Chemistry Name __________________________

Hour _______

Chemistry

Approximate Timeline

Students are expected to keep up with class work when absent.

CHAPTER 5 – MEASUREMENTS & CALCULATIONS

Day Plans for the day Assignment(s) for the day

1 Begin Chapter 5

5.2 – Counting sig figs

o Discuss 4 rules for counting sig. figs.

Assignment 5.0

Assignment 5.2a

2 5.2 – Math w/sig figs Assignment 5.2b

Read section(s) 5.1

3 Quiz 5.2 – Significant Figures

5.1 – Scientific Notation

o Writing decimal numbers in scientific

notation

o Writing scientific notation as a decimal

number

o Math with scientific notation

Assignment 5.1a

Assignment5.1b

Read section(s) 5.3

4 Quiz 5.1 – Scientific Notation

5.3 – Unit conversions – English

Assignment 5.3a due tomorrow

Assignment 5.3a

5 5.3 – Unit conversions – Metric

o single units (m cm)

o unit3 (cm

3 m

3)

Assignment 5.3b

Assignment 5.3c

6 Quiz 5.3.1 – Metric Equivalents 1

5.3 – Unit conversions – Metric

o unit/unit (g/cm3 kg/m

3)

Assignment 5.3d

7 Quiz 5.3.1 – Metric Equivalents 2 (if

needed)

5.3 – Unit conversions – Temperature

Assignment 5.3e

8 Quiz 5.3.4.1 – Metric Equivalents 3 (if

needed)

5.3 – Unit conversions – Density

Assignment 5.3f

9 Quiz 5.4 – Dimensional Analysis

Discuss Density Lab

10 Perform Density Lab

Lab Report due in 2 days

Assignment 5.4

11 Grade & discuss Assignment 5.4

Review for the Chapter 5 Test

12 Chapter 5 Test Read section(s) 6.1

Chemistry Name __________________________

Hour _______

Study Guides

Chapter 5 Reading Quizzes

Chemistry

Quiz 5.1 Scientific Notation & Units 1. A measurement always contains what two parts?

2. Scientific notation expresses a number as a ___ and a ___.

3. Convert a decimal number into scientific notation.

4. Which system of measurement is used by scientists all over the world?

5. Give the fundamental unit of:

a. mass

b. length

c. time

d. temperature

6. Give the metric prefix that means:

a. 1000

b. 1/10

c. 1/100

d. 1/1000

Quiz 5.2 Uncertainty in Measurements… 7. What do we mean when we say that a measurement always has a degree of uncertainty?

8. How is the degree of uncertainty for a particular measurement recorded?

9. Memorize the “Rules for Counting Significant Figures” on page 136.

10. Indicate the number of significant digits in a number.

11. Calculate and round your answer to the correct number of significant digits.

Quiz 5.3a Problem Solving and Unit Conversions 12. Define the term “conversion factor”.

13. Give on example of an “equivalence statement”.

14. What is “dimensional analysis”?

15. Use dimensional analysis to perform several unit conversions.

Quiz 5.3b Problem Solving and Unit Conversions 16. Define the term “density”.

17. Be able to solve density problems.

18. Be able to convert from one temperature scale to another.

Study Guide

Chapter 5 Test

At the completion of chapter 5 you should…

1. Know the definitions of the following terms

a. Measurements

b. Units

c. Scientific Notation

d. Significant Figures

e. Conversion Factor

f. Dimensional Analysis

g. Density

h. Specific Gravity

2. Scientific notation

a. Be able to write numbers from decimal notation into scientific notation

b. Be able to write numbers from scientific notation into decimal notation

3. Significant figures

a. Be able to count the number of significant figures in a measurement

b. Be able to express the answer to a calculation with the correct number of

significant figures

4. Unit conversions

a. Use the correct conversion factor to convert from one unit to another

b. Use dimensional analysis to solve problems

c. Be able perform temperature conversions

i. Fahrenheit to Celsius

ii. Celsius to Fahrenheit

iii. Celsius to Kelvin

iv. Kelvin to Celsius

5. Density

a. Be able to solve all type of density problems

Chemistry Name __________________________

Hour _______

Assignment 5.0 – Vocabulary

Define each of the following terms.

1. Measurement

2. Units

3. Scientific Notation

4. Significant Figures

5. Conversion Factor

6. Dimensional Analysis

7. Density

8. Specific Gravity

Chemistry Name __________________________

Hour _______

Assignment 5.2a – Significant Digits

Indicate the number of significant figures in each of the following.

1) 519 ____________

2) 0.19 ____________

3) 659.42 ____________

4) 2.0050 ____________

5) 0.04 ____________

6) 0.0498 ____________

7) 63500 ____________

8) 0.10082 ____________

9) 5000 ____________

10) 0.0000027 ____________

11) 0.00123 ____________

12) 14700 ____________

Chemistry Name __________________________

Hour _______

Assignment 5.2b – Math with Significant Digits

Solve each of the following problems. Your answer should be rounded to the correct number of

significant figures.

1) 37.76 + 3.907 + 226.4 _____________________

2) 319.15 – 32.614 _____________________

3) 104.632 + 27.09452 + 3.6125 _____________________

4) 20.6 – 3.71 _____________________

5) 3.156 x 4.103 _____________________

6) 12.16 / 3.12 _____________________

7) 1.35 x 2.79 x 4.06 _____________________

8) 0.005763 / 0.0251 _____________________

9) 127.0 x 0.000352 _____________________

10) 1255 + 429.6 + 37.254 _____________________

11) 37.0968 - 17.93724 _____________________

12) 0.00518 / 3.0 _____________________

Chemistry Name __________________________

Hour _______

Assignment 5.1a – Scientific Notation

Express the following numbers in scientific notation. Your answer should contain the correct

number of significant figures.

1) 3,180 _____________________

2) 850,000 _____________________

3) 0.00920 _____________________

4) 0.000539 _____________________

5) 4,120,000 _____________________

6) 395,000,000 _____________________

7) 0.00000826 _____________________

8) 0.00912 _____________________

9) 290.0 _____________________

10) 0.000370 _____________________

Convert each of the following to decimal notation. Your answer should contain the correct

number of significant figures.

11) 4 x 103 _____________________

12) 6.0 x 10-2

_____________________

13) 3.6 x 104 _____________________

14) 5.37 x 10-5

_____________________

15) 4.60 x 10-1

_____________________

16) 3.39 x 106 _____________________

17) 4.90 x 10-1

_____________________

18) 3.68 x 100 _____________________

19) 1.20 x 10-3

_____________________

20) 3.27 x 104 _____________________

Chemistry Name __________________________

Hour _______

Assignment 5.1b – Math with Scientific Notation

Perform the indicated operations. Your answer should be in scientific notation and have the

correct number of significant digits.

1) (2 x 103) x (3 x 10

4) ________________________

2) 7.2 x 104 / 8.6 x 10

5 ________________________

3) 4.26 x 105 – 1.46 x 10

5 ________________________

4) 3.5 x 103 + 2.5 x 10

3 ________________________

5) 9.00 x 10-5

/ 3.00 x 10-3

________________________

6) 6.4 x 109 / 3.60 x 10

7 ________________________

7) (1.6 x 102) x (2.8 x 10

4) ________________________

8) 9.7 x 10-3

/ 1.8 x 104 ________________________

9) 6.4 x 104 – 8.3 x 10

3 ________________________

10) 7.3 x 10-5

– 6.1 x 10-6

________________________

11) (3.7 x 104) x (8.2 x 10

2) ________________________

7.29 x 105

12) (2.5 x 10-2

) x (2.0 x 10-3

) ________________________

5.00 x 103

13) (7.1 x 104) x (2.6 x 10

-2) ________________________

(1.23 x 102) x (4.45 x 10

-1)

14) (2.702 x 10-11

) x (8.27 x 108) ________________________

(1.15 x 107) x (5.45 x 10

-4)

15) (6.02 x 1011

) x (1.09 x 106) ________________________

(3.7 x 105) x (7.159 x 10

14)

16) (2.0 x 102) x (3.0 x 10

3) ________________________

(4.0 x 10-4

) x (5.0 x 10-5

)

Chemistry Name __________________________

Hour _______

Assignment 5.3a – Dimensional Analysis (1)

Perform the following conversions. You must use dimensional analysis! Express your answer

with the correct number of significant digits and units.

1) 18 inches to yards

2) 2.400 miles to yards

3) 11.6 quarts to gallons

4) 6.20 miles to inches

5) 0.234 hours to seconds

Extra Credit

6) 3.64 x 1011

seconds to centuries

Chemistry Name __________________________

Hour _______

Assignment 5.3b – Dimensional Analysis (2)

Perform the following conversions. You must use dimensional analysis! Express your answer

with the correct number of significant digits and units.

1) 5.21 hours to seconds

2) 12.6 meters to centimeters

3) 79.1 centigrams to milligrams

4) 73.18 mg to g

5) 6189 nm to cm

6) 0.49 g to mg

7) 450 milligrams to grams

8) 3.62 grams to centigrams

9) 250.0 milliliters to liters

10) 5,280 centimeters to meters

Chemistry Name __________________________

Hour _______

Assignment 5.3c – Dimensional Analysis (3)

Perform the following conversions. You must use dimensional analysis! Express your answer

with the correct number of significant digits and units.

1) 228 dm3 to L

2) 50.0 mL to cm3

3) 159 cm3 to dm

3

4) 0.00587 L to cm3

5) 3.12 dm3 to cm

3

6) 100.0 cm3to L

7) 456 dm3 to cm

3

8) 761 cm3 to dm

3

9) 50.0 L to dm3

10) 1.40 cm3 to mL

Chemistry Name __________________________

Hour _______

Assignment 5.3d – Dimensional Analysis (4)

Perform the following conversions. You must use dimensional analysis! Express your answer

with the correct number of significant digits and units.

1) 956 mg/cm3 to g/cm

3

2) 220 dm3/sec to L/min

3) 20.5 L/min to cm3/sec

4) 2.0 kg/L to mg/cm3

5) 21.40 nm/sec to cm/min

6) 65.0 cm3/sec to dm

3/min

7) 570 cg/cm3 to g/dm

3

8) 52.0 kg/dm3 to mg/cm

3

9) 0.400 g/cm3 to kg/dm

3

10) 0.640 g/mL to kg/L

Chemistry Name __________________________

Hour _______

Assignment 5.3e – Temperature Conversions (2 pages)

Solve each of the following problems. In order to receive full credit you must do three things: (1)

write the equation, (2) plug in numbers with units, and (3) express your answer with the correct

number of significant figures and units.

1) 80.0°F to °C

2) 20.0°F to °C

3) 25.0°C to °F

4) -10.0°C to °F

5) 25°C to K

6) -15°C to K

7) 350.0 K to °C

8) 263 K to °C

9) 37.0°C to °F

10) 98°F to °C

11) -35.0°C to K

12) 292 K to °C

Chemistry Name __________________________

Hour _______

Assignment 5.3f – Density

Solve each of the following problems. In order to receive full credit you must do three things: (1)

write the equation, (2) plug in numbers with units, and (3) express your answer with the correct

number of significant digits and units.

1) A rock with mass 85.02 g occupies a volume of 20.3 cm3. What is the density of the

rock?

2) A student determines the mass and volume of a liquid to be 28.10 g and 35.8 mL

respectively. What is the density of the liquid?

3) The density of chloroform is 1.483 g/mL. What is the mass of 25.00 mL of chloroform?

4) The density of gold is 19.32 g/mL. What is the mass of 100.0 mL of gold?

5) The density of iron is 7.87 g/mL. What is the volume of 250.0 g of iron?

6) The density of aluminum is 2.70 g/mL. What is the volume of 500.0 g of aluminum?

Chemistry Name __________________________

Hour _______

Assignment 5.4 – Chapter Review

NO WORK = NO CREDIT (3 pages)

How many significant digits are in the following measurements?

1) 150 cm ____________

2) 0.250 L ____________

3) 0.035 km ____________

4) 10.00 g ____________

Perform the following calculations. Express your answer with the correct number of significant

digits and units.

5) 12.38 cm + 6.6 cm __________________

6) 125.37 g – 57.4 g __________________

7) 2.50 m x 6.000 m __________________

8) 104.0 g / 30.0 mL __________________

Express the following numbers in scientific notation. Your answer should include the correct

number of significant digits and units.

9) 760 mL ________________________

10) 0.0830 km ________________________

11) 0.000500 L ________________________

12) 96300 kg ________________________

Express the following numbers in decimal notation. Your answer should include the correct

number of significant digits and units.

13) 4.600 x 10-4

g ________________________

14) 7.800 x 102

m ________________________

15) 9.25 x 104 cm ________________________

16) 5.040 x 10-3

L ________________________

Perform the following conversions. You must use dimensional analysis. No work = no credit.

Your answer should include the correct number of significant digits and units.

17) 8.600 m to cm

18) 84.0 cm to dm

19) 250.0 mL to L

20) 176.0 mm to m

21) 47.0 mL to cm3

22) 2.40 dm3 to L

23) 450.0 cm3 to dm

3

24) 2.70 g/cm3 to kg/dm

3

25) 5.47 kg/dm3 to g/cm

3

Chemistry Name __________________________

Hour _______

Solve each of the following problems. In order to receive full credit you must do three things: (1)

write the equation, (2) plug in numbers with units, and (3) express your answer with the correct

number of significant digits and units.

26) Convert -155 ºC to K

27) Convert 52 K to ºC

28) Convert -40.0 ºF to ºC

29) Convert 20.0 ºC to ºF

30) If 89.2 mL of a liquid has a mass of 75.2 g, calculate the liquid’s density.

31) Mercury has a density of 13.6 g/mL. What is the volume of 50.0 g of mercury?

32) Gold has a density of 19.32 g/ml. What is the mass of 50.0 mL of gold?