measurements and calculations
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Chemistry Chapter 2. Measurements and calculations. Scientific Method. serendipity has played a role in science most of what we know has come by careful research and experimentation - PowerPoint PPT PresentationTRANSCRIPT
MEASUREMENTS AND
CALCULATIONS
ChemistryChapter 2
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
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
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
when scientists have a question they want answered, they usually state it in an “if-then” statement
hypothesis- testable statement (if-then)
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
Units of Measurement
What is wrong with this recipe?
Banana Nut Bread
3 flour 1 vanilla
2 eggs 2 mashed bananas
2 sugar ½ nutmeg
measurements represent quantities
quantity- something that has magnitude, size, or amount (UNIT)
most ALL m’ments are a NUMBER and a UNIT
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)
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)
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
the prefixes are used with the base units to measure larger or smaller quantities
for ex: length of room- meter
distance to Sylacauga-kilometer
length of book- centimeter
width of fingernail- millimeter
MASS
measure of the quantity of matter
base unit:
SI- kilogram
metric- gram triple-beam
balance
Weight
measure of the force of gravity between 2 objects
can change, mass DOESN’T
SI unit - Newton scale
Time
interval between 2 occurrences
SI unit- seconds
stopwatch/clock
Length
distance between 2 points
SI unit- meter
ruler
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
SI unit- Kelvin (K)measures extreme
temps metric- Celsius
(oC) based on the
freezing and boiling point of water
thermometer
Derived Units
combinations of SI units
produced by multiplying or dividing std units
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
Volume
can be calculated using a ruler and this formula: v = l x w x h
volume relationships:
1dm3 = 1L = 1 000cm3 = 1 000mL
1 000mL = 1 000cm3
Density
mass per unit volume density = mass
volume
D = m
v units can be g/mL, g/cm3 (whatever
units are used to measure mass and volume will be the units of density
can be used to identify substances
can use the formula to find mass or volume also
density of H2O = 1g/mL
How reliable are the measurements you make?
2 important terms indicate reliability:
1. accuracy- how close the m’ment is to the true value
2. precision- how close a set of m’ments for a quantity are to each other (regardless of accuracy)
% error
used to evaluate results obtained in lab
always positive number % error =
An automobile is traveling at 88 km/h. What is its speed in cm/s.
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?
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
To find sig digs:
1. find decimal point
2. find 1st non-zero digit in the sequence
3. that digit and everything to the right is significant
4. if no decimal point, count from the 1st non-zero digit to the last non-zero digit
10.0
0.002
2 000 000
25.0010
0.100
260
100 100
2.550
when doing calculations on calculator, the answer cannot have any more sig digs than the value in the problem
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
answer in multiplication or division must contain no more sig digs than the # with the fewest digits in the prob
18.3
x 1.4
25.62=
26
5.356
x 0.793
4.247308=
4.25
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 even
32.5 = 32 688.5 = 688
round up if # preceding 5 is odd
43.5 = 44 759.5 = 760.
4. if there are #s after the 5, round up no matter what the preceding # is
42.52 = 43 78.571 = 79
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 9.999
n = whole number exponent
convert into sci not:
650 000 000
6.5 x 108
0.000 000 974
9.74 x 10-7
convert into std numbers:
3.8 x 104
38 000
1.25 x 10-3
0.001 25
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
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
Proportions: 2 types
1. direct proportions- if 2 quantities can be divided and you get a constant value
y=kx
results in a straight line
as x increases, y increases
2. two quantities are inversely proportional if their product is constant
xy = k
forms a hyperbola
if x increases, y must decrease