Preview
Buy lesson
Buy lesson
(only $1.98) 
You Might Also Like

Chemistry: Dimensional Analysis 
Chemistry: The Nature of Energy 
Chemistry: Significant Figures 
Chemistry: Precipitation Reactions 
Chemistry: Standard Reduction Potentials 
Chemistry: Find Atomic Mass, Radius from Unit Cell 
Chemistry: Rates of Disintegration Reactions 
Chemistry: Using Standard Reduction Potentials 
Chemistry: Standard Free Energy Formation Changes 
Chemistry: Elimination Reactions 
College Algebra: Solving for x in Log Equations 
College Algebra: Finding Log Function Values 
College Algebra: Exponential to Log Functions 
College Algebra: Using Exponent Properties 
College Algebra: Finding the Inverse of a Function 
College Algebra: Graphing Polynomial Functions 
College Algebra: Polynomial Zeros & Multiplicities 
College Algebra: PiecewiseDefined Functions 
College Algebra: Decoding the Circle Formula 
College Algebra: Rationalizing Denominators

Chemistry: Elimination Reactions 
Chemistry: Standard Free Energy Formation Changes 
Chemistry: Using Standard Reduction Potentials 
Chemistry: Rates of Disintegration Reactions 
Chemistry: Find Atomic Mass, Radius from Unit Cell 
Chemistry: Standard Reduction Potentials 
Chemistry: Precipitation Reactions 
Chemistry: Significant Figures 
Chemistry: The Nature of Energy 
Chemistry: Dimensional Analysis
About this Lesson
 Type: Video Tutorial
 Length: 9:31
 Media: Video/mp4
 Use: Watch Online & Download
 Access Period: Unrestricted
 Download: MP4 (iPod compatible)
 Size: 101 MB
 Posted: 01/28/2009
This lesson is part of the following series:
Chemistry: Full Course (303 lessons, $198.00)
Chemistry Review (25 lessons, $49.50)
Chemistry: Introduction to Matter and Measurement (13 lessons, $14.85)
Chemistry: Scientific Measurement (5 lessons, $7.92)
Science involves a lot of measuring, but measurements are meaningless without units. Units, however, developed differently all over the world, and many are derived from parts of the body, such as the foot, the hand, and the cubit. Scientists developed a method of measurement for science that is more uniform, called the Systeme Internationale d'Unites (French for ""The International System of Units""), or the SI system. Professor Yee discusses the common measurements (such as length, mass, time, temperature) and their units (meter, kilogram, seconds, kelvins). In addition to the standard measurements, there are additional measurements that are derived from calculations using the standard measurements (energy, force, power). Many of these standard units are larger than most chemists will use, so Prof. Yee also gives us prefixes and some more derived units that are more commonly used for chemistry.
Taught by Professor Yee, this lesson was selected from a broader, comprehensive course, Chemistry. This course and others are available from Thinkwell, Inc. The full course can be found at http://www.thinkwell.com/student/product/chemistry. The full course covers atoms, molecules and ions, stoichiometry, reactions in aqueous solutions, gases, thermochemistry, Modern Atomic Theory, electron configurations, periodicity, chemical bonding, molecular geometry, bonding theory, oxidationreduction reactions, condensed phases, solution properties, kinetics, acids and bases, organic reactions, thermodynamics, nuclear chemistry, metals, nonmetals, biochemistry, organic chemistry, and more."
Gordon Yee is an associate professor of chemistry at Virginia Tech in Blacksburg, VA. He received his Ph.D. from Stanford University and completed postdoctoral work at DuPont. A widely published author, Professor Yee studies moleculebased magnetism.
About this Author
 Thinkwell
 2174 lessons
 Joined:
11/13/2008
Founded in 1997, Thinkwell has succeeded in creating "nextgeneration" textbooks that help students learn and teachers teach. Capitalizing on the power of new technology, Thinkwell products prepare students more effectively for their coursework than any printed textbook can. Thinkwell has assembled a group of talented industry professionals who have shaped the company into the leading provider of technologybased textbooks. For more information about Thinkwell, please visit www.thinkwell.com or visit Thinkwell's Video Lesson Store at http://thinkwell.mindbites.com/.
Thinkwell lessons feature a starstudded cast of outstanding university professors: Edward Burger (PreAlgebra through...
More..Recent Reviews
This lesson has not been reviewed.
Please purchase the lesson to review.
This lesson has not been reviewed.
Please purchase the lesson to review.
An Introduction to Matter and Measurement
Scientific Measurement
The Measurement of Matter Page [1 of 2]
If I were going to explain American football to my friend from someplace who doesn’t understand American football,
and I said that the distance from end zone to end zone was 100, what would be the problem with that? Well, the
answer is I haven’t associated any units with the 100. Is it 100 inches? Is it 100 miles? Is it 100 feet? So the
problem is that whenever you describe any sort of measurement in science, or in real life for that matter, what you
have to do is you always have to associate units with the measurement. Units have to go with the measurement. So
let’s explore some units of length, just for grins, and then we’ll see why it might be necessary to settle on one unit
when we’re doing scientific stuff.
Feet, for instance, is a very old unit of length and it probably started out as the length of somebody’s foot. Inches is
onetwelfth of a foot. Meters is what we’re going to come back to. Miles, you know, is 5,280 feet. Cubits, maybe
you’ve never heard of a cubit. Believe it or not, a cubit is the distance from your elbow to the tip of your finger. It’s
about 18 inches. And, obviously, it’s going to depend on whose hand, whose arm. Don’t know whose it was, but the
point is that a cubit is a fairly convenient unit in the sense that everybody’s got one. And so roughly speaking, it’s
going to be the same. As far as I know, nobody still uses cubits. On the other hand, the next unit, hands, believe it or
not, someone actually still uses a hand. What is hand? A hand is the width of Henry VIII’s hand. And it’s about 4
inches. Well, people who raise racehorses still use the term hands when describing how tall the horse is. It’s from the
ground up to its withers, which is about its shoulder, and a typical horse is about 15 hands. People whose race
horses also use furlongs. A furlong is 220 yards. Light year is something that astronomers use. It’s how far light
travels in one year. And a parse is 3.26 light years, but I don’t know why we need two lengths that are both quite
large. People who do deep sea diving or who go down in submarines use things like fathoms and leagues.
So there are just a plethora of lengths, or units of length that all these different civilizations have come up with. And
the problem with having all these different units is science is a very international effort. People in all these different
countries are doing science, and if they just reported all their numbers in the unit that they happen to use in their
country, then people would constantly be having to convert from inches to meters, and furlongs to parsecs, and blah,
blah, blah, and it would just be too much trouble. And so what scientists decided to do was to settle on a set of units
that everybody could agree on and everybody would report their data, all their measurements, with a set of units. And
that set of units goes by the name SI, and SI stands for Système International d’Unités, which is French, and pardon
my French, but basically the international system of units. And there are actually only seven base units in the SI
system, length, and the unit of length is the meter. And for those of you who might not know, a meter is about 39
inches. Mass is the kilogram, which is about 2.2 pounds. Time is the second, you know that. Temperature is the
Kelvin, and you’re unfamiliar with the Kelvin at this point. Chemical amount is the mole, and you’re unfamiliar with the
mole. Electric current is the ampere, something you’ve probably heard before. And luminous intensity is the candela,
and these quantities have these abbreviations here.
Right now, you’re probably only familiar with length, mass and time. And that’s fine. We’ll clarify all these other things
for you later on.
Now, there are some derived SI units, units that are just combinations of the original seven, but that have special
names as well. For instance, the unit of energy, which we’ll come to when we do thermochemistry, is the joule, has
the abbreviation J, and it’s a kilogram meter squared per second squared. And notice that the exponent has a minus
2. That means it’s in the denominator of this expression. A force not so important for chemists is the Newton. Power
is the watt. Light bulbs, how much power they consume is measured in watts. Pressure is the Pascal, something
you’ve probably never heard of before, and electric charge and electric potential difference, things that aren’t going to
be really very important for chemists, but here they are. When you take physics, these are the kinds of things you’re
going to need to know.
Now, since it isn’t necessarily convenient to always express things in the SI units, because they are, for instance, very
large, the unit of length is a meter, but not a lot of things in the chemistry lab are this long, we need to have prefixes
that allow us to make units that are smaller for convenience. So on top of the SI units, we have the fractions, and
these are the ones that you should probably commit to memory. 102 goes by the prefix centi. The symbol is
lowercase “c”. For example, c, lowercase c, lowercase m is a centimeter. I’m sure you already know what a
centimeter is, but it’s oneone hundredth of a meter. 103 is milli, lower case “m”, milliliter. I haven’t told you what a
liter is, but a milliliter is oneone thousandth of a liter. 1012 is pico, relatively less important, but it turns out that when
we’re talking about the size of an atom, a picometer is a useful size. It’s 1012 meters. And then, going the other
way, larger, kilo, 103 is a kilo, lowercase “k” is the symbol. Kilogram again is the SI unit of mass, but a kilometer, so
An Introduction to Matter and Measurement
Scientific Measurement
The Measurement of Matter Page [2 of 2]
we change the emphasis on how we pronounce it. Some people say kilometer, but the point is that’s one thousand
meters.
Now, there are some derived units from the SI system that don’t involve special names, like velocity is in meters per
second, and so “m” is the unit of length. That’s the meter, and the unit of time is a second. Volume, the unit of
volume is a cubic meter, and that’s a really big thing. It’s something that’s about a yard on a side, so it’s going to be
this gigantic thing. And we’re going to see that chemists have another unit that’s a little more convenient. Density is
the mass of an object divided by the volume that it occupies, so the SI unit is kilogram per cubic meter. The rate of
reaction, we’re going to see much later on, is, in SI units, the mole per cubic meter per second. And again, chemists
choose some more convenient units. Again, a cubic meter is not really convenient, because it’s big, so chemists talk
about things in terms of liters, where a liter is oneone thousandth of a cubic meter. And for those of you who might
not know, a liter is about the size of a quart. So a milk carton is about a liter, a unit of mass that, for chemists, is a
little more convenient. Chemists don’t measure typically things around the neighborhood of 2.2 pounds, which is what
a kilogram is, so we use oneone thousandth of a kilogram, which is just the gram. Thermometers are not typically
calibrated in Kelvins, they’re calibrated in degrees Celsius, and degrees Celsius is the scale that we’ll use most often,
and I’ll explain how you get from degrees Celsius to Kelvins later on. And finally, pressure, the unit that chemists
often use is the atmosphere for largely historical reasons, and its related to the SI unit by 101,325 Pascals, which is
the SI unit, is equal to 1 atmosphere.
Okay, so given that we sort of tweak the system a little bit as chemists to come up with units that are a little more
convenient, what you’re going to see is that when we’re talking about volume, very often, instead of cubic meters,
we’re going to be in cubic centimeters. A cubic centimeter is about the volume of the end of your thumb. For density,
instead of kilograms per cubic meter, grams per cubic centimeter is going to be much more likely. And similarly, for
rates of reaction, since the cubic meter is so large, most often this will be expressed as moles per liter, per second.
What’s the bottom line? The bottom line is if you’re going to make a measurement, you have to associate units with it.
If you’re going to report a measurement, you have to associate units with it. And here’s something to think about. If
your friend from Europe came over to the United States and went to get a haircut and asked the stylist or the barber to
cut three off, meaning three centimeters, that would be about an inch. But, in the United States, if you say, “three, cut
three off”, the barber or stylist is most likely to think three inches. And so the person from Europe is going to lose
about three times as much hair as he or she intended to lose. So again, it’s really important to associate units with
your measurements.
Get it Now and Start Learning
Embed this video on your site
Copy and paste the following snippet:
Link to this page
Copy and paste the following snippet: