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This formula is strictly valid only for ideal gases—those in which the molecules are far enough apart so that intermolecular forces can be neglected. At high pressures, such forces cause significant departure from the Ideal Gas Equation, and more complicated equations have been devised to treat such cases. The Ideal Gas Equation, however, gives useful results for most gases at pressures less than 100 atmospheres. This is the value stated in the carbon dioxide reaction; you were asked to memorize that 1 mole of any gas occupies 22.4 liters at STP. You should be able to use the Ideal Gas Equation to determine any one of the four quantities— pressure, volume, moles, or temperature—if you are given values for the other three. One important application is to deduce the molecular mass and formula for a gas. Assume that you know that the hydrocarbon propylene is, by mass, 85.6% carbon and 14.4% hydrogen. Then the atomic ratios of the compound are Therefore, the propylene molecule is some integral multiple of CH2: It can be CH2 or C2H4 or C3H6 or a yet larger molecule. Measuring the volume of 10 grams of propylene at STP yields 5.322 liters, which you can use to calculate its molecular mass. Because the atomic masses of 1 CH2 unit added together is 14.03, the molecule contains three such units. Consequently, the molecular formula for propylene is C3H6. 5. What is the volume occupied by 1 kilogram of carbon monoxide at 700°C and 0.1 atm? 6. The ozone molecule contains only oxygen atoms. Determine the molecular formula of ozone given that 2.3 grams occupies 1,073 milliliters at standard temperature and pressure. 129
130 The Learning Goal for this assignment is: Students will learn how the interactions between water molecules account for the unique properties of water and how the aqueous solutions form. Take note over the following chapter. Use the Headings provided to organize your notes. Define and number all highlighted vocabulary (total 22 ) as well as summarize and take notes over the sections. You may add pictures where needed. The pictures should be an appropriate size. Use Arial 12 for all text. This document should be 2 pages and should be saved as a pdf before you submit it into Angel. Chapter 15 Water and Aqueous Systems Pages 488 - 507 15.1 Water and Its Properties Water in the Liquid State- Without water life would not be possible. The oxygen atoms within the water form a covalent bond with the atoms of hydrogen. The bond between O-H is highly polar. Dipole interactions attract polar molecules to one another. Covalent bonds are known to be stronger than hydrogen bonds. Despite the previous statement, they are stronger than other intermolecular forces. Water has an inward force or pull that tends to minimize the surface area of a liquid, this is called surface tension 1 . The surface of water acts like a skin. Surface tension is reduced by a surfactant 2 which is any substance that interferes with hydrogen bonding in water molecules Water in the Solid State Water in its solid state has less density than water in its liquid state. It is important for certain organisms that ice floats, because a layer of ice on top of the water acts as an insulator for the water beneath which stops the water from freezing solid with the exception of extreme conditions 15.2 Homogeneous Aqueous Systems Solutions Because of the vast amount of substances that water dissolves when they come in contact with it you will never find water that is chemically pure in nature. All water contains dissolved substances, and this is called an aqueous solution 3 . Within an aqueous solution the medium in which the water is dissolved is refered to as a solvent 4 and the particles being dissolved are called a solute 5. All solutions are homogenous mixtures. The average diameter of solute particles, which can consist of atoms ions or molecules is ussually less than 1 nm. For this reason you can’t separate a solution through filter paper as both the solvent and solute would pass through. Nonpolar covalent compounds do not dissolve in water. In the process called solvation 6 , the positive and negative ions of an ionic solid become surrounded by solvent molecules. Electrolytes and Nonelectrolytes An electrolyte 7 is a compound that conducts an electric current when it is an aqueous solution or in the molten state. In order for an electric current to conduct it needs ions that are mobile, as they are capable of carrying electrical currents through a liquid. Some ionic compounds cannot conduct an electric current in an aqueous solution because they are insoluble, however despite this it does have the ability to conduct in a molten state. Compounds that can’t conduct in either states (aqueous or molten) are called nonelectrolytes 8 . In a solution that contains a strong electrolyte 9 all or almost all of the solute exists of ions. In a solution with a weak electrolyte 10 , only a fraction of the solute exists as ions and therefore it conducts poorly. Electrolytes are essential to all metabolic processes.
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Powered by TCPDF (www.tcpdf.org) Ed
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Table E Selected Polyatomic Ions Fo
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Table H Vapor Pressure of Four Liqu
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Table K Common Acids Table N Select
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Table R Organic Functional Groups C
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Table S Properties of Selected Elem
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Table T Important Formulas and Equa
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CHEMISTRY EXAM FORMULA AND RESOURCE
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Activity Series of Metals Name Symb
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Unit 1 Measurement Lab Separation o
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Unit 5 (28 days) Chapter 10 Chemica
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30. Always lubricate glassware (tub
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Print vs. print Online vs. online P
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To use the Stair-Step method, find
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Using SI Units Match the terms in C
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Standards of Measurement Fill in th
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SCIENTIFIC NOTATION RULES How to Wr
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Convert each number from Scientific
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Significant Figures Rules There are
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How Many Significant Digits for Eac
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The following rule applies for mult
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1qt=32 oz 1gal = 4qts 1.00 qt = 946
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Chapter 6 The Periodic Table The st
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Atoms Are Building Blocks Atoms are
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Electrovalence Don't get worried ab
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Summary 35
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Research the Scientist and summariz
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Electron Configuration Color the su
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Electron Configuration In order to
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10. Name __________________________
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Using Wikipedia, define the 8 categ
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Ionization Energy Define Ionization
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Ion Size Define Ion Size: the size
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The Nucleus A typical model of the
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Gamma Radiation After a decay react
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Nuclear Fission The word fusion mea
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Students will be able to predict sh
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This analysis shows that sodium has
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Metals, with only a few electrons i
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1 2 3 4 5 6 Name of Cation Calcium
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POLAR BONDING results when two diff
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Step 6 Put the atoms in the structu
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Orbitals Equation Lone Pairs Angle
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Carbon Dioxide Chemical Name CO2 Ch
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Hydronium Chemical Name H3O+ Chemic
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Sulfur Hexaflouride Chemical Name S
Page 100 and 101: Bent: They look, well, bent. Bond a
Page 102 and 103: 4. the chlorine atom in hydrochlori
Page 104 and 105: Chapter 23 Functional Groups The st
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Page 108 and 109: anched chains: Hexane - a 6-carbon
Page 110 and 111: Isomers Because carbon can bond in
Page 112 and 113: Chapter 12 Stoichiometry The studen
Page 114 and 115: Other atomic weights are listed on
Page 116 and 117: Find Molecular Mass 1- 10 1. NaBr N
Page 118 and 119: Step 3 Always leave hydrogen and ox
Page 120 and 121: 1) ___ 2 NaNO3 + ___ 1 PbO ___ 1 P
Page 122 and 123: 1) 2 NaNO3 + PbO Pb(NO3)2 + Na2O 2
Page 124 and 125: 4) Double displacement: This is whe
Page 126 and 127: Determine the Type of Reaction for
Page 128 and 129: Volume to Volume Conversions: the a
Page 130 and 131: we can determine that 2 moles of HC
Page 132 and 133: 111 When there is no limiting reage
Page 134 and 135: Example 7 How much 5M stock solutio
Page 136 and 137: Theoretical and Actual Yields Key T
Page 138 and 139: Review Purposes To get an over
Page 140 and 141: Chapter 14 The Behavior of Gases Th
Page 142 and 143: The learning goal for this assignme
Page 144 and 145: • When a particle is heated it st
Page 146 and 147: It is important that you realize th
Page 148 and 149: 3. The pressure of nitrogen gas in
Page 152 and 153: Hydrates the water contained in a c
Page 154 and 155: Create and interpret potential ener
Page 156 and 157: Structure effects: determines what
Page 158 and 159: Specific Heat Here is the definitio
Page 160 and 161: 139 Step One: solid ice rises in te
Page 162 and 163: 141 Step Three: liquid water rises
Page 164 and 165: Step Five: steam rises in temperatu
Page 166 and 167: 145 then it is exothermic, meaning
Page 168 and 169: 147 Define the types of reactions.
Page 170 and 171: 149 1. If this compound was at room
Page 172 and 173: 151 1. In what part of the curve wo
Page 174 and 175: Reduction Oxidation reduction react
Page 176 and 177: So far, the properties have an obvi
Page 178 and 179: The acid base theory of Brønsted a
Page 180 and 181: IV. Problems with the Theory This t
Page 182 and 183: Let's discuss significant figures a
Page 184 and 185: On your calculator you would input
Page 186 and 187: Ag+ + Cu ---> Ag + Cu2+ I have deli
Page 188 and 189: 7. Half Reactions A half-reaction i
Page 190: Notice that each separate substance
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