1. Metric System

2. Scientific Notation  Scientific notation is a way of writing very large and very small numbers more conveniently.  A number written in scientific notation has two distinct parts: 1. A number with a decimal point that falls between 1 & 10 2. The power of ten (either positive or negative) that shows which way and how many places to move the decimal point to take the number out of scientific notation.

3. Scientific Notation  The speed of light is 300,000,000 m/s. Write this in scientific notation:  3.0 x 10 8 m/s  A snail has a speed of 0.00086 m/s. Write this in scientific notation:  8.6 x 10 -4

4. Scientific Notation  Multiplying – multiply the numbers that appear before the multiplication signs and add the exponents  (3.0 x 10 8 )(5.0 x 10 2 ) = 15 x 10 10 = 1.5 x 10 11  Division – divide the numbers that appear before the exponential terms and subtract the exponents  (1.5 x 10 11 )/(3.0 x 10 8 ) =.50 x 10 3 = 5.0 x 10 2

5. Standards of Measurement A standard is an exact quantity that people agree to use for comparison or measurement. A standard is an exact quantity that people agree to use for comparison or measurement. The first such system of measurement called the Metric System was devised by a group of scientists in the late 1700’s. The first such system of measurement called the Metric System was devised by a group of scientists in the late 1700’s. In 1960 an improved version of the Metric System was devised and is now called the International System of Units. (SI) In 1960 an improved version of the Metric System was devised and is now called the International System of Units. (SI)

6. The Seven Fundamental Units of Measurement MeasurementSI Unit Lengthmeter (m) Masskilogram (kg) Volumeliter (L) Volumeliter (L) Timesecond (s) TemperatureKelvin (K) Amount of Substancemole (mol) Electric CurrentAmpere (A)

7. Commonly Used Prefixes PrefixSymbolMeaning Numeric Form Fraction Kilo - kThousand1,0001,000 Hecto - hHundred100100 Deca - daTen1010 (base unit) m, L, g One11 Deci - dTenth0.11/10 Centi - cHundredth0.011/100 Milli - mThousandth0.0011/1,000

8. Measurement Precision – A gauge of how EXACT a measurement is Ex: a digital clock is more precise than a regular clock

9. Measurement Accuracy – the closeness of a measurement to the accepted value for a quantity. Ex: an atomic clock is more accurate than our school clocks

10. Measurement Measurements can be accurate but not precise. Measurements can be accurate but not precise. They can be precise but not accurate. They can be precise but not accurate. They can be both accurate and precise. They can be both accurate and precise. They can be neither accurate nor precise. They can be neither accurate nor precise.

11. Measuring Length  When measuring length, we will be using a metric ruler or meterstick.  The numbered divisions are 1 cm divisions.  The smallest divisions marked are 1 mm divisions.

12. Measuring Mass  When using an electronic balance, write down all numbers printed on the screen.  When using a triple beam balance, the mass can be measured accurately to 0.01 grams.

13. Measuring Volume  The amount of space occupied by an object is called its volume.  There is no specific way to measure the object’s volume.

14. Measuring the Volume of a Solid  When measuring the volume of a solid object, multiply its length x width x height.  Typically the volume of a solid is measured in either cubic centimeters (cm 3 ) or cubic meters (m 3 ).

15. Measuring the Volume of a Liquid  When measuring a liquid volume, one must choose the appropriate device based upon the amount of liquid to be measured.  For smaller amounts of liquid, a graduated cylinder is used.  For larger amounts of liquids, a beaker would be used.  The most common units used for these types of volumes are liters (L) and milliliters (mL).

16. Density  Density is an important characteristic property of matter.  When one speaks of lead as being “heavy” or aluminum as “light,” one is actually referring to the density of these metals.  Density is defined as mass per unit volume.

17. Calculating Density An object with a mass of 10 grams and a volume of 5 cm 3 has a density of 2 g/cm 3. 10 g = 2g/cm 3 5 cm 3

18. Comparing Densities Where is the most dense object?Where is the most dense object? Where is the least dense object?Where is the least dense object?

19. Factor Label Method  Not all objects that are measured are in the units that are needed.  The factor label method is a mathematical way to convert from the units you have to the units you need.  In order to eliminate the unwanted units, you design a ladder-type set up of equalities that cancel out the units you no longer want.

20. Steps of Factor Label Example: How many liters are there in 3650 mL? 1. Find an equality relating to the original units and write it down in the ladder set up. Make sure to put the units that you DO NOT want in the denominator. Cross out the units that match. 3650 mLx 1 L____= _______ L 1000 mL 1000 mL

21. Steps of Factor Label 2. Ask yourself if you want the units in the numerator. If you don’t, repeat steps 1 and 2 until you get the correct units in the numerator. 3. Solve the problem by multiplying the numbers in the numerator, then dividing by the numbers in the denominator. 3650 mL x1 L_____= 3.65 L 1000 mL