1. Measurement and the Metric System
Quantitative observations

2. Fundamental quantities
Measurement
Fundamental quantities
Direct measurement
Indirect measurement
Derived quantities
Calculations
Density
Heat energy

3. Rules for Significant Measurements
One place past the smallest calibration
Indicates where uncertainty is
Communicate precision of the instrument

4. Protocols for deriving quantities
Multiplication and division
Addition and subtraction
Rounding values

5. Metric System Developed in France in 1795
Revised and called International System of Measurements (SI) in 1960
Based on units of 10

6. SI Base Units Quantity SI base unit symbol Length Meter m Mass gram g
Temperature
Kelvin
Celsius K oC
Time
Second s
Liquid volume
Liter L
Amount of substance
Mole
mol

7. Memorize these !!!!! * “unit” refers to “base unit”
1 Kilo = 1 x 103 units
1 Hecto = 1 x 102 units
1 Deka = 1 x 101 units
Basic unit = 1
1 x 101 deci (d) = 1 unit
1 x 102 centi (c)= 1 unit
1 x 103 milli(m) = 1 unit
1Giga(G) = 1 x 109 units
1Mega(M) = 1 x 106units
1 x 106 Micro(µ) = 1 unit
1 x 109 Nano(n) = 1 unit
1 x 1012 Pico(p) = 1 unit

8. Conversions Practice

9. Density Density is calculated by: D = mass volume
Amount of matter per unit volume
Water: g/ ml at 25C
Iron: g/cm3
Lead g/cm3
Density is calculated by:
D = mass
volume

10. Density Density is the amount of matter in a given space (volume)
D = mass
volume

11. Density
Measuring liquid volume
Volume displacement

12. Density Measuring solid volume Cylinder = V =πr2h
Cube = length x width x height
Cylinder = V =πr2h

13. Density
Ex: A solid displaces ml of water and has a mass of 98.5 grams. Calculate its density. Is it a block of lead?

14. Density practice

15. Specific gravity
Comparison of the ratio of the density of a substance to the density of liquid water at 4C
(1.00g/ml)

16. Temperature Scales
Temperature is the measure of the average kinetic energy of a system.
Implies molecular motion
Celsius temperature
Kelvin temperature

17. Temperature Scales Fahrenheit Celsius Kelvin Water Boils 373 K 212oF
100oC
Water Freezes
32oF
0oC
273 K
Molecular Motion Stops
-460oF
-273oC
0 K (absolute zero)

18. Converting between Temperature Scales
Fahrenheit and Celsius:
oC = 5/9 (oF-32)
oF = (9/5 x oC)+32
Ex.What is the Celsius value for 60.0oF?
oC = 5/9(60-32)
oC = 5/9(28)
oC =
oC =15.6

19. K = oC + 273 From Celsius to Kelvin: K = 80 + 273 K = 353
Ex.80.0oC would be what value on the Kelvin scale?
K =
K = 353

20. Heat and Specific Heat Heat is the flow of thermal energy in a system
Heat flows from hotter to cooler
Ice cubes!
Heat can flow into or out of a system

21. Heat and Specific Heat
Heat transfer that causes temperature changes simply change in KINETIC ENERGY
Heat transfer that causes phase changes imply change in POTENTIAL ENERGY

22. The Joule Metric unit of energy 4.18 joules raises 1.00g of water 1C.
This is the SPECIFIC HEAT OF WATER!

23. Percent Composition

24. When you see %, think……
Part
X 100 = %
Whole

25. Percent Composition percent by mass
% composition = Mass of element x 100%
mass of compound

27. Terms to review Fundamental and derived quantities
Precision and accuracy
Matter
Mass
Volume
Density
Significant Figures
% composition
Scientific notation
Metric system
Dimensional analysis