chapter 1 matter and measurement
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chemistry.TRANSCRIPT
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Chapter 1Introduction:
Matter and Measurement
Chemistry, The Central Science, 10th editionTheodore L. Brown; H. Eugene LeMay, Jr.;
and Bruce E. Bursten
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Matter and Measurement
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Chemistry:
The study of matterand the changes it undergoes.
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Scientific Method:
A systematic approach to solving problems.
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Matter:
Anything that has mass and takes up space.
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Matter
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• Atoms are the building blocks of matter.
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Matter
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• Atoms are the building blocks of matter.• Each element is made of the same kind of atom.
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Matter
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• Atoms are the building blocks of matter.• Each element is made of the same kind of atom.• A compound is made of two or more different kinds of
elements.
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States of Matter
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Classification of Matter
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Classification of Matter
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Classification of Matter
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Classification of Matter
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Classification of Matter
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Classification of Matter
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Classification of Matter
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Classification of Matter
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Classification of Matter
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Classification of Matter
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Mixtures and Compounds
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Properties and Changes of
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Changes of Matter
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Properties of Matter
• Physical Properties:□Can be observed without changing a
substance into another substance.
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substance into another substance.• Boiling point, density, mass, volume, etc.
• Chemical Properties:□Can only be observed when a substance is
changed into another substance.• Flammability, corrosiveness, reactivity with
acid, etc.
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Properties of Matter
• Intensive Properties:□ Independent of the amount of the
substance that is present.
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substance that is present.• Density, boiling point, color, etc.
• Extensive Properties:□Dependent upon the amount of the
substance present.• Mass, volume, energy, etc.
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Changes of Matter
• Physical Changes:□Changes in matter that do not change the
composition of a substance.
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composition of a substance.• Changes of state, temperature, volume, etc.
• Chemical Changes:□Changes that result in new substances.
• Combustion, oxidation, decomposition, etc.
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Chemical Reactions
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In the course of a chemical reaction, the reacting substances are converted to new substances.
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Chemical Reactions
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Compounds
Compounds can be broken down into more elemental particles.
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particles.
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Electrolysis of Water
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Separation of
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Mixtures
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Distillation:
Separates homogeneous mixture on the basis of differences in
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of differences in boiling point.
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Distillation
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Filtration:
Separates solid substances from liquids and solutions.
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Chromatography:
Separates substances on the basis of differences in solubility in a solvent.
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Units of
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Measurement
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SI Units
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• Système International d’Unités• Uses a different base unit for each quantity
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Metric System
Prefixes convert the base units into units that are appropriate for the item being measured.
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• Write down an unusual example of a chemical reaction on a piece of paper and give it to me with your name.
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and give it to me with your name.
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• What is the most abundant element on earth?
• What is the most abundant element in
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• What is the most abundant element in the human body?
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Volume
• The most commonly used metric units for volume are the liter (L) and the milliliter (mL).
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and the milliliter (mL).□ A liter is a cube 1 dm
long on each side.□ A milliliter is a cube 1 cm
long on each side.
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1L = 1000 ml
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1L = 1000 ml
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Conversions of units
Length1 km = 1000 meter 1 meter = 100 cm1 cm = 10 mm
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Mass 1 kg = 1000 g1 g = 1000 mg
Volume1 L = 1000 ml
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Temperature:
A measure of the average kinetic energy of the particles in a
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particles in a sample.
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Temperature• In scientific
measurements, the Celsius and Kelvin scales are most often used.
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• The Celsius scale is based on the properties of water.□ 0°C is the freezing point
of water.□ 100°C is the boiling
point of water.
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Temperature
• The Kelvin is the SI unit of temperature.
• It is based on the properties of gases.
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properties of gases.• There are no
negative Kelvin temperatures.
• K = °C + 273.15
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Temperature
• The Fahrenheit scale is not used in scientific measurements.
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measurements.• °F = 9/5(°C) + 32• °C = 5/9(°F − 32)
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Uncertainty in
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Measurement
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Uncertainty in Measurements
Different measuring devices have different uses and different degrees of accuracy.
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Significant Figures
• The term significant figures refers to digits that were measured.
• When rounding calculated numbers, we
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• When rounding calculated numbers, we pay attention to significant figures so we do not overstate the accuracy of our answers.
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Significant Figures
1. All nonzero digits are significant.2. Zeroes between two significant figures
are themselves significant.
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are themselves significant.3. Zeroes at the beginning of a number
are never significant.4. Zeroes at the end of a number are
significant if a decimal point is written in the number.
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Exact numbers
• These numbers are the ones whose values are known exactly.Counted numbers and
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Counted numbers and Conversion factors
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Exact Numbers
• The numbers that are obtained by counting and not by measuring are called exact numbers.
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called exact numbers. Examples:10 apples, 100 students
• Exact numbers also arise by definitionExample : 1 inch is defined as
exactly2.54 cm.
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• Exact numbers can be assumed to have an unlimited number of significant figures.
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figures. • These do not limit the number of
significant figures in a calculation.
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Rules for Multiplication and Division
• When multiplying or dividing numbers, the answer reported can not have more significant figures than either of the
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significant figures than either of the original numbers.
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Rules for Addition and Subtraction
When adding or subtracting numbers, the reported answer can not have more digits after the decimal point than any of
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digits after the decimal point than any of the added numbers.
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Accuracy versus Precision
• Accuracy refers to the proximity of a measurement to the true value of a quantity.
• Precision refers to the proximity of
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• Precision refers to the proximity of several measurements to each other.
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Dimensional Analysis
• This is a very powerful tool for conversion from one unit to another.
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• Those of you who were present in today morning’s discussion, please sign the attendance sheet.
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attendance sheet.
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Dimensional Analysis
Step 1: write the conversion factorsStep 2: write down two equivalence ratiosStep 3: write the number to be converted with the
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unitStep 4: multiply that with the equivalence ratio so
that the unit needed in the answer is on thetop and the unit that needs to go is on the bottom
Step 5: Calculate the answer
Check to see if your answer makes sense
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ExampleConvert 37 cm into meters. • Step 1: write the conversion factors
1m = 100 cm• Step 2: write down two equivalence ratios
1m 100 cm100 cm 1 m
• Step 3: write the number to be converted with the unit• Step 4: multiply that with the equivalence ratio so that the unit
needed in the answer is on the top and the unit that needs to go
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needed in the answer is on the top and the unit that needs to go is on the bottom
37 cm x 1m100 cm
• Step 5: Calculate the answer37 cm x 1m = 0.37 m Answer
100 cm
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Examples
• Convert 37 Km/h to m/s
Km37
1000mx
1hx
1minx
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Km37
h
1000mx
1Km
1hx
60min
1minx
60s
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• Convert 12 g / L to g/ml
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Density:
Physical property of a substance
d=m
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d=mV