3(aq)

24. Gaseous nitrogen trihydride reacts with oxygen gas to produce gaseous nitrogen monoxide and gaseous water and energy.

4NH_3(g) + 5O_2(g) → 4NO_(g) + 6H₂O_(g) + energy

25. Phosphoric acid reacts with Calcium hydroxide both in solution to produce and aqueous salt and water.

2H₃PO_4(aq) + 3Ca(OH)_2(aq) → Ca₃(PO₄)_2(aq) + 6H₂O_(l)

26. Write an equation for the combustion of sucrose.

C₁₂H₂₂O_11(s) + 12O_2(g) → 12CO_2(g) + 11H₂O_(l)

27. Write an equation for the cellular respiration of vitamin C.

C₆H₈O_6(s) + 5O_2(g) → 6CO_2(g) + 4H₂O_(l)

28. Describe what you know about covalent or molecular compounds.

Formula starts with a nonmetal

Shared electrons

Full valance shells

Stable compounds

Worksheet # 6 Balance each equation.

1. 2Sb + 5Cl₂ → 2SbCl₅

2. 2FeCl₂ + Cl₂ → 2FeCl₃

3. 2P + 3I₂ → 2PI₃

4. Na₂S + 2HCl → 2NaCl + H₂S

5. 3NaOH + FeCl₃ → 3NaCl + Fe(OH)₃

6. 3KOH + H₃PO₄ → K₃PO₄ + 3H₂O

7. 2NaOH + CuSO₄ → Na₂SO_{4 +} Cu(OH)₂

8. 2HNO₃ + Ca(OH)₂ → 2H₂O + Ca(NO₃)₂

9. 2NH₃ + 3CuO → 3H₂O + 3Cu + N₂

10. N₂ + 4C + Na₂CO₃ → 2NaCN + 3CO

11. 2NH₃ + 5O → 2NO + 3H₂O

12. 4NH₃ + 7O₂ → 4NO₂ + 6H₂O

13. 2NH₃ + 4O₂ → N₂O₅ + 3H₂O

14. 2P + 5N₂O → P₂O₅ + 5N₂

15. 2Al + 6HCl → 2AlCl₃ + 3H₂

16. Zn + 2KOH → K₂ZnO₂ + H₂

17. B₂O₃ + 3Mg → 3MgO + 2B

18. 2CH₃OH + 3O₂ → 4H₂O + 2CO₂

19. C₆H₁₂O₆ → 2C₂H₅OH + 2CO₂

20. 2Na + 2H₂O → 2NaOH + H₂

21. 2PbS + 3O₂ → 2PbO + 2SO₂

22. SiCl₄ + 4Na → Si + 4NaCl

23. 2Mg + CO₂ → 2MgO + C

24. 2Al + 3H₂SO₄ → Al₂(SO₄)₃ + 3H₂

Write balanced chemical formulas for each ionic compound.

25. Calcium hydroxide Ca(OH)₂

26. Aluminum sulphate Al₂(SO₄)₃

27. Iron III oxide Fe₂O₃

28. Zinc acetate Zn(CH₃COO)₂

29. Barium carbonate BaCO₃

30. Sodium phosphate Na₃PO₄

31.Cobalt II nitride Co₃N₂

32. Gallium sulphate Ga₂(SO₄)₃

33. Aluminum fluoride AlF₃

34. Ammonium sulphate (NH₄)₂SO₄

35. Aluminum acetate Al(CH₃COO)₃

Write balanced chemical formulas for each molecular (covalent) compound.

36. carbon monoxide CO

37. dinitrogen tetraiodide N₂I₄

38. triphosphorus hexafluoride P₃F₆

39. dinitrogen dioxide N₂O₂

Write balanced chemical equations for each word equation. Include phase symbols for all formulas.

40. Solid sodium oxide dissolves in water to make sodium oxide solution.

Na₂O_(s) → 2Na⁺_(aq) + O^2-_(aq)

41. Solid aluminum sulphate dissolves in water to make a solution

Al₂(SO₄)_3(s) → 2Al³⁺_(aq) + 3SO₄^2-_(aq)

42. Barium phosphate plus sodium sulphate (both in water) yields solid barium sulphate and aqueous sodium phosphate.

Ba₃(PO₄)_2(aq) + 3Na₂SO_4(aq) → 3BaSO_4(s) + 2Na₃PO_4(aq)

43. Lead metal added to Sulphuric acid solution produces lead IV sulphate precipitate and diatomic hydrogen gas.

Pb_(s) + 2H₂SO_4(aq) → Pb(SO₄)_2(s) + 2H_2(g)

44. Potassium iodide (aq) plus lead II nitrate (aq) yields potassium nitrate (aqueous) plus lead II iodide (solid).

2KI_(aq) + Pb(NO₃)_2(aq) → 2KNO_3(aq) + PbI_2(s)

45. Calcium carbonate (solid) plus aqueous hydrochloric acid yields (aqueous) calcium chloride, carbon dioxide gas and water.

CaCO_3(s) + 2HCl_(aq) → CaCl_2(aq) + CO_2(g) +H₂O_(l)

46. Potassium nitrate (aq) plus iron III hydroxide (aq) yields iron III nitrate (aq) plus potassium hydroxide (aq).

3KNO_3(aq) + Fe(OH)_3(aq) → Fe(NO₃)_3(aq) + 3KOH_(aq)

You are good if you can do these. On your own of course!

1. ___HCl + ____K₂CrO₄ → ____KCl + ____CrCl₃ +____H₂O +____Cl₂

2. __K₂Cr₂O₇ + __KI + __H₂SO₄ → __K₂SO₄ + __Cr₂(SO₄)₃ + ___I₂ +___H₂O

Worksheet # 7 Measurement and Uncertainty

1. Five different voltmeters are used to measure the voltage in a circuit. Determine the average and uncertainty.

25.61V

25.63V

25.65V 25.63 ± 0.02 V

25.64V

25.63V

Six thermometers give the following readings. Determine the average and the uncertainty.

352.4 ⁰C

352.5 ⁰C

352.6 ⁰C

352.5 ⁰C

352.7 ⁰C

352.6 ⁰C

2. Determine the average and uncertainty for the data:

25.56 g 25.54g 25.52g 25.53g 25.55g

Answer 25.54 ± 0.02 g

3. Determine the average and uncertainty for the data:

5.216 oC 5.218 oC 5.213 oC 5.214 oC 5.416 oC

Answer

4. How many significant figures are in each number?

25.63 4 101 3 0.0075 2

0.0002 1 1.00 3 2.005 4

10.031 5 1.0002 5 10005 5

0.00521 3 2.51 x 10⁴ 3 3 x 10^-7 1

2 x 10⁵ 1 2.00 x 10³ 3 250. 3

5. Round off to three significant figures.

0.05211      0.0521 0.0087251  0.00873

85.337 85.3 2.6177 x 10^-5 2.62 x 10^-5

2.5175 x 10^-18 2.52 x 10^-18 25.731 x 10⁵ 2.57 x 10⁶

Round off each measured number to three significant figures.

6. 0.002567 .00257

7. 94549 9.45 x 10⁴

8. 15.00 15.0

9. Round off the following numbers to three significant figures:

a) 35.234 35.2 b) 2.34521 2.35 c) 0.035219 0.0352

d) 2533521 2530000 e) 6255520000 6260000000

10. State the number of significant figures in each approximate number.

a) 305 3 b) 25.25 4 c) 3.00 3

d) 0.001 1 e) 3.0050 5

f) 6.25 x 10²³ 3 g) 7.00 x 10^-2 3 h) 1001 4

11. Add or subtract the measured quantities.

25.31 22.0 22.7 35.271

+ 6.4 + 0.04 + 0.77 + 0.2

31.7 22.0 23.5 35.5

22.71 25.217 2.51639 8.0558

- 0.299 + 0.017 - 1.2358 + .3259297

22.41 25.234 1.2806  8.3817

25.634 + 2.365 - 0.25498 + 0.225 = 27.969

12. 15.239 + 5.36 20.60

13. 2.6679 - 1.23 1.44

14. 2.059378 x 10²⁴ + 5.3 x 10²² 2.112 x 10²⁴

15. 8.5 x 10 ^-24 + 5.37894 x 10^-25 9.0 x 10^-24

16. 2.3 x 10 ¹⁶ + 8.224 x 10¹⁹ 8.226 x 10¹⁹

17. 5.6 x 10 ^–8 + 9.5563 x 10^-6 9.612 x 10^-6

18. 9.55 x 10 ^-10 + 5.4455 x 10^-12 9.60 x 10^-10

19. 2.66 x 10 ^-16 + 3.445 x 10^-18 2.69 x 10^-16

20. 3CaSi₂ + 2SbCl₃ → 6Si + 2Sb + 3CaCl₂

21. 2TiO₂ + B₄C + 3C → 2TiB₂ + 4CO

22. 4NH₃ + 5O₂ → 4NO + 6H₂O

23. SiF₄ + 8NaOH → Na₄SiO₄ + 4NaF + 4H₂O

24. 2NH₄Cl + CaO → 2NH₃ + CaCl₂ + H₂O

25. 4NaPb + 4C₂H₅Cl → Pb(C₂H₅)₄ + 3Pb + 4NaCl

26. Be₂C + 4H₂O → 2Be(OH)₂ + CH₄

27. 4NpF₃ + O₂ + 4HF → 4NpF₄ + 2H₂O

28. 3NO₂ + H₂O → 2HNO₃ + NO

Worksheet # 8

1. 25 x 3 2. 3.35 x 0.26 3. 799 x 877

8 x 10¹ or 80 0.87 7.01 x 10⁵ or 701000

4. (6.2 x 10³)( 3.55 x 10¹²) 5. (6.3 x 10⁷)(2.51 x 10^-7)

(3.214 x 10^-5)

2.2 x 10¹⁶ 4.9 x 10⁵

6. (7.52 x 10¹⁶)(3.1 x 10¹²) 7. 3.5 x 10² ÷ 3.1 x 10³

(2.5 x 10^-7)

9.3 x 10³⁵ 1.1 x 10^-1

8. (2.00 x 10²³)(3.51 x 10^-22)(3.5 x 10³)

(7.5 x 10^-3)(3.511 x 10¹²)(6.6 x 10^-6)

1.4

9. (5.200 x 10^-5)(6.02 x 10^-12)(3.58 x 10¹⁷)

(2.337 x 10^-3)(6.2154 x 10¹²)(5.22 x 10^-12)

1.48 x 10³

10. 156 x 256 x 21 x 0.0005687

0.02569 x 13.235 x 2654

0.53

11. (8.5 x 10 ^-24) ( 5.37894 x 10^-25) ( 4.532 x 10¹⁵)

(2.059378 x 10 ²⁴) (5.3 x 10²²) ( 9.37894 x 10^-13)

2.0 x 10^-67

12. 25.7 x 0.21 5.4

13 35 x 105 3.7 x 10³

14. 51.71 x 22.3 1.15 x 10³

15. 22 x 305 6.7 x 10³

16. Write three examples of exact numbers.

6 fish 8girlfriends 3pens

17. Write three examples of approximate numbers.

1.2 cm 2.45 Kg 2.233 V

Circle the uncertain digit and underline the uncertainty in each of the following numbers.

18. 35.2 ± 0.1 g 19. 22.221 ± 0.005 mm 20. 100. ± 2 lb.

21. Give the largest and smallest value of the approximate number

35.21 ± 0.02 g largest: 35.23 g smallest: 35.19 g

22. 26.215 23. 65.222 24. 22 - 0.01

- 0.3 + 1.03

25.9 66.25 22

25. 10. + 0.1 26. 33.3 + 0.35 27. 29.39 + 0.2

10. 33.7 29.6

Calculate the average measurement and the uncertainty of each measuring device below:

28. The mass (in grams) readings on a balance:

58.56

58.59

58.51

58.61

58.57

58.56

Answer 58.6 ± 0.1 g

29. The voltage (in mV) readings on a number of voltmeters:

123.2

124.5

124.0

124.3

124.3

Answer 124.3 ± 0.3 mV

30. State the number of significant digits for each number:

a) 0.00200 L 3 b) 5.000 g 4 c) 1.00003 A 6

d) 1000.000 Mm 7 e) 2.5 x 10⁷⁶ 2 f) 78.89 m 4

31. Perform the following calculations and round to the appropriate level of uncertainty (assume all numbers are from measurements):

a) 18 + 0.21 18

b) 62.1 x 3021.56 1.88 x 10⁵

c) 1.05 g + 253.8 mg + 24.98 mg Watch units!

1.05

0.2538

0.02498

1.32 g

d) (9.442 x 10^-3)(3.21 x 10⁸) 3.03 x 10⁶

e) 231.4 - 8.2295 223.2

f) (8.995 ^x 10⁶) + (3.55 ^x 10⁷) 4.45 x 10⁷

g) 12.0355 + 1.024 13.060

h) (4.56 x 10^-8)(2.5 x 10³⁵) 1.1 x 10²⁸

i) (9.24 x 10¹⁰)(5.233 x 10⁴) 4.84 x 10¹⁵

32. State the difference between accuracy and precision.

Accuracy refers to how close a measurement is to the true or accepted value.

Precision is the opposite of uncertainty and refers to the variation of a measurement with different measuring devices.

The lower the variation the greater the precision and the higher the uncertainty.

Worksheet # 9         Unit Analysis 1

All work must be shown as illustrated below. The work is more important than the answer.

1. 527 g to mg

527 g x 1 x 10³ mg = 5.27 x 10⁵ g

1g

2. 1.05 x 10⁶ um to m

1.05 x 10⁶ μm x 1 g = 1.05 m

1 x 10⁶ μm

3. 2.148 ML to mL

2.148 ML x 1 x 10⁶ L x 1 x 10³ mL = 2.148 x 10⁹ mL

1ML 1L

4. 0.0235 mg to Kg

0.0235 mg x 1g x 1kg = 2.35 x 10^-8 kg

1 x 10³ mg 1 x 10³ g

5. 8.32 x 10^-4 mL to ML

8.32 x 10^-4 mL x 1 L x 1 ML = 8.32 x 10^-13 ML

1 x 10³ mL 1 x 10⁶ L

6. 772.5 us to ms

772.5 μs x 1 ms = 0.7725 ms

1 x 10³ μs

7. 3.06500 cg to kg

3.06500 cg x 1 g x 1 kg = 3.06500 x 10^-5 Kg

1 x 10² cg 1 x 10³ g

8. 9.450 Mm to mm

9.450 Mm x 1 x 10⁶ m x 1 x 10³ mm = 9.450 x 10⁹ mm

1Mm 1 m

9. 5.64 x 10³ mm² to cm²

5.64 x 10³ mm² x 1 cm² = 5.64 x 10¹ cm²

1 x 10² mm²

1. 605 µm to mm

0.605 mm

2. 6.5 x 10^-6 Mm to m

6.5 m

3. 20.0 km to cm.

2.00 x 10⁶ cm

4. 8.774 x 10¹⁵ µm to Mm.

8774 Mm

5. 25 cL to ML

2.5 x 10^-7 ML

6. 648 kPa to mPa

6.48 x 10⁸ mPa

7. 2.665 Mg to µg

2.665 x 10¹² μg

Worksheet # 10

Use unit analysis and the conversion factors to perform the following conversions:

2.210 lb = 1.000 kg 14 lb = 1 stone (defined) 2000 lb = 1 ton (defined)

1.61 km = 1.00 mile 4.54 L = 1.00 gallon 16 oz = 1 lb (defined)

1. 170 lb to kg

170 lb x 1 kg = 76.9 kg

2.210 lb

2. 648 KPa to atm

648 kpa x 1 atm = 6.40 atm

101.3 kpa

3. 256 oz to tons

256 oz x 1 lb x 1 ton = 8.00 x 10^-3 tons

16 oz 2000 lb

4. 0.025 ton to mg

0.025 ton x 2000 lb x 1 kg x 1 x 10³ g x 1 x 10³ mg = 2.3 x 10⁷ mg

1 ton 2.21 lb 1 kg 1 g

5. 0.236 Gal to mL

1.07 x 10³ mL

6. 5.8 x 10⁶ mL to Gal

1.3 x 10⁴ Gal

7. 5.66 x 10⁶ mg to stones

0.893 stones

8. 15 miles to mm

2.4 x 10⁷ mm

9. 5.63 x 10⁹ µm to miles

3.50 miles

10. 152 mL to gal

152 mL x 1 L x 1 gal = 3.35 x 10^-2 gal

1000 mL 4.54 L

11. 8.6 stone to oz

256 stone x 14 lb x 16 oz = 1.9 x 10³ oz

1 stone 1 lb

12. 4.3 m to miles

4.3 m x 1 Km x 1.00 mile = 2.7 x 10^-3 miles

1000 m 1.61 Km

13. 15.2 mi/gal to L/km

1 gal x 4.54 L x 1 mi = 0.186 L/km

15.2 mi 1 gal 1.61 km

14. 2.3 gal to mL

1.0 x 10⁴ mL

15. 45.2 oz to stones

0.202 stones

15. 46.3 miles to m

7.45 x 10⁴ m

17. 36 L/km to mi/gal

0.078 mi/gal

18. If 3 dogs are worth 2 cats, 8 cats are worth 2 lions, 5 lions are worth 8 elephants, 2 elephants are worth 8700000 ducks, 47 ducks are worth 63 geese, 14 geese are worth 27 snakes, 42 snakes are worth 778396 fruit flies, and a dog costs $205.00, how much does a fruit fly cost? Use unit analysis and assume all conversions are exact.

1 FF x 42 sn x    14 ge x 47 du x 2 el x 5 li x 8 ca x 3 do x $205.00

  778396 FF 27 sn 63 ge 8700000 du 8 el 2 li 2 ca 1 dog

$ 4 x 10^-9 for one fruit fly

19. Light travels 9.46 x 10¹⁵ m in one year. This distance is called a light-year. Calculate the speed of light in metres per second. Use unit analysis.

3.00 x 10⁸ m/s

20. The following trade ratios are used in a small country in the Middle East near Iran called Yrtsimehc. A young man is in love with a beautiful woman, however, he must pay a dowry of 12 camels to marry her. The young man is a yam farmer and has only 12,000 yams to trade. Can he marry his true love?

Use unit analysis to support your answer.

15 pigs = 2 cows 3 cows = 2 horses 17 chickens = 1 pig

2 horses = 3 camels 20 lbs of figs = 16 chickens 56 yams = 10 lbs of figs

1.3 x 10² camels Yes he can marry and have camels left over for the honeymoon.

Worksheet # 11 Review

Given:	$0.2045 Can.	=	1.00 Francs (French)
	$2.1860 Can.	=	£ 1.00 (UK)
	$1.3572 Can.	=	$ 1.00 U.S.
	$0.1534 Can.	=	1.00 Peso (Mexico)
	$0.0109 Can.	=	¥ 1.00 (Japanese Yen)
	$0.0263 Can.	=	1.00 Rupee (India)
	$1.00 U.S.	=	1.9325 Marks (Germany)

Convert:

1. $300.00 Can. to £.

137.24 £.

2. $1025.00 Can. to pesos.

6681.88 pesos

3. $450.00 U.S. to yen.

56031 yen

4. £ 652.23 to francs.

6972.0 francs

5. 85.2 Marks to £.

27.4 £

6. 3842.35 Yen to Rupees.

1592.46 Rupees

7. 9668.75 Francs to Marks.

2815.39 marks

Black Market Trading Conversions

Given:	1 Ticket	=	2 CDs
	5 Buttons	=	3 T Shirts
	4 Tickets	=	1 Back Stage Pass
	1 CD	=	3 T Shirts
	7 Posters	=	3 Buttons

Convert:

1. 28 Posters to buttons.

28 Pos             x          3 But               =          12 buttons

7 Pos

2. 10. CDs to tickets.

10 CD x 1 ticket = 5.0 tickets

2 CD

3. 100. Buttons converted to CDs.

20.0 CDs

4. 1 Back Stage Pass converted to T Shirts.

24 T-shirts

5. 280. Posters to Back Stage Passes.

3.00 BSP

6. 6 Back Stage Passes to buttons.

240 buttons

Use unit analysis to perform the following conversions:

7. 6.372 hL to mL 6.372 x 10⁵ mL

6.372 hL x 1 x 10² L x 10³ mL= 6.372 x 10⁵ mL

1 hL 1 L

8. 4.9 x 10¹⁵ µg to Mg 4.9 x 10³ Mg

4.9 x 10³ Mg

9. 8.774 x 10³ cm³ to m³ 0.008774 m³

8.774 x 10^-3 m³

10. Given the following relationships, determine how many zings can be obtained when you trade 20.6 balls.

4 clangs = 3 dangs 7 dangs = 3 jars 2 balls = 5 clangs 6 jars = 1 zing

2.76 zings

11. State the number of significant digits for each number:

a) 25.0 g 3 b) 1000 g infinite c) 25.036 A 5 d) 5.214 x 10^-62 mL 4

1 kg

3 infinite 5 4

e) 0.0000005 L 1 f) 8.2000 m

1 55

Determine the average and uncertainty given the following measurements from a

12. Centigram balance

82.62 g

82.54 g

82.48 g 82.6 ± 0.1 g Note the uncertainty is in the first decimal place.

82.72 g

82.65 g 82.6 ± 0.1 g

13. Show the interval on the number line that represents the range for the above measurement after it has been round off correctly.

	82.5	82.6	827

Write chemical formulas for each ionic or molecular compound.

14. Iron III oxide Fe₂O₃

15. Triphosphorous hexoxide P₃O₆

16. Aluminum hydroxide Al(OH)₃

17. Nickel II phosphate octahydrate Ni₃(PO₄)₂ ^. 8H₂O

Name each chemical formula

18. K₃PO₄ Potassium phosphate

19. Mn₃P₂ Manganese II phosphide

20. Ga₂(SO₃)₂ ^. 6H₂O Gallium sulphite hexahydrate

21. P₄O₁₀ tetraphosphorus decoxide

Worksheet # 12 Density Calculations

 Density calculations

1.         Calculate the volume in cm³ of 25.3 g of iron.

25.3 g     x     1 cm³                 =          3.22 cm³

                      7.87 g

2.         Calculate the mass of 65 cm³ of iron in mg.

65 cm³             x       7.87 g             x      1000 mg        =          5.1 x 10⁵ mg

                                 1 cm³ 1g

3.         Calculate the density of an expensive element that has a mass of 56.76 g and a volume of 2.938 cm³. Determine the identity of the element.

D         =          56.76 g            =          19.32 g/cm³

                        2.938 cm³

Au

4.         Calculate the density of a radioactive element that has a mass of 164.3 g and a volume of 8.693 cm³. Determine the identity of the element.

D         =          164.3 g            =          18.90 g/cm³

                        8.693 cm³

U

5.         Determine the volume in mm³ of a 55.3 g sample of lead.

55.3 g     x     1 cm³       x        1000 mm³        =          4.88   x  10³ mm³

                      11.34 g              1 cm³

6.         Determine the mass of a 59.3 mm³ sample of lead.

59.3 mm³         x          1 cm³               x          11.34 g                        =          0.672 g

                                    1000 mm³                    1 cm³

7.         Determine the volume in mm³ of a 1.0 x 10^-8 ton sample of gold.

1.0 x 10^-8 ton   x   2000 lb   x    1.00 kg   x   1000 g    x    1 cm³    x    1000 mm³     =   0.47 mm³

                                1 ton             2.21 lb          1 kg           19.32 g          1 cm³

Worksheet 13         Practice Test

Balance each equation.

1. 2Sb + 5Cl₂ → 2SbCl₅

2. 2NH₃ + 4O₂ → N₂O₅ + 3H₂O

3. 2C₁₂H₂₆ + 37 O₂ → 24CO₂ + 26H₂O

4. 2Al + 3H₂SO₄ → 3H₂ + Al₂(SO₄)₃

(The next one is the tough one!!)

5. 3Cu + 8HNO₃ → 3Cu(NO₃)₂ + 2NO + 4H₂O

Write a balanced equation for each word equation including phase symbols.

6. Barium phosphate plus sodium sulphate (both in water) yields solid barium sulphate and aqueous sodium phosphate.

Ba₃(PO₄)_2(aq) + 3Na₂SO_4(aq) → 3BaSO_4(s) + 2Na₃PO_4(aq)

Write chemical formulas for each ionic or molecular compound.

7. Mercury II sulfide HgS

8. Diphosphorous pentoxide P₂O₅

9. Barium hydroxide Ba(OH)₂

10. Copper II sulphate hexahydrate CuSO₄^.6H₂O

Name each chemical formula

11. Na₃PO₄ sodium phosphate

12. Co₃P₂ cobalt II phosphide

13. Al₂(CO₃)₂ ^. 6H₂O aluminum carbonate hexahydrate

14. Si₂I₆ disilicon hexaiodide

15. Determine the average and uncertainty for the data:

25.56g

25.54g

25.52g

25.53g

25.55g

Answer 25.54 ± 0.02g

16. Determine the average and uncertainty for the data:

5.216 ^oC

5.218 ^oC

5.213 ^oC

5.214 ^oC

5.416 ^oC reject

Answer 5.215 ± 0.003 ^oC

Round off each measured number to three significant figures.

17. 0.002567 0.00257

18. 94549 94500 or 9.45 x 10⁴

19. 15.00 15.0

Add or subtract the measured quantities.

20. 15.239 + 5.36 20.60

21. 2.6679 - 1.238 1.430

22 12.65449 + 0.2493 12.9038

23. 8.57 x 10⁷ + 5.37894 x 10⁹ 5.4646 x 10⁹

Simplify the following rounding to the correct number of significant figures.

24. 156 x 256 x 21 x 0.0005680

.02569 x 13.235 x 2654 Answer 0.53

25. (8.5 x 10 ^-24) (5.37894 x 10^-25) ( 4.532 x 10¹⁵)

(2.059378 x 10 ²⁴) (5.3 x 10²²) (9.37894 x 10^-13)

Answer 2.0 x 10^-67

Complete the relationships:

26. 1 Mg = 1 x 10⁶ g 27. 1 Km = 1 x 10³ m

28. 1 L = 1 x 10³ mL 29. 1 g = 1 x 10⁹ ng

30. 1 x 10⁶ µs = 1 s 31. 1 x 10² cg = 1 g

32. 1 x 10¹²pg = 1 g 33. 1 x 10¹² s = 1Ts

Use unit analysis to perform the following conversions:

34. 8.13 kg to cg.

8.13 x 10⁵ cg

35. 2.3 x 10¹² µm to Mm.

2.3 Mm

36. 1.52 x 10⁴ Mm to mm.

1.52 x 10¹³ mm

37. 2.13 Mg to cg.

2.13 x 10⁸ cg

38. 8.88 x 10¹² mm to Mm.

8.88 x 10³ Mm

39. 8.52 x 10^-8 Mm to pm.

8.52 x 10¹⁰ pm

Use unit analysis and the conversion factors to perform the following conversions:

2.210 lb = 1.000 kg 14 lb = 1 stone (defined) 2000 lb = 1 ton (defined)

1.61 km = 1.00 mile 4.54 L = 1.00 gallon 16 oz = 1 lb (defined)

40. 635 mL to gal

0.140 gal

41. 3.8 stone to oz

8.5 x 10² oz

42. 25.6 m to miles

0.0159 miles

43. 26 mi/gal to L/Km

1 gal x 4.55 L x 1 mi = 0.11 L/Km

26mi 1gal 1.61 km

44. 14.5 L/Km to mi/gal

1 Km x 4.54 L x 1 gal = 0.194 mi/gal

14.5 L 1 gal 1.61 km

45. Mr. Iannone’s chemistry class is at a “Periodic Table” party. Everyone at the party is hungry, and they decide as a group that everyone wants sushi, california rolls. No one at the party has any money though. One bright student remembers that the class has a credit for 15 pizzas at Boston Pizza. Using the conversion factors below, will Mr. Iannone’s class be able to buy enough California rolls for their “Periodic Table” party if there are 28 students at the party? Assume all conversions are exact.

1 pizza = 2 Wendy’s burgers 100 brussel sprouts = 3 pieces of toast

5 pieces of toast = 1 california roll 30 tacos = 1 bag of Doritos

4 Wendy’s burger = 7 tacos 6 bowls of lime jello = 3 bag of Doritos

1 bowl of lime jello = 1000 brussel sprouts

15 Pizzas x 2 WB x 7 Tacos x 1 Bag D x 6 Lime Jello x 1000 Brussels x 3 Toast x 1 Cal Roll = 21 Cal Rolls

1 Pizz 4 WB 30 Tacos 3 Bag D 1 Lime Jello 100 Brussels 5 Toast

Sorry, the answer is no.

Read each scale and estimate the measurement to the correct number of significant figures.

46. 6.62 mL

47. 52.5 ml

48.                                         21.5 mL

49.                                                                              2.97 cm

50. 9.23 mL

51.       Micrometer Scale in mm.        5.78 mm

52.       Vernier Scale in cm.                                    1.63 cm

53.       Micrometer Scale in mm 10.93 mm

54.       Calculate the volume in cm³ of 65.3 g of copper.

7.29 cm³

55.       Calculate the mass of 208 cm³ of copper in mg.

1.86 x 10⁶ mg

56.       Calculate the density of an explosive element when wet that has a mass of 46.26 g and a volume of 24.70 cm³. Determine the identity of the element.

1.873 g/cm³

57.       Calculate the density of a element found in your bathroom that has a mass of 46.31 g and a volume of 6.4409 cm³. Determine the identity of the element.

7.190 g/cm³

58.       Determine the volume in mm³ of a 44.3 g sample of lead.

3.90 x 10³ mm³

59.       Determine the mass of a 19.3 mm³ sample of lead.

0.219 g

60.       Determine the volume in mm³ of a 6.44 x 10^-10 ton sample of copper.

           0.0650 mm³

61.       Read the graduated cylinder in mL. 21.31 mL

.

62.       Read the graduated cylinder in mL. 52.8 mL

63.       Read the buret in mL. 0.60 mL

64.       Read the buret in mL.          15.45 mL

65.       Read the buret in mL. 38.53 mL