1.1 – The Scientific Method (SM) ▪ Understand the process ▪ Define the four components ▪ Understand the meaning of the word theory

as it applies to the SM

Define the Question/Problem

Propose Hypothesis: educated guess

Carry out experiments & collect data

Develop Theory: conclusion(s) based on factual data

Increase the rate of a particular reaction

Utilize a catalyst

Experiment with various catalysts

and conditions (i.e., temp pres vol)If any combination was

successful in addressing the question then develop

a theory based on that catalyst and condition.

Distinguish among the terms: Atom: Smallest particle of an element Element: Substances that are composed of one type of atom

Compounds: Pure substances composed of two or more different atoms

Physical Change: Change in matter that does not involve chemical composition Chemical Change: Change in matter that does involve chemical composition

<<< Physical Change

Chemical Change >>>

Memorize the names and symbolsfor the following:

H, He, Li, Na, K, Mg, CaMn, Fe, Ni, Cu, Zn, Au, Ag, Hg, WAl, Sn, PbC, N, O, F, P, S, Cl, Br, IHe, Ne, Ar

1.3 Significant Figures (applies to measured values only)

Recognize the number of significant figures in experimental (measured) values

For a particular measure device, accuracy is associated to the number of significant figures

1.3 – Apply Scientific Notation to Data ▪ Used to represent very large or very small

numbers as powers of 10 ▪ Examples: 0.00002 is written as 2 x 10-5 2,000,000 is written as 2 x 106 ▪ Coefficient criteria ▪ Base 10 with exponent ▪ Multiply and divide

1.4 & 1.5 – Making Measurements & Performing Conversions… Know the three Metric base units Meters (m) - Length

Liters (l) - Volume Grams (g) - Mass

Know how to convert… 1) Within the metric system Metric – use of Table 1.2

giga

mega

kilo

deci

centi

milli

micro

nano

109

106

103

10-1

10-2

10-3

10-6

10-9

G

k

d

c

m

n

Prefix ValueSymbol

M

Know how to convert… 2) Between the English & the Metric systems –

use Table 1.3 Length

1 in. = 2.54 cm1 m = 39.37in.

1 mile = 1.609 km

Mass1 oz1 lb1 kg

===

28.35 g453.6 g2.205 lb

Volume

1 qt1 gal

1 L

===

0.946 L3.785 L33.81 fl oz

1 L = 1.057 qt1 fl oz = 29.57 mL1 g = 15.43 grains

Temperature oC: degrees Celcius oC = 5/9(oF – 32)

oF: degrees Fahrenheit oF = 9/5 oC + 32 K: Kelvin K = oC + 273

Know how to convert… 3) Between the temp systems

1.6 Distinguish among the three States of Matter

• GasGas – has no definite shape or volume.– expands to fill whatever container it is put into.– is highly compressible.

• LiquidLiquid– has no definite shape but a definite volume.– is only slightly compressible.

• SolidSolid– has a definite shape and volume.– is essentially incompressible.

1.7 Density & Specific Gravity Understand both as a physical property Define density…

…in general as mass/volume …specifically as grams/mL for solids and liquids grams/L for gases

Carry out problems using density Determining density Using density as a conversion factor

Define specific gravity (SG) as a unitless value related to density SG = density of substance/density of water

1.9 Make the relationship between heat and temperature ▪ Heat is thermal energy in the units of calories or joules ▪ Changes in temperature occur when is transferred ▪ Understand that the Specific Heat of a substance relates

heat to temperature - see Table 1.4 ▪ Know how to predict the relative amount of heat needed to

heat two different substances

WaterIceSteamIronAluminumCopperLead

WoodGlassRockEthanolMethanolEther

1.000.480.480.110.220.0920.038

0.420.220.200.590.610.56

Acetone 0.52

Substance SubstanceSpecific Heat(cal/g •°C)

Specific Heat(cal/g •°C)

Carbon tetrachloride0.21

Drug Dosage and Body Mass

Covered during “lab”