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2.9: Multimedia Resources for Chapter 2

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Copy and distribute the lesson worksheets. Ask students to complete the worksheets alone or in pairs as a review of lesson content.

About Observations Worksheet

1. Tools for making accurate measurements are essential for a scientist’s work.

A. True
B. False

2. A scientist can make a general conclusion after doing an experiment one time.

A. True
B. False

3. If the results of an experiment do not support the hypothesis, then the experiment was a waste of time.

A. True
B. False

4. Science has played a large role in improving our standard of living.

A. True
B. False

5. Organized science has been a part of human existence for thousands of years.

A. True
B. False

6. Scientists have already found almost all the answers to questions about nature.

A. True
B. False

7. As a rule, men make better scientists than women.

A. True
B. False

8. Scientists have no definite method they can follow when they set out to solve a problem.

A. True
B. False

Identify each of the following observations as quantitative or qualitative.

9. The lamp is light green in color. _______________________

10. The liquid tastes sour. ____________________

11. The longest leaf is 9~ cm long._________________________

12. When you remove the cork, a loud popping sound occurs. _______________________

13. The mass of the computer is 1.5~ kg. _______________________

14. The veins are about 3~ mm wide. _______________________

15. Over time, the solution becomes darker and darker. __________________________

Mass Versus Weight Worksheet

CK-12 Foundation Chemistry

Name___________________________ Date_________

The mass of an object is a measure of the amount of matter in it. The mass (amount of matter) of an object remains the same regardless of where the object is placed. For example, moving a brick to the moon does not cause any matter in it to disappear or be removed. The weight of an object is the force of attraction between the object and the earth (or whatever large body it is resting on). We call this force of attraction, the force of gravity. The gravitational pull on the object varies depending on where the object is with respect to the earth or other gravity producing object. For example, a man who weighs 180 \ pounds on earth would weigh only 45 \ pounds if he were in a stationary position, 4,000 \ miles above the earth's surface. This same man would weigh only 30 \ pounds on the moon because the moon's gravity is only one-sixth that of earth. If this man were in outer space with no planet or moon nearby, his weight would be zero. There would be gravitational pull on him at all. The mass of this man, however, would be the same in all those situations because the amount of matter in him is constant.

We measure weight with a scale, which is a spring that compresses when a weight is placed on it. If the gravitational pull is less, the spring compresses less and the scale shows less weight. We measure mass with a balance. A balance compares the unknown mass to known masses by balancing them on a lever. If we take our balance and known masses to the moon, an object will have the same measured mass that it had on the earth. The weight, of course, would be different on the moon.

On, or near the surface of, the earth, the force of gravity is constant and so we can determine either the mass or the weight of an object if we know one of those two. On or near the surface of the earth, the conversion factor between mass and weight is: 1.00 \ kg of mass will have a weight of 9.80 \ Newtons (the standard unit of force in the SI system).

Example: What is the weight in Newtons of a 3.0 \ kg mass on the surface of the earth?

(\text{gravitational force} = (3.00 \ kg)(9.80 \ N/kg) = 29.4 \ N)

Example: If an object weighs 200. \ N on the surface of the earth, what is its mass?

\text{mass} = (200. \  N) \left (\frac {1.00 \ kg} {9.80 \ N}\right ) = 20.4 \ kg

Exercises

  1. If an object weighs 400. \ N on the earth, how much mass does it contain?
  2. What is the weight, in Newtons, of a 50 \ kg mass on the surface of the earth?
  3. On the surface of the earth, how much mass is contained in a 600. \ N weight?
  4. If an object weighs 1200 \ N on the earth, how much will it weigh on the moon?
  5. If an object has a mass of 120 \ kg on the earth, what is its mass on the moon?

Measurements Worksheet

Name___________________________ Date_________

Measurement makes it possible to obtain more exact observations about the properties of matter such as the size, shape, mass, temperature, or composition. It allows us to make more exact quantitative observations. For example, the balance makes it possible to determine the mass of an object more accurately than we could by lifting the object and a clock gives a better measure of time than we could determine by observing the sun's position in the sky.

Measurements were orginally made by comparing the object being measured to some familiar object. Length was compared to the length of one's foot. Other measures were handspans, elbow to fingertip, and so on. As people's needs increased for more consistent measurements, STANDARD systems of measurement were devised. In a standard system of measurement, some length is chosen to be the standard and copies of this object can then be used by everyone making measurements. With a standard system of measurement, two people measuring the same distance will get the same measurement.

For a time, the standard for length (one meter) was a platinum bar which was marked and stored at constant temperature in a vault. It was stored at constant temperature so that it did not expand or contract. Standard masses are also stored in airtight containers to insure no change due to oxidation. Presently, the standard meter is the distance light travels in a vacuum in  \frac {1}{299,792,458} second and the standard second is based on the vibrations of a cesium -133 atom.

For any system of measurements, all measurements must include a unit term; a word following the number that indicates the standard the measurement is based on. Systems of measurement have several standards such as length, mass, and time, and are based on physical objects such as platinum bars or vibrating atoms. Standards based on physical objects are called undefined units. All the other standards are expressed in terms of these object-based standards. For example, length and time are object-based standards and velocity (meters/second) and acceleration (m/s_2) are expressed in terms of length and time. Volume is expressed in terms of the length standard, volume = length \times length \times length, such as cm^3.

There are two major systems of standards used in the United States. The one commonly used by the public (pounds, feet) and the system used for all scientific and technical work (kilograms, meters). The system used for scientific work is called the Metric System in its short form and is called the International System (SI) in its complete form. The undefined units in the SI system are the meter, gram, and second. All the sub-divisions in the SI system are in decimal form.

Conversion Factors, English to Metric

1.00 \ inch = 2.54 \ centimeters

1.00 \ quart = 0.946 \ liter

1.00 \ pound = 4.54 \ Newtons \ (= 454 \ grams on earth)

Units and Sub-Divisions for the SI System

Basic unit for length = meter

Basic unit for mass = gram

Basic unit for time = second

Unit for volume = liter (lee-ter)

1000 \ millimeters = 1 \ meter

100 \ centimeters = 1 \ meter

1000 \ meters = 1 \ kilometer

10 \ centimeters = 1 \ millimeter

1000 \ milligrams = 1 \ gram

1000 \ grams = 1 \ kilogram

1000 \ milliliters = 1 \ liter

1 \ milliliters = 1 \ cubic \ centimeter = 1 \ cm^3

All the relationships between units are defined numbers and therefore, have an infinite number of significant figures. When converting units, the significant figures of the answer are based on the significant figures of the measurement, not on the conversion factors.

The unit terms for measurements are an integral part of the measurement expression and must be carried through every mathematical operation that the numbers go through. In performing mathematical operations on measurements, the unit terms as well as the numbers obey the algebraic laws of exponents and cancellation.

Examples:

Unit Terms Follow the Rules of Algebra
Math Operations Unit Term Operations
6x + 2x = 8x 6 \ mL + 2 \ mL = 8 \ mL
(5x)(3x) = 15x^2 (5 \ cm)(3 \ cm) = 15 \ cm^2
 \frac {9x^3}{3x} = 3x^2  \frac{9 \ cm^3}{3\ cm} = 3 \ cm^2
 \frac{21x}{3a} = 7( \frac{x}{a})  \frac{21 \ grams}{3 \ cm^3} = 7 \ \frac{grams}{cm^3}

Converting Units

Frequently, it is necessary to convert units measuring the same quantity from one form to another. For example, it may be necessary to convert a length measurement in meters to millimeters. This process is quite simple if you follow a standard procedure called unit analysis. This procedure involves creating a conversion factor from equivalencies between various units.

For example, we know that there are 12 \ inches in 1 \ foot. Therefore, the conversion factor between inches and feet is 12 \ inches = 1 \ foot. If we have a measurement in inches and we wish to convert the measurement to feet, we would generate a conversion factor  \left (\frac {1 \ foot} {12 \ inches}\right ) and multiply the measurement by this conversion factor.

Example: Convert 500. \ inches to feet.

(500. \ inches)\left (\frac{1 \ foot}{12 \ inches}\right ) = 41.7 \ feet

We design the conversion factor specifically for this problem so that the unit term “inches” will cancel out and the final answer will have the unit “feet”. This is how we know to put the unit term “inches” in the denominator and the unit term “foot” in the numerator.

Example: Convert 6.4 \ nobs to hics given the conversion factor, 5 \ hics = 1 \ nob.

(6.4 \ nobs)\left (\frac {5 \ hics}{1 \ nob}\right ) = 32 \ hics

Example: Convert 4.5 \ whees to dats given the conversion factor, 10 \ whees = 1 \ dat.

(4.5 \ whees)\left (\frac {1 \ dat}{10 \ whees}\right ) = 0.45 \ dats

Sometimes, it is necessary to insert a series of conversion factors.

Example: Convert 5.00 \ wags to pix given the conversion factors, 10 \ wags = 1 \ hat, and 1 \ hat = 2 \ pix.

(5.00 \ wags)\left (\frac{1 \ hat}{10 \ wags}\right )\left (\frac{2 \ pix} {1 \ hat}\right ) = 1.00 \ pix

Solved Conversion Problems

1. Convert 1.22 \ cm to mm.

(1.22 \ cm)\left (\frac{10 \ mm}{1 \ cm}\right ) = 12.2 \ mm

2. Convert 5.00 \ inches to mm.

(5.00 \ inches)\left (\frac{2.54 \ cm}{1 \ inch}\right )\left (\frac {10 \ mm} {1 \ cm}\right ) = 127 \ mm

3. Convert 66 \ lbs to kg. As long as the object is at the surface of the earth, pounds (force) can be converted to grams (mass) with the conversion factor 454 \ g = 1 \ lb.

(66 \ lbs)\left (\frac{454 \ g}{1 \ lb}\right )\left (\frac{1 \ kg} {1000 \ g}\right ) = 30. \ kg

The mathematical answer for this conversion comes out to be 29.964 but must be rounded off to two significant figures since the original measurement has only two significant figures. When 29.964 is rounded to two significant figures, it requires a written in decimal after the zero to make the zero significant. Therefore, the final answer is 30. \ kg.

4. Convert 340. \ mg/cm^3 to lbs/ft^3.

 \left (\frac {340. \ mg} {1 \ cm^3}\right )\left (\frac {1 \ g}{1000 \ mg}\right )\left (\frac{1 \ lb}{454 \ g}\right )\left (\frac {16.39 \ cm^3}{1 \ in^3}\right )\left (\frac {17.28 \ in^3} {1 \ ft^3}\right ) = 21.2 \ lbs/ft^3

You should examine the units yourself to make sure they cancel and leave the correct units for the answer.

Exercises

  1. Convert 40. \ cots to togs given the conversion factor, 10 \ cots = 1 \ tog.
  2. Convert 8.0 \ curs to nibbles given the conversion factor, 1 \ cur = 10 \ nibbles.
  3. Convert 100. \ gags to bobos given the conversion factor, 5 \ gags = 1 \ bobo.
  4. Convert 1.0 \ rat to utes given the conversion factors, 10 \ rats = 1 \ gob and 10  \ gobs  = 1 \ ute.
  5. Express 3.69 \ m in cm.
  6. Express 140 \ mm in cm.
  7. Convert 15 \ inches to mm.
  8. Express 32.0 \ grams in pounds. (Be aware that such a conversion between weight and mass is only reasonable on the surface of the earth.)
  9. Express 690 \ mm in m.
  10. Convert 32.0 \ lbs/qt to g/mL.
  11. Convert 240. \ mm to cm.
  12. Convert 14,000 \ mm to m.

Significant Figures Worksheet

Name___________________________ Date_________

Working in the field of science almost always involves working with numbers. Some observations in science are qualitative and therefore, do not involve numbers, but in chemistry, most observations are quantitative and so, require numbers. You have been working with numbers for many years in your math classes thus numbers are not new to you. Unfortunately, there are some differences between the numbers you use in math and the numbers you use in science.

The numbers you use in math class are considered to be exact numbers. When you are given the number 2 in a math problem, it does not mean 1.999 rounded to 2 nor does it mean 2.000001 rounded to 2. In math class, the number 2 means exactly 2.00000000... with an infinite number of zeros - a perfect 2! Such numbers are produced only by definition, not by measurement. That is, we can define 1 \ foot to contain exactly 12 \ inches, and these two numbers are perfect numbers, but we cannot measure an object to be exactly 12 \ inches long. In the case of measurements, we can read our measuring instruments only to a limited number of subdivisions. We are limited by our ability to see smaller and smaller subdivisions, and we are limited by our ability to construct smaller and smaller subdivisions. Even using powerful microscopes to construct and read our measuring devices, we eventually reach a limit, and therefore, even though the actual measurement of an object may be a perfect number of inches, we cannot prove it to be so. Measurements do not produce perfect numbers and since science is greatly involved with measuring, science does not produce perfect numbers (except in defined numbers such as conversion factors).

It is very important to recognize and report the limitations of measurements along with the magnitude and unit of the measurement. Many times, the analysis of the measurements made in a science experiment is simply the search for regularity in the observations. If the numbers reported show the limits of the measurements, the regularity, or lack there of, becomes visible.

Two Sets of Observations
Observations List A Observations List B
22.41359 \ m 22.4 \ m
22.37899 \ m 22.4 \ m
22.42333 \ m 22.4 \ m
22.39414 \ m 22.4 \ m

In the lists of observations above, it is difficult to perceive a regularity in List A, but when the numbers are reported showing the limits of the measurements as in List B, the regularity becomes apparent.

One of the methods used to keep track of the limit of a measurement is called Significant Figures. In this system, when you record a measurement, the written number must indicate the limit of the measurement, and when you perform mathematical operations on measurements, the final answer must also indicate the limit of the original measurements.

To record a measurement, you must write down all the digits actually measured, including measurements of zero and you must NOT write down any digit not measured. The only real problem that occurs with this system is that zeros are sometimes used as measured numbers and are sometimes used simply to locate the decimal point and ARE NOT measured numbers.

In the case shown above, the correct measurement is greater than 1.2  \ inches but less than 1.3 \ inches. It is proper to estimate one place beyond the calibrations of the measuring instrument. Therefore, this measurement should be reported as either 1.23, 1.24, 1.25, 1.26, or 1.27 \ inches.

In this second case, it is apparent that the object is, as nearly as we can read, exactly at 1 \ inch. Since we know the tenths place is zero and can estimate the hundredths place to be zero, the measurement should be reported as 1.00 \ inch. It is vital that you include the zeros in your measurement report because these are measured places.

This is read as 1.13, 1.14, 1.15, or 1.16 \ inches.

This is read 1.50 \ inches.

These readings indicate that the measuring instrument had subdivisions down to the tenths place and the hundredths place is estimated. There is some uncertainty about the last and only the last digit.

In our system of writing significant figures, we must distinguish between measured zeros and place-holding zeros. Here are the rules for determining the number of significant figures in a measurement.

RULES FOR DETERMINING THE NUMBER OF SIGNIFICANT FIGURES

  1. All non-zero digits are significant.
  2. All zeros between non-zero digits are significant.
  3. All beginning zeros are NOT significant.
  4. Ending zeros are significant if the decimal point is actually written in but not significant if the decimal point is an understood decimal.

Examples of the Rules

1. All non-zero digits are significant.

543 has 3 significant figures.

22.437 has 5 significant figures.

1.321754 has 7 significant figures.

2. All zeros between non-zero digits are significant.

7,004 has 4 significant figures.

10.3002 has 6 significant figures.

103.0406 has 7 significant figures.

3. All beginning zeros are NOT significant.

00013.25 has 4 significant figures.

0.0000075 has 2 significant figures.

0.000002 has 1 significant figure.

4. Ending zeros are significant if the decimal point is actually written in but not significant if the decimal point is an understood decimal.

37.300 has 5 significant figures.

33.00000 has 7 significant figures.

1.70 has 3 significant figures.

1,000,000 has 1 significant figure.

302,000 has 3 significant figures.

1,050 has 3 significant figures.

1,000,000. has 7 significant figures.

302,000. has 6 significant figures.

1,050. has 4 significant figures.

Exercises

How many significant figures are given in each of the following measurements?

  1. 454 \ g _____
  2. 2.2 \ lbs _____
  3. 2.205 \ lbs _____
  4. 0.3937 \ L _____
  5. 0.0353 \ L _____
  6. 1.00800 \ g _____
  7. 500 \ g _____
  8. 480 \ ft _____
  9. 0.0350 \ kg _____
  10. 100. \ cm _____
  11. 1,000 \ m _____
  12. 0.625 \ L _____
  13. 63.4540 \ mm _____
  14. 3,060 \ m _____
  15. 500. \ g _____
  16. 14.0 \ mL _____
  17. 1030 \ g ______
  18. 9,700 \ g _____
  19. 125,000 \ m _____
  20. 12,030.7210 \ g _____
  21. 0.0000000030 \ cm _____
  22. 0.002 \ m _____
  23. 0.0300 \ cm _____
  24. 1.00 \ L _____
  25. 0.025 \ m/s _____
  26. 0.100 \ kg _____
  27. 0.00300 \ km _____
  28. 303.0 \ g _____
  29. 250 \ g _____
  30. 1,000. \ m _____

Maintaining Significant Figures Through Mathematical Operations

In addition to using significant figures to report measurements, we also use them to report the results of computations made with measurements. The results of mathematical operations with measurements must include an indication of the number of significant figures in the original measurements. There are two rules for determining the number of significant figures after a mathematical operation. One rule is for addition and subtraction, and the other rule is for multiplication and division. (Most of the errors that occur in this area result from using the wrong rule, so always double check that you are using the correct rule for the mathematical operation involved.

Significant Figure Rule for Addition and Subtraction

The answer for an addition or subtraction problem must have digits no further to the right than the shortest addend.

Example:

& \quad 13.3843 \ cm\\&  \quad \ 1.012 \quad cm\\& \underline{+ \ \ 3.22 \quad \ cm}\\& \quad 17.6163 \ cm = 17.62 \ cm

Note that the vertical column farthest to the right has a 3 in the top number but that this column has blank spaces in the next two numbers in the column. In elementary math lasses, you were taught that these blank spaces can be filled in with zeros, and in such a case, the answer would be 17.6163 \ cm. In science, however, these blank spaces are NOT zeros but are unknown numbers. Since they are unknown numbers, you cannot substitute any numbers into the blank spaces and you cannot claim to know, forsure, the result of adding that column. You can know the sum of adding (or subtracting) any column of numbers that contains an unknown number. Therefore, when you add these three columns of numbers, the only columns for which you are sure of the sum are the columns that have a known number in each space in the column. When you have finished adding these three numbers in the normal mathematical process, you must round off all those columns that contain an unknown number (a blank space). Therefore, the correct answer for this addition is 17.62 \ cm and has four significant figures.

Example:

& \quad 12 \qquad \quad  m\\& \underline{+ \ \ 0.00045 \ m}\\& \quad 12.00045 \  m = 12 \ m

In this case, the 12 has no numbers beyond the decimal and therefore, all those columns must be rounded off and we have the seemingly odd result that after adding a number to 12, the answer is still 12. This is a common occurrence in science and is absolutely correct.

Example:

& \ \quad 56.8885 \ cm\\&  \quad \ \ 8.30 \ \quad cm\\& \underline{+ \ 47.0 \qquad cm}\\& \ \ 112.1885 \  cm = 112.2 \ cm

This answer must be rounded back to the tenths place because that is the last place where all the added numbers have a recorded digit.

Significant Figure Rule for Multiplication and Division

The answer for a multiplication or division operation must have the same number of significant figures as the factor with the least number of significant figures.

Example: (3.556 \  cm)(2.4  \ cm) = 8.5344  \ cm^2 = 8.5 \ cm^2

In this case, the factor 2.4 has two significant figures and therefore, the answer must have two significant figures. The mathematical answer is rounded back to two significant figures.

Example: (20.0 \ cm)(5.0000 \ cm) = 100 \ cm^2 = 100. \ cm^2

In this example, the factor 20.0 \ cm has three significant figures and therefore, the answer must have three significant figures. In order for this answer to have three significant figures, we place an actual decimal after the second zero to indicate three significant figures.

Example:  (5.444 \ cm)(22 \ cm) = 119.768 \ cm^2 = 120 \ cm^2

In this example, the factor 22 \ cm has two significant figures and therefore, the answer must have two significant figures. The mathematical answer is rounded back to two significant figures. In order to keep the decimal in the correct position, a non-significant zero is used.

Exercises

Add, subtract, multiply, or divide as indicated and report your answer with the proper number of significant figures.

1.

& \quad 703 \quad \ \ g\\&  \qquad 7 \quad \ \ g\\& \underline{+ \quad \ 0.66 \ g}

2.

& \qquad 5.624 \ ft\\&  \qquad  0.24 \ \ ft\\& \underline{+ \ \ 16.8 \quad ft}

3.

& \ \ 34 \quad \ kg \\& \underline{- \  0.2 \  kg}

4.

& \ \ 18.7 \quad \ m\\& \underline{+ \ 0.009 \ m}

5. Add 65.23 \ cm, 2.666 \ cm, and 10 \ cm.

6. Multiply 2.21 \ cm and 0.3 \ cm.

7. Multiply: (2.002 \ cm)(84 \ cm)

8. Multiply: (107.888 \ cm)(0.060 \ cm)

9. Divide 72.4 \ cm by 0.0000082 \ cm.

10. Multiply 0.32 \ cm by 600 \ cm and then divide the product by 8.21 \ cm.

Exponential Notation Worksheet

Name___________________________ Date_________

Work in science frequently involves very large and very small numbers. The speed of light, for example, is 300,000,000 \ meters/second; the mass of the earth is 6,000, 000, 000, 000, 000, 000, 000, 000 \ kg; and the mass of an electron is 0.0000000000000000000000000000009 \ kg. It is very inconvenient to write such numbers and even more inconvenient to attempt to carry out mathematical operations with them. Imagine trying to divide the mass of the earth by the mass of an electron! Scientists and mathematicians have designed an easier method for dealing with such numbers. This more convenient system is called Exponential Notation by mathematicians and Scientific Notation by scientists.

In scientific notation, very large and very small numbers are expressed as the product of a number between 1 and 10 and some power of 10. The number 9,000,000, for example, can be written as the product of 9 times 1,000,000 and 1,000,000 can be written as 10^6. Therefore, 9,000,000 can be written as 9 \times 10^6. In a similar manner, 0.00000004 can be written as 4 times  \frac {1}{10^8} or 4 \times 10^{-8}.

Examples
Decimal Notation Scientific Notation
95,672 9.5672 \times 10^4
8,340 8.34 \times 10^3
100 1 \times 10^2
7.21 7.21 \times 10^0
0.014 1.4 \times 10^{-2}
0.0000000080 8.0 \times 10^{-9}
0.00000000000975 9.75 \times 10^{-12}

As you can see from the examples above, to convert a number from decimal to exponential form, you count the spaces that you need to move the decimal and that number becomes the exponent of 10. If you are moving the decimal to the left, the exponent is positive, and if you are moving the decimal to the right, the exponent is negative. One and only one non-zero digit exists to the left of the decimal and ALL significant figures are maintained. The value of using exponential notation occurs when there are many non-significant zeros.

Exercises

Express the following decimal numbers in exponential form. The exponential form should have exactly one non-zero digit to the left of the decimal and you must carry all significant figures.

  1. 1000
  2. 150,000
  3. 243
  4. 9.3
  5. 435,000,000,000
  6. 0.0035
  7. 0.012567
  8. 0.0000000000100
  9. 0.000000000000467
  10. 0.000200
  11. 186,000
  12. 9,000,000,000,000
  13. 105
  14. 77,000
  15. 502,000

Carrying Out Mathematical Operations with Exponential Numbers

When numbers in exponential notation are added or subtracted, the exponents must be the same. If the exponents are the same, the coefficients are added and the exponent remains the same.

Consider the following example.

4.3 \times 10^4 + 1.5 \times 10^4  =  (4.3 + 1.5) \times 10^4 = 5.8 \times 10^4 \ (43,000 + 15,000 = 58,000)\\8.6 \times 10^7 - 5.3  10^7  = (8.6 - 5.3) \times  10^7 = 3.3 \times 10^7 \ (86,000,000 -  53,000,000 = 33,000,000)

If the exponents of the numbers to be added or subtracted are not the same, then one of the numbers must be changed so that the two numbers have the same exponent.

Examples

The two numbers given below, in their present form, cannot be added because they do not have the same exponent. We will change one of the numbers so that it has the same exponent as the other number. In this case, we choose to change 3.0 \times 10^4 to 0.30 \times 10^5. This change is made by moving the decimal one place to the left and increasing the exponent by 1. The two numbers can now be added.

8.6 \times 10^5 + 3.0 \times 10^4 = 8.6 \times 10^5 + 0.30 \times 10^5 = 8.9 \times 10^5

We also could have chosen to alter the other number. Instead of changing the second number to a higher exponent, we could have changed the first number to a lower exponent.

8.6 \times 10^5 \rightarrow 86 \times 10^4

Now, we can add the numbers, 86 \times 10^4 + 3.0 \times 10^4 = 89 \times 10^4

The answer, in this case, is not in proper exponential form because it has two non-zero digits to the left of the decimal. When we convert the answer to proper exponential form, it is exactly the same answer as before, 89 \times 10^4 \rightarrow 8.9 \times 10^5.

Exercises

Add or subtract the following exponential numbers as indicated.

  1. (8.34 \times 10^5) + (1.22 \times 10^5) \ =
  2. (4.88 \times 10^3) - (1.22 \times 10^3) =
  3. (5.6 \times 10^{-4}) + (1.2 \times 10^{-4}) =
  4. (6.38 \times 10^5) + (1.2 \times 10^4) =
  5. (8.34 \times 10^5) - (1.2 \times 10^4) =
  6. (8.34 \times 10^{-5}) + (1.2 \times 10^{-6}) =
  7. (4.93 \times 10^{-1}) - (1.2 \times 10^{-2}) =
  8. (1.66 \times 10^{-5}) + (6.4 \times 10^{-6}) =
  9. (6.34 \times 10^{15}) + (1.2 \times 10^{16}) =
  10. (6.34 \times 10^{15}) - (1.2 \times 10^1) =

Multiplying or Dividing with Numbers in Exponential Form

When multiplying or dividing numbers in scientific notation, the numbers do not have to have the same exponents. To multiply exponential numbers, multiply the coefficients and add the exponents. To divide exponential numbers, divide the coefficients and subtract the exponents.

Examples of Multiplying Exponential Numbers

Multiply: (4.2 \times 10^4)(2.2 \times 10^2) = (4.2 \times 2.2)(10^{4+2}) = 9.2 \times 10^6

The coefficient of the answer comes out to be 9.24 but since we can only carry two significant figures in the answer, it has been rounded to 9.2 .

Multiply: (2 \times 10^9)(4 \times 10^{14}) = (2 \times  4)(10^{9+14}) = 8 \times 10^{23}

Multiply: (2 \times 10^{-9})(4 \times 10^4) = (2 \times 4)(10^{-9+4}) = 8 \times 10^{-5}

Multiply: (2 \times 10^{-5})(4 \times 10^{-4}) = (2 \times 4)(10^{-5-4}) = 8 \times 10^{-9}

Multiply: (8.2 \times 10^{-9})(8.2 \times 10^{-4}) = (8.2 \times 8.2)\left (10^{(-9)+(-4)}\right ) = 32.8 \times 10^{-13}

The product in the last example has too many significant figures and is not in proper exponential form, so we must round to two significant figures, 33 \times 10^{-13}, and then move the decimal and correct the exponent, 3.3 \times 10^{-12}.

Examples of Dividing Exponential Numbers

Divide:  \frac {8 \times 10^7}{2 \times 10^4} = \left (\frac{8}{2}\right )(10^{7-4}) = 4 \times 10^3

Divide:  \frac {8 \times 10^{-7}}{2 \times 10^{-4}} = \left (\frac{8}{2}\right )\left (10^{(-7)-(-4)}\right ) = 4 \times 10^{-3}

Divide:  \frac {4.6 \times 10^3}{2.3 \times 10^{-4}} = \left (\frac{4.6}{2.3}\right )\left (10^{(3)-(-4)}\right ) = 2.0 \times 10^7

In the final example, since the original coefficients had two significant figures, the answer must have two significant figures and therefore, the zero in the tenths place is carried.

Exercises

  1. Multiply: (2.0 \times 10^7)(2.0 \times 10^7) =
  2. Multiply: (5.0 \times 10^7)(4.0 \times 10^7) =
  3. Multiply: (4.0 \times 10^{-3})(1.2 \times 10^{-2}) =
  4. Multiply: (4 \times 10^{-11})(5 \times 10^2) =
  5. Multiply: (1.53 \times 10^3)(4.200 \times 10^5) =
  6. Multiply: (2 \times 10^{-13})(3.00 \times 10^{-22}) =
  7. Divide:  \frac {4.0 \times 10^5}{2.0 \times 10^5} =
  8. Divide:  \frac {6.2 \times 10^{15}}{2.0 \times 10^5} =
  9. Divide:  \frac {8.6 \times 10^{-5}}{3.1 \times 10^3} =
  10. Divide: \frac {8.6 \times 10^{-5}}{3.1 \times 10^{-11}} =

Graphing Worksheet

You will need a piece of graph paper for this activity.

Experimental data consists of information about the variables in an experiment from specific measurements. Graphs can be prepared from the data. A straight line or curve is drawn using the data points as a guide. The data points are not connected in a “dot-to-dot” manner. Rather, the line is drawn that “best fits” the data.

Readers of the graph may need to know the value of a variable at a point that was not measured. Interpolation is a method used to approximate values that are between data points on a graph. Extrapolation is a method for approximating values that are beyond the range of the data. Data must be extrapolated when needed values are not in the range of the measurements obtained. Unless you have a reason to believe that the graph line continues smoothly beyond the ends of the data points, extrapolation is risky . . . that is, it may produce wildly incorrect data.

The data in the following table were obtained from an experiment conducted to find out how the volume of a gas changes when its temperature is changed. Use this data to construct a graph.

Procedure

1. Put a title on the graph paper.

2. Mark the x-axis and y-axis lines on the graph paper. Use the x-axis for the independent variable (temperature) and use the y-axis for the dependent variable (volume). Write the names of the variables along the axis including the units of measure for each variable.

3. Write in the temperature measures along the temperature axis. The temperature axis should include all temperatures from 0 K to 600 K.

4. Write in the volume measures along the volume axis. The volume axis should include all volumes from 0 mL to 500 mL.

5. Plot a point for set of data where you have a measurement for both temperature and pressure.

6. Draw a line that best fits the data points.

Questions

1. Use your graph to predict values for the volume of the gas at 0 K, 140 K, 273 K, 400 K, and 600 K. Place the values of these volumes in the data table.

2. What technique did you use to estimate the volume measurements at 140 K and 273 K?

3. What technique did you use to estimate the volume measurements at 0 K and 600 K?

4. Write a sentence that describes the relationship between the temperature and the volume of a gas.

Answers to Worksheets

  • The worksheet answer keys are available upon request. Please send an email to teachers-requests@ck12.org to request the worksheet answer keys.

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Aug 18, 2012

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Jul 21, 2014
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