1 / 33

Measurement

Learn the basics of the International System of Units (SI) used in chemistry: measurement, mass, volume, temperature scales, SI prefixes, conversions, and dimensional analysis. Master the fundamental units and their applications to excel in scientific studies.

bqueen
Download Presentation

Measurement

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. There are many ways to measure things and not everyone uses the same units of measure. That’s one reason why scientists developed an International System (SI) for standardizing units of measure. While this system has helped scientists, many people are still unfamiliar with the S.I. system, since the U.S. refuses to go along with the rest of the world. Our goal here is to become familiar with the S.I. system as it is used in the study of chemistry. Measurement

  2. Base Units of the S.I. System • The following units are the most basic units of the S.I. system. All other units are derived from these basic units. • Notice that the base unit of mass is the kilogram, not the gram!

  3. Length • To measure length, we use the meter • A meter is equal to 3.28 ft. • Scientists often need to accurately measure things that are either very small or very big • The micrometer at right can measure with an accuracy to 0.001 mm The “cubit” was not a very precise unit, since it was based on forearm length.

  4. Mass • Mass is defined as the amount of matter. Although the kilogram is the base unit, we normally use grams in lab. • Mass in our class will be measured using a digital balances. They measure to the nearest centigram, or 0.01 g. • We also have an analytical balance, which measures to 0.001 g. It is really precise!

  5. Volume Measurements • The units of volume we will use are mL and L because that is what we measure in the lab. These are a type of “derived” unit, since they are made up of base units. • V = l x w x h or (cm x cm x cm) = cm3 • 1.0 cm3 = 1.0 mL Yeah, this is important! • Example: Convert 749 mL to liters • 749 mL x 1 L = 0.749 L 1000 mL

  6. Can You Read the Volume Correctly? • What is the volume of water in this cylinder? • Read the bottom of the meniscus, estimate to the nearest 0.1 mL • 52.8 mL (+/- 0.1 mL)

  7. Temperature Scales William Thompson, Lord Kelvin • Most people think that the base temperature units of the S.I. system are degrees Celsius. • While it is true that Celsius is the most commonly used unit, the Celsius scale is actually based on the Kelvin scale. Kelvin is the base unit for temperature. • Degrees Kelvin are called Kelvins, K • No degree symbol is used for K • K is also called the “absolute temperature scale” • K = °C + 273

  8. S.I. Prefixes • The best thing about the S.I. system is that it is based on multiples of 10. The English system is based on weird numbers like 16. (Like there are 16 16ths in an inch…why?!) There are many prefixes used to indicate the size of S.I. units relative to each other. We don’t need to learn them all, but several of them are very common, and must be learned.

  9. S.I. Prefixes To Know

  10. S.I. Conversions • How do we use these prefixes? Why do we need to know this? • Example: Two students were given identical rulers and asked to calculate the area of a piece of notebook paper. One student measured the length of the paper as 28.0 cm. The other student reported that the width of the paper was 216 mm. Before multiplying these values to find the area, the units of each measurement must be the same. • 216 mm x 1 cm = 21.6 cm Because a mm is 10 times smaller • 10 mm than a centimeter. • A = l x w = 28.0 x 21.6 = 605 cm2 Notice the conversion factor that was used.

  11. B. S. Rule (This stands for “brilliantly simple”, by the way) • There are many ways to remember how to convert from one unit to another. Many students draw stair steps and know sayings about King Henry. • Try learning the prefixes and using the B. S. Rule. Just draw an arrow between B and S! • B  S When going from a big unit to a small unit, move the decimal to the right. • B  S When going from small to big units, move the decimal to the left. • Yeah, but how many places do I move it??

  12. Number Line If you think of the SI units as being on a number line, you can just hop around. |10-9 |10-6 |10-3 |10-2 |10-1 |100 |101 |102 |103 |106 |109 n µ m c d ↑ da h k M G base unit  Smaller Bigger 

  13. Using the Prefixes • It’s easy to do conversions if you think of the prefixes as being on a number line. • Example: Convert 458 nm to m • Find nm on the number line. Since it is way smaller than the m, the decimal moves to the left nine places. B  S 0.000000458 m or in scientific notation 4.58 x 10-7

  14. Dimensional Analysis • Dimensional analysis is a method of problem solving that uses conversion factors, which are written a fractions. • The fractions have numbers as well as units • The quantity in the numerator is equivalent to the quantity in the denominator • Examples: 10 mm60 s1 min • 1 cm 1 min 60 s

  15. How do we do the math? • Most people are pretty comfortable multiplying fractions. • 1 x 5 x 3 = 15 we just multiply the numerators together, and then the 2 3 4 24 the denominators. Then divide 15 by 24, which is 0.625 We can also use “Railroad Tracks” to make the calculation look neater: 1 | 5 | 3 = 15 = 0.625 2 | 3 | 4 24 Treat units the same way you treat numbers. They get multiplied and divided, too! Example: cm x cm x cm = cm3 Example: m3 = m m2

  16. Dimensional Analysis Example: How many mm are in 147 km? 147 km x 1000 m x 1000 mm = 147,000,000 mm 1 1 km 1 m = 1.47 x 108 mm Step 1: Start with what you are given. Step 2: Multiply by a conversion factor that has the starting units in the denominator, and the unit you want to find in the numerator. (It may take more than one conversion factor to get to where you want to go.) Step 3: Multiply it out and then write in scientific notation

  17. What about Scientific Notation Math? • When multiplying, add the exponents: 103 m x 104 m = 107 m2 • When dividing, subtract the exponents 103 m = 10-1 104 m • OMG what if one of them is like, a negative? 103 m = 107 3-(-4) = 7 10-4 m

  18. Using Dimensional Analysis to Solve Problems • If you watched any of the Olympics, you know some amazing athletes competed. Let’s look at some of the new World Records and see if we can convert them to everyday units, using dimensional analysis

  19. Swimming Michael Phelps broke a World Record and won a Gold Medal by swimming the 100 m Butterfly in 50.58 seconds. • What is this speed in feet per second? How ‘bout in miles per hour? • 100 m x 3.28 ft = 6.48 ft 50.58 s 1 m s 6.48 ft x 1 mile x 3600 s = 4.42 mi 1 s 5280 ft1 hr hr Metric to English conversion factors will be provided if you need them.

  20. Swimming • How does Michael’s phenomenal speed compare to another Gold Medalist, Cesar Cielo of Brazil? Cesar swam the 50 m Freestyle in 21.30 seconds. • 50 m x 3.28 ft x 1 mi x 3600 s = 5.25 miWow, phaster than Phelps? 21.30 s 1 m 5280 ft 1 hr hr Cesar studies at Auburn University. (Great school.)

  21. Track and Field • Speaking of fast, have you seen this guy run? • Usain Bolt of Jamaica, won a Gold Medal and broke Olympic and World Records with his time on the Men’s 200 meter. • Usain made it look easy as he ran it in19.30 s.

  22. Track and Field • Use dimensional analysis to find out Usain’s speed in feet per second, and also in miles per hour. 200 m x 3.28 ft = 40.0 ft 19.30 s 1 m s 40.0 ft x 3600 s x 1 mi = 27.3 mi s 1 hr 5280 ft hr

  23. Accuracy vs. Precision • Accuracy refers to how close a measured value is to an accepted value. In other words, “is it correct?” • The person practicing archery in this photo was not very accurate, only a few of the arrows hit the bull’s eye. They are not very precise either, since the arrows are all over the place. (Random errors.) This person needs glasses!

  24. Precision • Precision has two general meanings: • Precision refers to how close a series of measurements are to one another. In other words, “is it repeatable?” • The word precision is also used to indicate how exact a measurement is. For example, 2.54 cm is more precise than 2.5 cm. • The target at right shows both accuracy and precision. This archer is accurate and precise!

  25. We need accuracy and precision… World Champion Archer Joo Hyun Jung from Korea says, “You need both precision and accuracy to win the GOLD!”

  26. Significant Figures “Sig Figs” • If we want to measure things with accuracy and precision, we must consider a topic known as significant figures, a.k.a. significant digits. • Significant digits include all known digits plus one estimated digit, for most measuring instruments. Examples: • A large graduated cylinder can be read to the 0.1 mL • A buret can be read to the .01 mL • A digital balance does not have any estimated digits, you just copy all the digits down. • Don’t drop final zeroes if they are to the right of the decimal point!

  27. Rules for Sig Figs- gotta know these 5 rules! • Rule Number One: Non-zero numbers are always significant. • Look at these examples: • You can see that we are simply counting the number of digits in these measurements.

  28. Sig Fig Rules • Rule Number Two: • Zeros between non-zero numbers are always significant. • Look at these examples: • Again, you can see that we are simply counting all of the digits

  29. Sig Fig Rules • Rule Number Three:All final zeros to the right of the decimal point are significant. • We are used to the idea that 2.0 is the same thing as 2. With measurements, this is not true! The 2.0 is a more accurate measurement.

  30. Sig Figs • Rule Number Four: Zeros that act as placeholders are not significant. Convert numbers to scientific notation to remove the placeholder zeros. • See how converting to scientific notation lets you see how many digits to count?

  31. Significant Figures • Rule Number Five: Counting numbers and defined constants have an infinite number of significant figures. • This just means that these numbers do not limit the precision of your calculations.

  32. Calculations Involving Sig. Figs • There are two rules to keep in mind when doing calculations involving significant figures. • When adding or subtracting measurements, your answer must have the same number of digits to the right of the decimal point as the value with the fewest digits to the right of the decimal point. • Example: 28.0 cm Line up the decimals! 23.538 cm 25.68 cm + 77.218 cm The answer can only go to the tenths place. The answer is 77.2 cm. (If the sum had been 77.278 cm, the answer would have rounded up to 77.3 cm.)

  33. Calculations Involving Sig. Figs. • The second rule is that when multiplying or dividing measurements, your answer must have the same number of significant figures as the measurement with the fewest significant figures. • Example: 3.20 cm x 3.65 cm x 2.05 cm = 23.944 cm3 = 23.9 cm3 (since you can only have three sig figs, you must round off to the tenth’s place.)

More Related