chemistry chapter 2. scientific method serendipity has played a role in science most of what we...
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quantitative data -involves numbers measurements using rulers, thermometers, graduated cylinders, etc. for ex- temp 25 o C qualitative data - is descriptive for example- sulfur is a yellow chemicalTRANSCRIPT
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MEASUREMENTS AND
CALCULATIONS
ChemistryChapter 2
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Scientific Method serendipity has played a role in science most of what we know has come by
careful research and experimentation scientific method- logical approach to
solving problems by observing, collecting data, formulating hypotheses, testing hypotheses, & formulating theories supported by data
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quantitative data-involves numbers
measurements using rulers, thermometers, graduated cylinders, etc.
for ex- temp 25oC
qualitative data- is descriptive
for example- sulfur is a yellow chemical
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experiments are controlled to test one variable and collect data
system- a specific portion of matter in a given region of space is studied in an experiment or observation
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when scientists have a question they want answered, they usually state it in an “if-then” statement
hypothesis- testable statement (if-then)
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control- part of experiment that remains the same
variable- part of experiment that is changed
during the experiment, any change observed is usually due to the effects of the variable
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Units of Measurement What is wrong with this recipe?
Banana Nut Bread3 flour 1 vanilla2 eggs 2 mashed bananas2 sugar ½ nutmeg
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measurements represent quantities
quantity- something that has magnitude, size, or amount (UNIT)
most ALL m’ments are a NUMBER and a UNIT
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SI System a standard system of m’ment 7 base units system is monitored by International
organizations
commas are NOT used in numbers = for example: 75 000 not 75,000
(many other countries use commas as decimal points)
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few differences between SI system and metric
base units specific for certain quantities(table 1)
prefixes are used to indicate quantities larger or smaller than the base unit
prefixes are based on 10 (table 2)
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Most common prefixes kilo– means 1000 deci– means tenth (0.1) centi- means hundredth (0.01) milli- means thousandth (0.001)
commit these to memory
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the prefixes are used with the base units to measure larger or smaller quantities
for ex: length of room- meterdistance to Sylacauga-kilometerlength of book- centimeterwidth of fingernail- millimeter
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MASS measure of the
quantity of matter
base unit:SI- kilogrammetric- gram
triple-beam balance
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Weight measure of the
force of gravity between 2 objects
can change, mass DOESN’T
SI unit - Newton scale
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Time interval
between 2 occurrences
SI unit- seconds
stopwatch/clock
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Length distance
between 2 points
SI unit- meter
ruler
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Temperature
matter is composed of molecules, ions, and atoms which are in constant motion (i.e. have kinetic energy)
temp measure of the average kinetic energy of all these particles
increase heat, increase movement of particles, increase KE
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SI unit- Kelvin (K)measures extreme
temps metric- Celsius
(oC) based on the
freezing and boiling point of water
thermometer
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Derived Units combinations of SI
units produced by
multiplying or dividing std units
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Volume amount of space an
object takes up SI unit- 1m3
metric- liter (L)1cm3 and 1mL are
smaller and usually used in the lab
1cm3 = 1mL graduated cylinder
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Volume can be calculated using a ruler
and this formula: v = l x w x h volume relationships:
1dm3 = 1L = 1 000cm3 = 1 000mL1 000mL = 1 000cm3
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Density mass per unit volume density = mass
volumeD = m v
units can be g/mL, g/cm3 (whatever units are used to measure mass and volume will be the units of density
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can be used to identify substances
can use the formula to find mass or volume also
density of H2O = 1g/mL
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How reliable are the measurements you make? 2 important terms indicate
reliability:1. accuracy- how close the m’ment is
to the true value2. precision- how close a set of
m’ments for a quantity are to each other (regardless of accuracy)
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% error used to evaluate results
obtained in lab always positive number % error =
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An automobile is traveling at 88 km/h. What is its speed in cm/s.
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Density pop quiz1. A 30.0 cm3 sample of quartz has a
density of 2.65g/cm3. What is the mass?2. The density of a sample of cork is
0.24g/cm3. What is the volume of a 35.0g sample?
3. What is the density of a piece of marble with the following dimensions: 552g and 212 cm3?
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Significant Digits In science, significance means
measured, not importance.
the # of sig digs in a m’ment depends on the scale of instrument used
m’ment includes 1 uncertain, or estimated, digit
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To find sig digs:1. find decimal point2. find 1st non-zero digit in the sequence3. that digit and everything to the right
is significant4. if no decimal point, count from the 1st
non-zero digit to the last non-zero digit
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10.00.0022 000 00025.0010
0.100260100 1002.550
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when doing calculations on calculator, the answer cannot have any more sig digs than the value in the problem
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answers in addition & subtraction must contain no more digits to the right than the # with the least digit to the right in the prob
52.63- 12.4
40.23=40.2
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answer in multiplication or division must contain no more sig digs than the # with the fewest digits in the prob
18.3x 1.4
25.62=26
5.356x 0.793
4.247308=4.25
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Rounding Rules1. # 1-4 round down
21.31 =21.3
2. #6-9 round up36.7 = 37
3. # 5 -round down if # preceding 5 is even32.5 = 32 688.5 = 688
round up if # preceding 5 is odd43.5 = 44 759.5 = 760.
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4. if there are #s after the 5, round up no matter what the preceding # is
42.52 = 43 78.571 = 79
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Scientific Notation very small and very large numbers are written
in this shorthand method
#s are written in this format:M x 10 n
M = 1 to 9.999n = whole number exponent
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convert into sci not:650 000 000
6.5 x 108
0.000 000 974
9.74 x 10-7
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convert into std numbers:3.8 x 104
38 000
1.25 x 10-3
0.001 25
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adding/subtracting in sci not exponents must be same
moving decimal to LEFT increases exp
moving decimal to RIGHT decreases exp
4.5 x 105
+ 3.1 x 107
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multiplying/dividing in sci not multiply – ADD exponents
divide- SUBTRACT exponents
2.74 x 103 x 3.1 x 108 =
9.58 x 104
3.7 x 106
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Proportions: 2 types1. direct proportions- if 2
quantities can be divided and you get a constant value
y=kx
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results in a straight line
as x increases, y increases
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2. two quantities are inversely proportional if their product is constant
xy = k
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forms a hyperbola
if x increases, y must decrease