1. General Chemistry the Central Science
Brown & LeMay
Chapter One: Introduction, Matter & Measurement

2. Molecular Perspective
Classifications of Matter States, Pure Substances, Mixtures, Elements, Compounds
Properties of Matter
Units of Measurement SI Units, Derived Units, Uncertainty, Dimensional Analysis

3. Atoms & Molecules -- basic nature of chemistry
Atoms & Molecules -- basic nature of chemistry -necessary to understand the nature of matter art, medicine, agriculture, environment, home
Classifications of Matter -states gas, liquid, solid (H) -pure substance fixed composition/distinct properties (elements or compounds) -elements cannot be decomposed to simpler substances -compounds combination of two or more elements -mixture combination of two or more pure substances (heterogeneous & homogeneous/solutions)

4. Gas Liquid Solid
no shape, no volume
volume no shape
volume & shape

5. Elements. -112 elements known
Elements elements known -listed on periodic table with symbols (H) -arranged in a particular order such that closely related elements are grouped
Compounds -two or more elements chemically combined -law of constant composition or definite proportions eg. water is always 11% H and 89% O
while peroxide is 6% H and 94% O

7. Mixture. Physical combination of two or more pure substances
Mixture Physical combination of two or more pure substances which can be physically separated into the components
Heterogeneous -composition, properties, appearance vary -non-uniform in appearance
Homogeneous -uniform appearance/properties but may vary between different samples -a “solution”

8. no
yes
yes no no
yes

9. Properties of Matter. -Physical Properties -- color, odor, density, b
Properties of Matter -Physical Properties -- color, odor, density, b.pt. -Chemical Properties -- chemical changes occur -Intensive Properties -- do not depend upon quantity of material present temp, m.pt., density -Extensive Properties -- dependent upon the quantity of material present mass, volume
Changes of Matter -Physical -- appearance changes but not composition -Chemical -- transformation into chemically different substance

10. Find Patterns, Trends, Laws
Scientific Method
Find Patterns, Trends, Laws
Observations & Experiments
Formulate & Test Hypothesis
Theory

11. Units of Measurement SI Units Quantity Name Abbrev.
Mass* Kilogram kg Length Meter m Time Second s Electric Curr. Ampere A Temperature Kelvin K Lum. Intensity Candela cd Amount Mole mol
*quantity of matter

12. Selected Prefixes Prefix Abbrev. Meaning
Mega- M Kilo- k Deci- d Centi- c Milli- m Micro- m Nano- n Pico- p Femto- f

13. Temperature Kelvin Celsius Fahrenheit 373K 100° C 212° F 273K 0° C

14. Derived Units -- combinations of other units
Volume -SI unit for volume is m L = 1 dm mL = 1cm3
Density -amount of mass in a unit volume -combination of mass and volume units -typically g/mL for solids and liquids & g/L for gases

15. Practice Exercise 1.3 (pg. 18) g of ethanol needed, density = g/mL, how many mL of ethanol needed?
need a volume unit, mL, we have a mass unit, g, and a combination unit, g/mL
15.0 g x mL = g
19.0 mL ( )

16. Uncertainty in Measurement
Precision vs Accuracy -Precision -- agreement of measurements -Accuracy -- proximity to true value
good precision poor precision good precision good accuracy poor accuracy poor accuracy

17. 1 2 3
2.55
2.5 3 1 2

18. Significant Figures 1. all non-zero digits are significant 1.2357
2. zeros between non-zero digits are significant
3. zeros to the left of the first non-zero digit in a number are not significant
4. when a number ends in zeros to the right of decimal point, the zeros are significant
5. when a number ends in zeros which are to the left of the decimal those zeros may or may not be significant or or or 2000

19. Use in Calculations
multiplication & division -result reported to no more total sig. digits than the piece of data with the least number of digits
addition & subtraction -result reported to same number of significant decimal places as the piece of data with the least number of significant decimal places

20. Use in Calculations
multiplication & division -result reported to no more total sig. digits than the piece of data with the least number of digits (1.27)(2.3) =
addition & subtraction -result reported to same number of significant decimal places as the piece of data with the least number of significant decimal places =

21. Dimensional Analysis 1 ft = 12 in 1 ft = 12 in 1 ft 1 ft
1 = 12 in or = ft ft in
conversion factors

22. conversion factors convert between two different units
Convert 56 inches to feet.
56 in x ft = in
4.7 ft

23. Practice Excersize 1.8 pg 26 Convert 500.0 mi to km 1 mi = 1.6093 km
1. need a conversion factor
1 mi = km
500.0 mi x km 1 mi
2. set up to cancel mi
3. do the math, cancel the appropriate units
500.0 mi x km = km 1 mi

24. Convert the volume of a 10 m x 10 m x 10 m room to liters.
1 dm3 = 1 L
1 dm = m
1000 m3 x 1 dm x 1 dm x 1 dm = 1.0 x 106 dm m m m
1 dm m3
1.0 x 106 dm3 x 1 L = 1.0 x 106 L dm3

25. Problems If I weigh 52.3 kg, how many grams do I weigh?
If a tennis ball is served at 140 mph, what is its speed in m/s?
You have a 40 lb baggage limit, the scale reads kg. Are you over or under?
Convert 2.5 L to cm3

26. Problems
Glycerol is a viscous, sweet-tasting liquid. In an experiment, a 25.0 mL sample was found to weigh 31.6 g. What is the density of glycerol?(2.60)
Diethyl ether has a density of g/mL. What volume of diethyl ether is needed to equal 28.0 g?(2.64)

27. Problems
The density of the sulfuric acid solution of a fully charged lead storage battery is about 1.28 g/mL. What is the mass of the solution whose volume is 1.50 L? (2.89)
The density of red blood cells is about g/cm3, somewhat higher than that of blood plasma. What is the mass of cells whose volume is 5.67 cm3?(2.88)

28. Problems
To identify a metal, an experimenter placed a 32.6 g sample in a grad. cylinder. He then poured in 25.0 mL of water, covering the metal and bringing the liquid level in the cyliner to 28.7 mL. What is the density of the metal? (2.62)
You are buying $15.00/sq. yd for a 1500 sq. ft house. How much will it cost?

29. Problems
If liquid nitrogen has a boiling point of 77K, and the temperature is -300°F, will it be a solid, liquid or gas?
A 175 lb patient is to undergo surgery and will be given an anesthetic intravenously. The safe dosage of anesthetic is 12 mg/kg of body weight. Determine the maximum dose of anesthetic that should be used.