explain why a knowledge of chemistry is central to many human endeavors. list and describe the steps...
TRANSCRIPT
CHAPTER 1: CHEMISTRY AND YOU
Explain why a knowledge of chemistry is central to many human endeavors.
List and describe the steps of the scientific method.Explain the basic safety rules that must be followed when working in the
chem lab.Identify the metric units of measurement used in chemistry.
Explain what causes uncertainty in measurements.Compare accuracy and precision.
Explain how to use significant figures and scientific notation.Calculate percent error.
Define density and explain how it is calculated.Explain how dimensional analysis and conversion factors are used to
solve problems in chemistry.
Vocab
Chemistry Scientific method Observation Hypothesis Experiment Conclusion Natural law Theory Variable Experimental control Metric system International System of
Units (SI)
Base unit Mass Volume Metric prefix Precision Accepted unit Accuracy Significant digit Percent error Density Dimensional analysis Conversion factor
Chapter 1: Chemistry and You
Look at the pic on p. 2 and read the caption Name some of the
basic chemical substances that make up your body.
Name some other chemical processes, besides digestion, that occur in your body.
Can you think of an important chemical reaction that occurs in plants and trees?
Section 1-1What is Chemistry?
Chemistry in Action
Chemistry is a broad science that touches nearly every aspect of human life.
What are some ways chemistry affects the 2 careers mentioned in the section? Examining a wetlands habitat Preserving historical artifacts
The Central Science
Chemistry has been called the central science b/c it overlaps so many sciences
Careers that use chemistry Hair stylists Construction Biologists What others?
Possible chemistry careers Police departments (CSI) Perfume companies Research chemists
Why Study Chemistry?
It is involved in many aspects of life Helps you to understand the world
around you
Cleaning Priceless Art
Read the “Connection” box on p. 6 What occupation is using chemistry? What did they do to clean the art? Why are some people upset about their
actions?
Section 1-2The Scientific Method
The Scientific Method
A way of answering questions about the world we live in
Oscar Has Extremely Colorful T-Shirts
Observation
Question
Hypothesis
Experiment
Conclusion
Natural Law
Theory(Model)
Prediction
Experiment
Theory modifie
d as needed
Observation
Seeing a problem or asking a question that you cannot answer
Always leads to a question
Hypothesis
An educated guess Usually asked in a “cause-effect”
statement Must be able to test the hypothesis
Experiment
A test of the hypothesis
Data will be collected and analyzed
Must have 1 variable and at least 1 constant Variable – the
particular factor being tested
Conclusion
The result of the analyzed data May agree or disagree with your
hypothesis
Theory
Answers the original question as well as any others formed during the process
Predicts the results of further experiments
Scientific/Natural Law
Describes how nature behaves but not why
1-2 Section Review
On looseleaf to turn in, page 13 (1-5)
Bikini Bottom Experiments
With your small group, complete the SpongeBob worksheet
SpongeBob Scientific Method.pdf
Section 1-3Safety in the Lab
Section 1-4Units of Measurement
Units of Measurement
Measurement: always includes a number and unit If someone is 7 feet tall, “7” is the number and
“feet” is the unit Saying someone is 7 does not tell you enough
info They could be 7 yrs old, 7 feet tall, 7 inches tall, …
Feet and inches are part of the English system of measurement
In science, we use the Metric system All scientists, no matter their country or
language, use the metric system
United States, Liberia, and Burma
International System of Units
SI units used by all scientists around the world
Based on 7 metric units called base units Length meter (m) Mass kilogram (kg) Time second (s) Count/Quantity mole (mol) Temperature Kelvin (K) Electric Current ampere (A) Luminous Intensity candela (cd)
Derived Units
Area square meter (m2)Volume cubic meter (m3)Force Newton (N)Pressure Pascal (Pa)Energy joule ( J )Power watt (W)Voltage volt (V)Frequency hertz (Hz)Electric charge coulomb (C)
Units
Science is a process, not a collection of rules
The most frequently used units in class that differ than SI: Temperature - Celsius (˚C) Volume – liter (L) Pressure – atmosphere (atm)
millimeters of mercury (mmHg)
Energy – calorie (cal)
Commonly used units
Length A dime is 1 mm thick A quarter is 2.5 cm in diameter Average height of a man is 1.8 m
Mass A nickel has a mass of 5 g A 120 lb woman has a mass of about 55 kg
Volume A 20 oz can of soda has a volume of 360 mL A ½ gallon of milk is equal to 2 L
Metric Prefixes
Prefix Abbreviation
Meaning
kilo- k 1 000
hecta- H 100
deca- D 10
Base Unit 1
deci- d 0.1
centi- c 0.01
milli- m 0.001
KingHenry Died by drinking chocolate milk
Base units include meter, liter, second, gram
How to Use Prefixes
kilo-
hecto-
deca-Base units
deci-
centi-
milli-
Example
kilo-
hecto-
deca-base units
deci-
centi-
milli-
How many millimeters are in a meter?1 meter = mm
1 meter = 1000 mm
Practice Problems
Convert a volume of 16 deciliters into liters 1.6 L
Convert 1.45 meters into centimeters 145 cm
Convert a volume of 8 deciliters into liters 0.8 L
Is 5 centimeters longer or shorter than 8 millimeters? Explain. 5 cm is longer than 8 mm b/c 0.05 m is
greater than 0.008m
Metric ManiaWorksheet
Section 1-5Uncertainty in Measurement
Making Measurements
When making a measurement, write down everything given to you with one uncertain estimated number 5.1 inches is easy to spot but we still
need 1 uncertain number My estimation = 5.12 inches
Measurements are uncertain b/c: Measuring instruments are never completely
free of flaws Measuring always involves some estimation
Reliability in Measurement
Precision: the same result is given over and over under the same conditions
Accuracy: the result is close to a reliable standard
Accepted value: the reliable standard
High PrecisionHigh Accuracy
Section 1-6Working with Numbers
Working with numbers
Measurements are rarely used just by themselves.
Usually used in some form of mathematics (+, -, x, or ÷)
Produces values of mass, temperature, volume, etc.
Significant Figures (Digits)
The certain digits and the estimated digit of a measurement Example: In the # 31.7, there are 3 sig figs
The 3 and 1 are certain digits while the 7 is the uncertain digit
Rules for Sig Figs
Nonzero #: any number that is not a zero 1, 2, 3, 4, 5, 6, 7, 8, or 9
Zeros Never count “leading zeros”
0023 only count the 2 and 3 0.054 only count the 5 and 4
Always count “captive” or “sandwiched” zeros 303 count the 3, 0, and 3
“Trailing zeros”: zeros to the right Only count if used with a decimal point
5400 only count the 5 and 4 5.400 count the 5, 4, 0, and 0
Example
How many sig figs are in 0.057 010 g? Nonzero numbers:
0.057 010 Captive zeros
0.057 010 Trailing zeros when there is a decimal
0.057 010 Final Answer
0.057 010 5 significant figures
Practice Problems
How many sig figs in the following numbers? 0.002 6701 m
5 sig figs 0.002 6701 19.0550 kg
6 sig figs 19.0550 3500 V
2 sig figs 3500 1 809 000 L
4 sig figs 1 809 000 95 600 m
3 sig figs 95 600 520 mL
2 sig figs 520 0.0102 ms
3 sig figs 0.0102
Sig Fig Practice Wkst
Significant Figures in Calculations
Multiplying and Dividing The answer will have the same # of sig
figs as the measurement with the smallest # of sig figs
Volume = 3.052 m x 2.10 m x 0.75 m (4 sig figs) (3 sig figs) (2 sig
figs)
= 4.8069 m3
= 4.8 m3
Sig Figs in Calculations
Adding and Subtracting The answer will have the same # of decimal
places as the measurement with the smallest # of decimal places
951.0 g 1407 g 23.911 g + 158.18 g 2540.091 g Since there aren’t any decimals in 1407, our
answer will not have decimals Final answer = 2540 g
Practice Problems
6.15 m x 4.026 m = 24.7599 m2 = 24.8 m2
1.45 m x 1.355 m x 2.03 m = 3.9884425 m3 = 3.99 m3
0.3287 g + 45.2 g = 45.5287 g = 45.5 g
0.258 mL ÷ 0.361 05 mL = 0.71458246 mL = 0.715 mL
More PracticeWorksheet
Scientific Notation
In science we work w/ very large and very small #s
For example: 1 drop of water contains =
1,700,000,000,000,000,000,000 molecules The mass of 1 proton =
0.000 000 000 000 000 000 000 000 001 672 62 kg
Scientific Notaion
To make it easier for ourselves, we use scientific notation 1 drop of water contains =
1,700,000,000,000,000,000,000 molecules 1 drop of water contains = 1.7 x 1021
The mass of 1 proton = 0.000 000 000 000 000 000 000 000 001 672 62 kg
The mass of 1 proton = 1.67262 x 10-21
How to make # into scientific notation
Write 1700 in scientific notation Write down the full number
1700 Move the decimal until it is right after the first
1-10 number 1700 1700. 1.700
Write down this new number without the zeros 1.7
Place “x 10” after this number 1.7 x 10
Count how many times you had to move the decimal and place that number after the 10 as an exponent
If you move to the right = negative exponent If you move to the left = positive exponent
1.7 x 103
Examples
37 700 3.77 x 104
1 024 000 1.024 x 106
0.000 000 003 901 3.901 x 10-9
8960 8.96 x 103
0.000 23 2.3 x 10-4
Percents
Data will often be given as a percent If it is a fraction,
just divide and multiply by 100
Ex: 900 million kilograms of plastic soft drink bottles are produced each year. 180 million kilograms of them are recycled.180 million
kilograms900 million kilograms
= 0.2 x 100% = 20%
Percent Error
A measurement can be compared to its accepted value by finding the percent error
% error can be positive or negative Positive = measured value is greater than
accepted Negative = measured value is less than
accepted% error = measured value – accepted value
accepted valuex 100%
Example
In an experiment dealing with finding the boiling point of water, you performed 3 experiments and found water to boil at 98.4˚C, 98.9 ˚C, and 97.5˚C. What is the average and % error of your data? (Hint: the accepted value of the boiling point of water is 100˚C)
98.4 + 98.9 + 97.5 = 294.8 / 3 = 98.3 % error = (100 – 98.3) / 100 x 100 = 1.7%
PracticeWork the problems on your “Accuracy Precision and Percent Error” worksheet from a few class periods ago
Density
Density – compares the mass of an object to its volume measured in:
grams per cubic centimeters (g/cm3)
grams per milliliter (g/mL)
Density
Mass
Volume=
Density Problems If a sample of aluminum has a mass of
13.5g and a volume of 5.0 cm3, what is its density?
2.7 g/cm3
Suppose a sample of aluminum is placed in a 25 mL graduated cylinder containing 10.5 mL of water. The level of the water rises to 13.5 mL. What is the mass of the aluminum sample? (Use the density you found in the problem before this)
8.1 g
A piece of metal with a mass of 147g is placed in a 50mL graduated cylinder. The water level rises from 20mL to 41mL. What is the density of the metal?
7 g/mL
What is the volume of a sample that has a mass of 20g and a density of 4g/mL?
5 mL
A metal cube has a mass of 20g and a volume of 5cm3. Is the cube made of pure aluminum? Explain. (Hint: Pure Aluminum will have a density of 2.7g/cm3.)
4 g/cm3
Dimensional Analysis
Technique of converting between units How many feet are in 86 centimeters?
We know 12 inches = 1 foot We also know 1 inch = 2.54 centimeters
86 cm 1 in 1 ft2.54 cm 12 in= 2.82 ft
Practice Problems
Use Fig 1-29 on page 38 to help you solve the following problems
How many cubic centimeters are in 2.3 gal? 8 700 cm3
How many meters are in 3.5 mi? 5 600 m
How many pascals are in 770 mm Hg? 103 000 Pa
How many seconds are in 10.5 hours? 37 800 s
How many days are in 12 583 seconds? 0.14564 days
Graphing
How to draw a scientific graph Need independent variable (x – axis)
the variable being changed Need dependent variable (y – axis)
the variable being changed by the independent variable
Label each axis Do not connect each dot, use a “line of best
fit” Give the graph a title which tells what it is of
Example
A balloon is filled with air and attached to the bottom of a large container of water. If the water temperature is changed, by heating or adding ice, the volume of the air in the balloon also changes. Data was collected from taking volume measurements at different temperatures. Independent variable: temperature Dependent variable: volume
Sample Graph
20 30 40 50 60 70 8090
95
100
105
110
115
120
Volume (mL)Trial Temperature
(˚C)Volume
(mL)
1 25 101.3
2 30 103.2
3 35 103.4
4 40 105.0
5 45 106.7
6 50 108.4
7 55 110.0
8 60 111.5
9 65 112.9
10 70 114.2