chapter #1 spring 2008
TRANSCRIPT
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MatterAnd
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Chemistry
The study of
1. Matter
2. Properties of matter.
3.Changes that matter undergoes.
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Scientific Method
A systematic approach to solving problems.
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Qualitative Observation
• An observation that does not involve any numerical information.– Carbon monoxide is a poisonous gas– Soap is slippery– Gold does not rust– Aluminum has a low density– Tin is a shiny, gray metal
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Quantitative Observation
• An observation involving numerical values in a measurement.– Carbon dioxide freezes at -78ºC– The density of aluminum is 2.70 grams/mL– The sample of gold weighs 34.6 grams– The chemical reactions liberates 45.5 calories
of energy
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Matter
Anything that has mass and takes up space.
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Matter
• Atoms are the building blocks of matter.
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Matter
• Atoms are the building blocks of matter.• Each element is made of the same kind of atom.
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Matter
• 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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Classification of Matter
• Elements (Pure)
• Compounds (Pure)
• Mixtures (Impure)
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Elements
• Elements are the simplest form of matter that can exist under conditions that we normally encounter in the laboratory
• An element is a substance that cannot be separated into simpler substances by chemical methods.
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Elements
• 113 Elements have been identified.
• 82 Elements occur naturally on Earth– Gold, Aluminum, Lead, Oxygen, Carbon
• 31 Elements have been created by scientists.– Technetium, americium, seaborgium
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Elements
• Elements can exist in either the atomic or molecular forms.– Neon Ne
– Hydrogen H2
– Bromine Br2
– Phosphorus P4
– Sulfur S8
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States of Matter
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Compound
A compound is a substance composed of atoms of two or more elements chemically combined in fixed proportions (by either mass or atoms).
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Compounds
• A compound does not change its identify in physical changes but can be broken down into its constituent elements by chemical methods.
• The simplest unit of a compoud is the molecule or ion-pair.
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Carbon Dioxide
• 44.01 grams of carbon dioxide contains 12.01 grams of carbon and 32.00 grams of oxygen. (2.66 : 1.00 ratio of oxygen to carbon).
• 1 molecule of carbon dioxide contains 1 atom of carbon and two atoms of oxygen.
• Carbon dioxide contains 27.29% carbon and 72.71% oxygen (by mass).
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Compounds
• Carbon dioxide CO2
• Magnesium oxide MgO
• Sodium Phosphate Na3PO4
• Sucrose C12H22O11
• Penicillin C14H21N3O6S
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Mixtures
• Mixture – A combination of two or more substance in which the substances retain their distinct identities.– Seawater– Sand in water– Coca-Cola– Bronze alloy– Atmospheric gases– Italian salad dressing
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Characteristics of Mixtures
• Variable composition.
• Variable physical properties.
• Separated into their components by physical methods.– Boiling– Filtration– Decanting
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Homogenous vs. Heterogeneous
• Homogeneous – Uniform throughout sample; no boundaries and separate phases.
• Heterogeneous – Non-uniform throughout sample; boundaries and multiple phases are present.
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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 of Matter
• Intensive Properties:□ Independent of the amount of the
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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Properties of Matter
• Physical Properties
• Chemical Properties
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Physical Properties
• Physical Properties:□ Can be observed without changing a substance
into another substance.• Physical state (gas, liquid, solid) • Mass• Volume• Color/Luster• Hardness• Boiling point • Melting point• Density
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Chemical Properties
• Chemical Properties:□ Can only be observed when a substance is
changed into another substance.• Flammability or combustibility • Corrosiveness• Reactivity with acid, etc.
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Changes of Matter
• Physical Changes:□ Changes in matter that do not change the
composition of a substance.• Changes of state, temperature, volume, etc.• Freezing• Boiling• Melting• Condensation• Sublimation• Dissolving sugar in water`
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Chemical Changes
• Chemical Changes:□ A change in which one or more kinds of
matter is transformed into a new kind of matter or several new kinds of matter.
□ Changes that result in new substances.□ Chemical composition is altered.
• Combustion • Oxidation • Decomposition etc.
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Chemical Reactions
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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Electrolysis of Water
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Example of Chemical Change
• Magnesium metal combusts to produce the white ash, magnesium oxide.
2 Mg(s) + O2(g) → 2 MgO(s)
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Example of Chemical Change
• Sodium reacts vigorously with water to produce hydrogen gas and an aqueous solution of sodium hydroxide.
2 Na(s) + 2 H2O(l) → H2(g) + 2 NaOH(aq)
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Separation of Mixtures
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Distillation:
Separates homogeneous mixture on the basis 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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Measurements
• Numerical Value
• Uncertainty
• Units
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Significant Figures
• When physical quantities are used in arithmetic, it is important that the number of digits reported represents the uncertainty in the original measurements.
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Significant Figures
• Rule #1: Any digit that is not zero is significant.
• 12.345 grams
• Rule #2: Zeros between nonzero digits are significant.
• 20.05 mL
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Significant Figures
• Rule #3: Zeros to the left of the first nonzero digit are not significant.
• 0.0125 kg
• Rule #4: If a measured number is greater than “1”, then all zeros to the right of the decimal point are significant.
• 2.500 meters
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Significant Figures
• Rule #5: If a number is less than “1”, then only the zeros that are at the end of the number and in the middle of nonzero digits are significant.
• 0.2500 grams
• 0.06050 tons
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Significant Figures - Multiplication or Division
• The number of significant figures in the result of multiplication or division is set by the original number that has the smallest number of significant figures.
• 4.51 x 3.6666 = 16.536366
• 16.5
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Significant Figures
0.0608 x 1025.40
25.06
= 2.487802075
2.49
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Significant Figures - Addition or Subtraction
• The answer cannot have more digits to the right of the decimal point than any of the original numbers possess.
• 89.332 + 1.1 = 90.432
• 90.4
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Exact Numbers
• Numbers from definitions or numbers of objects are considered to have an infinite number of significant figures.
(i.e. conversion factors, counting numbers• The average of three measured lengths: 7.65
m, 7.49 m, and 7.60 m.• (7.65 + 7.49 + 7.60)/3 =
• 7.58 not 8
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Uncertainty in Measurements
Different measuring devices have different uses and different degrees of accuracy.
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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 several measurements to each other.
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SI Units
• 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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Volume
• The most commonly used metric units for volume are the liter (L) 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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Conversion Factors
• Length --- 1 meter = 39.37 inches
• Mass --- 453.6 grams = 1 pound
• Volume --- 1 liter = 1.056 quarts
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Dimensional Analysis Method of Solving Problem
• Determine which unit conversion factor(s) are required.
• Carry units through calculation.
• If all units cancel except for the desired unit(s), then the problem was solved correctly.
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Temperature
A measure of the average kinetic energy of the particles in a sample.
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Temperature• In scientific
measurements, the Celsius and Kelvin scales are most often used.
• The Celsius scale is based on the properties of water.□ 0C is the freezing point
of water.□ 100C 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.
• There are no negative Kelvin temperatures.
• K = C + 273.15
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Temperature
• The Fahrenheit scale is not used in scientific measurements.
F = 9/5(C) + 32 C = 5/9(F − 32)
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Density
Physical property of a substance
d=mV