“I’m Curious…”: Generate a list of at least three things that you’re most curious about...
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Transcript of “I’m Curious…”: Generate a list of at least three things that you’re most curious about...
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Warm-up
“I’m Curious…”: Generate a list of at least three things that
you’re most curious about in chemistry.
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Review and Recall
The Study of Chemistry
Properties of Matter
Units of Measurement
Uncertainty in Measurement
Dimensional Analysis
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The Study of Chemistry
Essential Question (E.Q.): Can I explain from my perspective what chemistry is about and why it is useful to learn chemistry?
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The Study of Chemistry
Study of composition and behavior of matter.
Matter – Physical material of the universe. Has mass, occupies space, and created by elements.
Atom – Building block of matter.
Element – Basic particles created by atoms. 117 are currently known!
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The Study of Chemistry
Every change in our observable world has its basis in the world of atoms.
We’ll speak in terms of two realms: Macroscopic (Macro = large) Submicroscopic ( Atoms, compounds, and
molecules.
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“Coach Lightfoot…Why Study Chemistry???”
Understand how the world works Extremely practical! Public concern Environmental protection Food, clothing, and shelter Food production Understand how chemicals effect us
Chemistry – THE CENTRAL SCIENCE
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Chemistry Put to Work…
Top Eight Chemicals Produced by the Chemical Industry
Rank
Chemical Formula
2006 Production
Principal Uses
1 Sulfuric Acid H2SO4 79B pounds Fertilizers
2 Ethylene C2H4 55B pounds Plastics, antifreeze
3 Lime CaO 45B pounds Paper, cement
4 Propylene C3H6 35B pounds Plastics
5 Phosphoric acid H3PO4 24B pounds Fertilizers, Coca-Cola
6 Ammonia NH3 23B pounds Fertilizers
7 Chlorine Cl2 23B pounds Bleaches, plastics
8 Sodium hydroxide
NaOH 18B pounds Aluminum production, soap
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Household Chemicals
Baking Soda Borax Clorox™ Hydrogen Peroxide Pepto-Bismol™ Vinegar Windex™ Zerex™ (Antifreeze)
Sodium bicarbonate Sodium borate Sodium hypochlorite Hydrogen peroxide Bismuth subsilicate Acetic acid Acetic acid Ethylene glycol
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Chemistry and Life!
Plants Respiration Plant Defense Seasonal Change
Animals Respiration Defense/Immunity Growth and reproduction
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Take 2min. Try these with your neighbor!
Discuss what chemicals you’d like to learn more about.
*Explain from your perspective what chemistry is about and why its useful to learn chemistry.
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Summary…
What is chemistry about? What is matter composed of? Where is chemistry useful?
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See you Later!Study your notes!
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Warm-Up
In a brief paragraph, opine how cooking and chemistry are alike.
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Review and Recall
The Study of Chemistry
Properties of Matter
Units of Measurement
Uncertainty in Measurement
Dimensional Analysis
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Properties of Matter
E.Q.: Can I identify and explain the different properties of matter?
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Properties of Matter
Each substance has a unique set of properties.
These properties can be physical or chemical.
Physical Property – Physically observable properties (color, odor, density, melting point, boiling point, and hardness).
Chemical Property – Describes a substance by its identity (reactivity and flammability).
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Properties of Matter
Observe the image...
With physical and chemical properties come physical and chemical changes!
Copper is red-brown, opaque, solid: physical properties.
Ethanol is flammable: a chemical property.
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Physical and Chemical Changes
Physical Property – Changes physical appearance but not its chemical identity. Ex. Changes of state: boiling, freezing,
sublimation, etc.
Chemical Property – Changes a chemical identity. Ex. Chemical reactions
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Key Terms: Properties
Physical change - No change in composition.
No new substances are formed. Ex. Evaporation; melting;
cutting wood; dissolving sugar in water.
Chemical change or chemical reaction - A change in composition.
New substances are formed. Ex. Burning gasoline;
dissolving metal in acid; spoilage of food.
The liquid fuel evaporates: a physical change.
The vapor burns, combining with oxygen: a chemical change.
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Separation of Mixtures
Because each component of mixtures has its own properties, we can separate a mixture into its components. Three methods:
Chromatography
Distillation
Filtration
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Take 2min. Try These!
Identify each as a physical or chemical change: Photosynthesis Water vapor in the air on a cold day forms frost.
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Summary…
What are the properties of matter? What type of changes can matter undergo? What are the three types of separation
techniques?
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See You Later!Study Your Notes!
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Warm-Up
In a brief paragraph, explain everything you know about units of measurement.
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Review and Recall
The Study of Chemistry
Properties of Matter
Units of Measurement
Uncertainty in Measurement
Dimensional Analysis
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Units of Measurement
E.Q.: How do I explain the importance of accurate units of measurement in chemical and physical processes?
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Units of Measurement
Many properties of matter are quantitative. Quantitative – Relating to NUMBERS!
When a number represents a measurement, its units must be specified.
The units used for scientific measurement are those of the metric system.
In 1960, an international agreement was reached to expressed a choice of metric units – SI Units.
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SI Base Units
SI Base UnitsPhysical Quantity Name of Unit Abbreviation
Mass Kilogram kg
Length Meter m
Time Second s
Temperature Kelvin K
Amount of Substance Mole mol
Electric Current Ampere A
Luminous Intensity Candela cd
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Metric Prefixes
Metric PrefixesPrefix Abbreviation Meaning Example
Tera T 1012 1 gigameter (Tm) = 1 x 1012 m
Giga G 109 1 gigameter (Gm) = 1 x 109 m
Mega M 106 1 megameter (Mm) = 1 x 106 m
Kilo K 103 1 kilometer (km) = 1 x 103 m
Deci d 10-1 1 decimeter = 1 x 10-1 m
Centi c 10-2 1 centimeter = 1 x 10-2 m
Milli m 10-3 1 millimeter = 1 x 10-3 m
Micro μ 10-6 1 micrometer = 1 x 10-6 m
Nano n 10-9 1 nanometer = 1 x 10-9 m
Pico p 10-12 1 picometer = 1 x 10-12 m
Fempto f 10-15 1 femptomenter = 1 x 10-15 m
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Temperature
Measure of the hotness or coldness of an object.
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Derived SI Units
Speed
Force
Pressure
Energy
Density…The only one that we’ll look at!
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Volume
Burette
Syringe
Pipette
Graduated Cylinder
Volumetric Flask
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Density
Property of matter defined as the amount of mass in a unit of volume of substance.
Usually expressed in grams per milliliter (g/mL).
More dense items sink; less dense float!
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Chemistry in the News!!!
Biofuels
New element created (Element 118)
Antibiotic Modified to Combat Bacterial Resistance
The Hole Story (Ozone)
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Take 2min. Try These!
Calculate the density of 18.0g of mercury occupying a volume of 100.0mL.
Indicate the SI units for mass, length, volume, and temperature.
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Summary…
Units of Measurement…
Density…
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See You Later!Study Your Notes!
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Warm-Up
What is meant by the term “Uncertainty”?
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Review and Recall
The Study of Chemistry
Properties of Matter
Units of Measurement
Uncertainty in Measurement
Dimensional Analysis
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Uncertainty in Measurement
E.Q.: Can I realize the relationship between accuracy and precision?
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Uncertainty in Measurement
Two types of numbers are encountered in scientific work:
Exact numbers (1 dozen = 12, 1.0m = 100cm)
Inexact numbers (Numbers obtained by measurement)
Which of the following is an exact number? Number of students in class OR mass of a penny
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Precision and Accuracy
PRECISION
How closely many measurements agree with one another
ACCURACY
How closely many measurements agree with the “correct” value
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Significant Figures (aka Sig Figs)
Uncertainties always exist in measurements.
These uncertainties are shown by significant figures.
Significant figures - All digits of a measured quantity.2.2g = 2 sig figs 5.46g = ______ sig figs
2.2405g = 5 sig figs 1.67g = ______sig figs
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3 Rules for Sig Figs…
Zeros between nonzero digits are always significant – 1005kg (four); 1.03kg (three)
Zeros at the beginning of a number are never significant – 0.02L (one); 0.0026L (two)
Zeros at the end of a number are significant if number contains a decimal – 0.0200kg (three)
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Significant Figures in Calculations
General: Base the number of digits in a result on the measurements and not on known values (such as atomic masses, accurately known densities, other physical constants, etc.)
Multiplication and division: Use the same number of sig figs in the result as the
data with the fewest sig figs. Addition and Subtraction:
Use the same number of decimal places in the result as the data with the fewest decimal places.
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Significant Figure Fun!
WE GO LUNCH AT 11:42004332233AM!!!
I WEIGH 187.0004LBS!!!
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Try These!
The width, length, and height of a small box are 15.5cm, 27.3cm, and 5.4cm. Calculate the volume of the box using correct sig figs!
10.5m x 100.00m = _________m2
(3.2 + 12.00)g = _________g
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Summary…
Uncertainty in Measurements… Accuracy vs. Precision… Sig Figs…
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See You Later!
Try these at home:
3.45g + 5.00g = _________g
100.5m - 10.00m = _________m2
2.30m x 5.00m = _________m2
100.00m2 / 10.00m = _________m2
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Warm-Up
In your own words, define analysis.
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Review and Recall
The Study of Chemistry
Properties of Matter
Units of Measurement
Uncertainty in Measurement
Dimensional Analysis
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Dimensional Analysis
E.Q.: How is dimensional analysis used to solve scientific problems?
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Dimensional Analysis
An aid in problem solving
Units “cancel out” to yield proper answers.
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Dimensional Analysis
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Try this! Take 2min...
If a woman has a mass of 115lb, calculate her mass in grams. (HINT: 1.0lb = 453.6g)
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Two or More Conversion Factors
We also have conversion factor that convert from one measure to a different measure.
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Try this! Take 2min...
The average speed of a nitrogen molecule in air is 515m/s. Convert this speed to miles per hour (mph). (1600m = 1.0mi)
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Try this!
A car travels 28mi per gallon (mpg) of gasoline. Convert these unit to km per liter (km/L). (HINT: 3.8L = 1.0 gallon).
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Try these!
Using your knowledge of metric units, convert the following: 0.076L to mL 0.05m to mm 5.0 days to seconds.
ACCELERATED: Try these also! Speed of light is 3.00 x 108m/s to miles per hour
(mph) 5.85gal/hr to liters per second (L/s)
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Summary...
Dimensional analysis... Measurement conversions...
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See You Later!Study your notes!