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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
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”