Unit 1 Safety, Review and Measurement

Lesson            Day                 Date                Topic                                       Homework

1.                                                         Safety                                      Assignment # 1

2.                                                         Review                                    Assignment # 2

3.                                                         Balancing Equations

4.                                                         Formulas Equations                 Assignment # 4

5.                                                         Measurement and Uncertainty

6.                                                         Uncertainty Lab Day 1

7.                                                         Uncertainty Lab Day 2

8.                                                         Significant Figures                  Assignment # 5

9.                                                         Unit Analysis 1                        Assignment # 6

10.                                                       Unit Analysis 2                        Assignment # 7

11.                                                       Review                                    Assignment # 8

12.                                                       Practice Test

Assignment # 1           Safety and Review

Complete the safety map for the room by indicating the location of the fire   extinguishers,             doors, eyewash,                     , fire blanket,             , eye-goggles, broken glass container,         soap dispensers,         paper towel dispensers, and   soap sprayers. This is like a treasure hunt. Get up and look for everything.

 Room #

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.

*For those that start with H (covalent compounds) the two largest formulas are solids, the next three larger formulas are liquids, and the three smallest are gases.

The last one, which you can drink, is a liquid.

 Li Mg Al NH4 Na Ba K Ca *H OH 1 2 3 4 5 6 7 8 9 SO4 10 11 12 13 14 15 16 17 18 Br 19 20 21 22 23 24 25 26 27 F 28 29 30 31 32 33 34 35 36 NO3 37 38 39 40 41 42 43 44 45 PO4 46 47 48 49 50 51 52 53 54 S 55 56 57 58 59 60 61 62 63 C2O4 64 65 66 67 68 69 70 71 72 Cr2O7 73 74 75 76 77 78 79 80 81

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Chemical Equations from Word Equations

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

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.

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

Assignment # 2           Physical Chemical Changes Balancing Equations

Classify as a physical or chemical change.

1.         Spoiling of food

2.         Vaporization of ice

3.         Stretching of a rubber band

4.         Dynamite explosion

5.         Shattering of glass

7.         Extraction of iron from form (Fe2O3)

8.         Spontaneous combustion of oily rags

9.         Grinding of wheat

10.       Melting snow

11.       2 H2O  →2 H2 + O2    +     Energy

12.       E    +     NaCl(s)        NaCl(aq)

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

mp                   bp                    physical state

a)         Mercury

b)         Bromine

c)         Chlorine

Classify as a physical or chemical properties.

14.       Sugar chars when heated

15.       Yellow color of sulphur

16.       Tarnishing ability of sulphur

17.       Flexibility of a spring

18.       Thermal conductivity of iron

19.       Hardness of a diamond

20.       Stability of nitrogen

21.       Describe 11 and 12 as exothermic or endothermic

Write Ionic Formulas

22.       Aluminum oxide

23.       Aluminum chloride

24.       Ammonium acetate

25.       Barium phosphate

26.       Calcium hydroxide

27.       Sodium hydroxide

28.       Strontium phosphate

29.       Iron II phosphate

30.       Cobalt III sulphate pentahydrate

31.       Copper II nitrate hexahydrate

Write a balanced equation and include all phase symbols

32.       Sodium chloride dissolving in water (endothermic).

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

34.       List three chemical and physical properties.

Assignment # 2           Classifying Matter And Balancing Equations

1.         Label each as chemical or physical.

a)         Ice cubes turn to water

b)         Steam forms water droplets in a mirror

c)         Milk is made into ice milk

d)         Ice cubes shrink in a freezer

e)         Perspiration “dries”

f)         Bromine is liquefied from solid bromine

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

a) Rain

b) Snow

c) Frost

d) Steam

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.

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

a)         Photosynthesis (CO2+H2O→Sugar+oxygen)

b)         Antifreeze boils out of a radiator

c)         A firefly emits light

d)         A nail is magnetized

e)         A nail rusts

f)         Leaves turn color in autumn

g)         Food spoils

h)         Dynamite explodes

I)         Grinding of wheat into flour

j)         Shattering of glass

k)         Extraction of iron from iron ore (Fe2O3)

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

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

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

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

a)         Methane  (CH4)

b)         Pizza

c)         Milk shake

d)         Zinc

e)         Laughing gas

f)         Clean air

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.

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.

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

Balancing Equations

1.         ___KNO3                                                    ___KNO2        +          ___O2

2.         ___CaC2          +          ___O2                      ___Ca              +          ___CO2

3.         ___C5H12         +          ___O2                      ____CO2         +          ___H2O

4.         ___K2SO4             +          ­___BaCl2                 ____KCl         +          ___BaSO4

5.         ___KOH          +          ___H2SO4                ____K2SO4      +          ___H2O

6.         ___Ca(OH)2    +          ___NH4Cl               ____ NH4OH   +          ___CaCl2

7.         ___C   +          ___SO 2                                           ___CS2            +          ___CO

8.         ___Mg3N2             +          ­___ H2O                  ____ Mg(OH)2     +     ___NH3

9.         ___V2O5          +          ___Ca                      ___CaO           +          ___V

10.       ___Na2O2              +          ­___H2O                   ____NaOH      +          ___O2

11.       ___Fe3O4         +          ___H2                      ____Fe            +          ___H2O

12.       ___Cu  +          ___H2SO4              ____CuSO4       +       ___H2O    +    ___SO 2

13.       ___Al  +          ___H2SO4                            ____ H2           +          ___ Al2(SO4)3

14.       ___Si4H10        +          ___O2                      ___SiO2           +          ___H2O

15.       ___NH3           +          ___O2                      ___N2H4          +          ___H2O

16.       ___C15H30        +          ___O2                      ___CO2           +          ___H2O

17.       ___BN             +          ___F2                                   ___BF3                    +          ___N2

18.       ___CaSO4 . 2 H2O       +   ___SO3                   ___CaSO4   +          ___H2SO4

19.       ___C12H26        +          ___O2                      ___CO2           +          ___H2O

20.       ___C7H6O3      +          ___O2                      ___CO2           +          ___H2O

21.       ___Na             +          ___ZnI2                           ___NaI                        +          ___NaZn4

22. ___LiAlH4             +      ___BF3                   ___LiF       +  ___AlF3    +   ___B2H6

23. ___HBrO3             +       ___HBr                      ___H2O           +     ____Br2

24. ___O2        +      ___All4C3   +       ___H2O                   ___Al(OH)3   +   ___CH4

25. ___Ca(NO3)2 . 3H2O  +  ___LaC2          Ca(NO3)2   +  ___La(OH)2    +   ___C2H2

26. ___CH3NO2   +   ___Cl2           ___CCl3NO2       +         ___HCl

27. ___Ca3(PO4)2   +   ___SiO2   +   ___C         ___CaSiO3   +   ___CO   +   ___P

28. ___Al2C6   +   ___H2O                                 ___Al(OH)3   +   ___C2H2

29. ___NaF   +   ___CaO   +   ___H2O              ___CaF2   +   ___NaOH

30. ___LiH   +   ___AlCl3                                  ___LiAlH4             +          ___LiCl

31. ___CaF2   +   ___H2SO4   +   ___SiO2         ___CaSO4   +  ___SiF4   +   ___H2O

32. ___CaSi2   +   ___SbCl3                   ___Si   +   ___Sb   +   ___CaCl2

33. ___TiO2   +   ___B4C   +   ___C                  ___TiB2   +   ___CO

34. ___NH3                 +          ___O2                      ___NO   +   ___H2O

35. ___SiF4     +           ___NaOH                      ___Na4SiO4   +   ___NaF   +   ___H2O

36. ___NH4Cl             +   ___CaO                     ___NH3   +   ___CaCl2   +   ___H2O

37. ___NaPb                           +   ___C2H5Cl                ___Pb(C2H5)4   +   ___Pb   +   ___NaCl

38. ___Be2C                +   ___H2O                     ___Be(OH)2   +   ___CH4

39. ___NpF3   +   ___O2   +   ___HF                 ___NpF4   +   ___H2O

40. ___NO2                 +   ___H2O                     ___HNO3   +   ___NO

Some Tough Ones

___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 # 3           Balancing Equations

1.         ___Al  +          ___HCl                               ___AlCl3         +          ___H2

2.         ___Zn  +          ___KOH                              ___K2ZnO2   +             ___H2

3.         ___B2O3          +          ___Mg                     ___MgO          +          ___B

4.         ___C6H11OH   +          ___O2                      ___H2O  +       ___CO2

5.         ___C12H26        +          ___O2                       ___HOH   +    ___CO2

6.         ___Na +          ___H2O                               ___NaOH        +          ___H2

7.         ___PbS            +          ___O2                      ___PbO           +          ___SO2

8.         ___SiCl4          +          ___Na                     ___Si   +          ___NaCl

9.         ___Mg +          ___CO2                               ___MgO          +          ___C

10.       ___Al  +          ___H2SO4                            ___Al2(SO4)3   +   ___H2

Write Formulas for each

11.               Zinc phosphate

12.               Ammonium carbonate

13.               Iron III oxalate

14.               Copper II tripolyphosphate pentahydrate

15.               Cobalt II borate

16.               Triphosphorus tetroxide

17.               Dicarbon hexachloride

18.               Trisilicon octafluoride

19.               Sodium tetraborate

20.               Aluminum dichromate

21.               Calcium oxide

22.               Silver thiosulphate

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.

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

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

26.       Write an equation for the combustion of sucrose.

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

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

Worksheet # 4           Balancing Equations Naming Formulas

1.         ___Sb  +          ___Cl2                                             ___SbCl5

2.         ___FeCl2               +          ___Cl2                                 ___FeCl3

3.         ___P                +          ___I2                                    ___PI3

4.         ___Na2S          +          ___HCl                   ___NaCl          +          ___H2S

5.         ___NaOH        +          ___FeCl3                 ___NaCl          +          ___Fe(OH)3

6.         ___KOH          +          ___H3PO4                ___K3PO4        +          ___H2O

7.         ___NaOH        +          ___CuSO4               ___Na2SO4   +   __Cu(OH)2

8.         ___HNO3        +          ___Ca(OH)2             ___H2O           +       __Ca(NO3)2

9.         ___NH3           +          ___CuO      ___H2O           +   ___Cu        +   ___N2

10.       ___N2  +    ___C    +___Na2CO3                 ___NaCN  +    ___CO

11.       ___NH3           +          ___O                       ___NO +          ___H2O

12.       ___NH3           +          ___O2                      ___NO2           +          ___H2O

13.       ___NH3           +          ___O2                      ___N2O5          +          ___H2O

14.       ___P                +          ___N2O                   ___P2O5           +          ___N2

15.       ___Al  +          ___HCl                               ___AlCl3         +          ___H2

16.       ___Zn  +          ___KOH                              ___K2ZnO2   +             ___H2

17.       ___B2O3          +          ___Mg                     ___MgO          +          ___B

18.       ___CH3OH      +          ___O2                      ___H2O           +          ___CO2

19.       ___C6H12O6                                                 ___C2H5OH   +    ___CO2

20.       ___Na +          ___H2O                               ___NaOH        +          ___H2

21.       ___PbS            +          ___O2                      ___PbO           +          ___SO2

22.       ___SiCl4          +          ___Na                     ___Si   +          ___NaCl

23.       ___Mg +          ___CO2                               ___MgO          +          ___C

24.       ___Al  +          ___H2SO4                            ___Al2(SO4)3   +   ___H2

Write balanced chemical formulas for each ionic compound.

25.       Calcium hydroxide

26.       Aluminum sulphate

27.       Iron III oxide

28.       Zinc acetate

29.       Barium carbonate

30.       Sodium phosphate

31.       Cobalt II nitride

32.       Gallium sulphate

33.       Aluminum fluoride

34.       Ammonium sulphate

35.       Aluminum acetate

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

36.       carbon monoxide

37.       dinitrogen tetraiodide

38.       triphosphorus  hexafluoride

39.       dinitrogen  dioxide

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.

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

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

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

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

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

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

You are good if you can do these.

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

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

Worksheet # 5           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

25.64V

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

3.         Determine the average and uncertainty for the data:

5.216 oC          5.218 oC          5.213 oC          5.214 oC          5.416 oC

4.         How many significant figures are in each number?

25.63                                       101                                          0.0075

0.0002                                     1.00                                         2.005

10.031                                     1.0002                                     10005

0.00521                                   2.51 x 104                                3 x 10-7

2 x 105                                     2.00 x 103                                250.

5.         Round off to three significant figures.

0.05211                                                           0.0087251

85.337                                                             2.6177 x 10-5

2.5175 x 10-18                                                                                   25.731 x 105

Round off each measured number to three significant figures.

6.         0.002567

7.         94549

8.         15.00

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

a)         35.234                                                 b)         2.34521

c)         0.035219                                             d)         2533521

e)         6255520000

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

a)         305                                          b)         25.25

c)         3.00                                         d)         0.001

e)         3.0050                                                            f)         6.25 x 1023

g)         7.00 x 10-2                               h)         1001

11.       Add or subtract the measured quantities.

25.31                  22.0                          22.7                             35.271

+   6.4              +   0.04                    +    0.77                      +     0.2

22.71                25.217                        2.51639                       8.0558

- 0.299             + 0.017                  -     1.2358                    +   0.3259297

25.634   +  2.365  -   0.25498  +  0.225  =

12.       15.239  +  5.36

13.       2.6679   -    1.23

14.       2.059378  x  1024    +   5.3    x   1022

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

16.       2.3  x  10 16    +   8.224    x   1019

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

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

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

Assignment # 6

1.         25  x 3

2.          3.35  x  0.26

3.         799  x  877

4.         (6.2 x 103)( 3.55 x 1012)

5.         (6.3 x 107)(2.51 x 10-7)

(3.214 x 10-5)

6.         (7.52 x 1016)(3.1 x 1012)

7.         3.5 x 102  ÷  3.1 x 103

(2.5 x 10-7)

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)

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)

10.       156   x   256   x  21   x  0.0005687                                                                                             0.02569   x   13.235   x   2654

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)

12.       25.7 x  0.21

13.       35 x 105

14.       51.71 x  22.3

15.       22 x 305

16.       Write three examples of exact numbers.

17.       Write three examples of approximate numbers.

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

22.          26.215                      23.    65.222                            24.    22  -  0.01

-  0.3                                  +  1.03

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

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

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

58.56 g

58.59 g

58.51 g

58.61 g

58.57 g

58.56 g

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

123.2

124.5

124.0

124.3

124.3

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

a)         0.00200 L                                b)         5.000 g

c)         1.00003 A                               d)         1000.000 Mm

e)         2.5 x 1076                                                         f)         78.89 m

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

a)         18. + 0.21

b)         62.1  x  3021.56

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

d)         (9.442 x 10-3)(3.21 x 108)

e)         231.4  -  8.2295

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

g)         12.0355 + 1.024

h)         (4.56 x 10-8)(2.5  x 1035)

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

33.       State the difference between accuracy and precision.

Worksheet # 7                       Unit Analysis 1

1.         527 g to mg

2.         1.05  x  106 um to m

3.         2.148 ML to mL

4.         0.0235 mg to kg

5.         8.32  x 10-4  mL  to ML

6.         772.5 us to ms

7.         3.06500 cg to Kg

8.         9.450 Mm to mm

9.         5.64  x  103  mm2 to cm2

Non-metric/Metric Conversions

Given that:                   2.210 lb =  1.00  kg                             4.54 L = 1.00 Gal

1.000 atm = 101.3 kPa            1.61 km = 1.00 mile

14 lb = 1 stone                                    2000 lb = 1 ton

16 oz = 1 lb

10.       170. lb to kg

11.       648 kPa to atm

12.       256 oz to tons

13.       0.025 ton to mg

14.       0.236 Gal to mL

15.       5.8 x 106 mL to Gal

16.       5.66 x 106 mg to stones

17.       15 miles to mm

18.       5.63 x 109 µm to miles

Worksheet # 8                       Unit Analysis 2

1.         605 µm  to mm

2.         6.5  x  10-6   Mm  to m

3.         20.0 Km  to cm.

4.         8.774  x  1015  µm to Mm.

5.         25 cL  to  ML

6.         648 KPa  to  mPa

7.         2.665 Mg  to  µg

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)

8.         152 mL to gal

9.         8.6 stone to oz

10.       4.3 m to miles

12.       15.2 mi/gal to L/km

13.       2.3  gal to mL

14.       45.2 oz to stones

15.       46.3 miles to m

16.       36 L/km to mi/gal

17.       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.

18.       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.

19.       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

6 yams = 10 lbs of figs

Worksheet # 9           Unit Analysis and Measurement Review

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

Assume all of the conversions have the number of significant figures indicated.

Convert:

1.         \$300.00 Can. to Ł.

2.         \$1025.00 Can. to pesos.

3.         \$450.00 U.S. to yen.

4.         Ł 652.23 to francs.

5.         85.2 Marks to Ł.

6.         3842.35 Yen to Rupees.

7.         9668.75 Francs to Marks

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.

2.         10. CDs to tickets.

3.         100. Buttons converted to CDs.

4.         1 Back Stage Pass converted to T Shirts.

5.         280. Posters to Back Stage Passes.

6.         6 Back Stage Passes to buttons.

7.         6.372 hL to mL

8.         4.9 x 1015 µg to Mg

9.         8.774 x 103 cm3 to 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

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

a)  25.0 g                                       b)       1000 g = 1 kg

c)  25.036 A                                  d)  5.214  x  10-62  mL

e) 0.0000005 L                              f) 8.2000 m

Determine the average and uncertainty given the following measurements from a

12.       Centigram balance

82.62 g

82.54 g

82.48 g

82.72 g

82.65 g

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

Write chemical formulas for each ionic or molecular compound.

14.       Iron III oxide

15.       Triphosphorous hexoxide

16.       Aluminum hydroxide

17.       Nickel II phosphate octahydrate

Name each chemical formula

11.       K3PO4

12.       Mn3P2

13.       Ga2(SO3)2 . 6H2O

14.       P4O10

Worksheet # 10                     Unit 1 Practice Test

Balance each equation.

1.         ___Sb              +          ___Cl2             ®        ___SbCl5

2.               ___NH3           +          ___O2             ®        ___N2O5          +          ___H2O

3.         ___C12H26        +          ___O2              ®        ___CO2           +          ___H2O

4.         ___Al     +    ____H2SO4            ®        ____H2 + ____Al2(SO4)3

(The next one is the tough one!!)

5.         ___Cu    +    ____HNO3          ® ____Cu(NO3)2   + ____NO +____H2O

.

6.         Barium phosphate plus sodium sulphate (both in water) yields solid barium sulphate and aqueous sodium phosphate. Write a balanced equation with phase symbols

Write chemical formulas for each ionic or molecular compound.

7.         Mercury II sulfide

8.         Diphosphorous pentoxide

9.         Barium hydroxide

10.       Copper II sulphate hexahydrate

Name each chemical formula

11.       Na3PO4

12.       Co3P2

13.       Al2(CO3)2 . 6H2O

14.       Si2I6

15.       Determine the average and uncertainty for the data:

25.56g

25.54g

25.52g

25.53g

25.55g

16.       Determine the average and uncertainty for the data:

5.216 oC

5.218 oC

5.213 oC

5.214 oC

5.416 oC

Round off each measured number to three significant figures.

17.       0.002567

18.       94549

19.       15.00

Add or subtract the measured quantities.

20.       15.239  +  5.36

21.       2.6679   -    1.238

22        12.65449   +   0.2493

23.       8.57  x  107   +   5.37894    x   109

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

24.         156   x   256   x  21   x  0.0005687

.02569   x   13.235   x   2654                      Answer

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)

Complete the relationships:

26.                     Mg     =               g                 27.                     km     =               m

28.                     L        =               mL              29.                     g        =               ng

30.                     µs      =               s                 31.                     cg       =               g

32.                    pg       =               g                 33.                     s        =               Ts

Use unit analysis to perform the following conversions:

34.       8.13 kg to cg.

35.       2.3 x 1012 µm to Mm.

36.       1.52 x 104 Mm to mm.

37.       2.13 Mg to cg.

38.       8.88 x 1012 mm to Mm.

39.       8.52 x 10-8 Mm to 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

41.       3.8 stone to oz

42.       25.6 m to miles

43.       26 mi/gal to L/km

44.       14.5 L/km to mi/gal

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?

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

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

4 Wendy’s burger = 7 tacos                            6 lime jello cups = 3 bags of Doritos

1 bowl of lime jello = 1000 brussel sprouts

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

46.

47.

48.

49.

50.

51.       Micrometer Scale in cm.

52.       Vernier Scale in cm.