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The Learning Goal for this assignment is: The students will learn how the interaction between water molecules account for the unique properties of water and how aqueous solutions form Page 124 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 Many unique and important properties of water – including its high surface tension, low vapor pressure, and high boiling point – result from hydrogen bonding Surface Tension - The inward force or pull that tends to minimize the surface area of a liquid. Surfactant – Any substance that interferes with the hydrogen bonding between water molecules and thereby reduces surface tension Water is a simple molecule requiring three atoms; the oxygen atom forms a covalent bond with each of the hydrogen atoms. In a water molecule, the bond polarities are equal, but the two poles do not cancel each other because a water molecule is bent. The molecules as a whole is polar; the negative end attracts the positive end. Hydrogen bonding also occurs – the oxygen atom has a partial negative charge. The surface of water acts like a skin – the ability of water molecules to form hydrogen bonds with other molecules that surround them on all sides. Water forms nearly spherical drops on a leaf. Water molecules at the surface of the water drop cannot for hydrogen bonds with molecules in the air, so they are drawn into the body of the liquid. Water drops bead up on some surfaces, is added to water, the drop spreads out. So basically a surfactant causes the beads of water to collapse and spread out. An extensive network of hydrogen bonds holds the molecules in liquid water to one another. These hydrogen bonds must be broken before water changes states so the tendency of these molecules to escape is low and evaporation is slow. Molecular compounds of low molar mass are usually gases or liquids with low boiling points at normal atmospheric pressure. Water in the Solid State The structure of ice is a regular open framework of water molecules in a hexagonal arrangement As a typical liquid cools, it begins to contract and its density increases gradually; it increases because the molecules of the liquid move closer together so that a given volume of the liquid contains more molecules and thus more mass. A typical solid sinks in its own liquid because the density of the solid is greater than that of the corresponding liquid. As water begins to cool, it behaves initially like a typical liquid, it contracts slightly and its density gradually increases. Below 4 ° C, water no longer behaves like a liquid and at 0° it forms as ice. The unique properties of ice are a result of hydrogen bonding. Extensive hydrogen bonding in ice holds the water molecules farther apart in a more ordered arrangement than in liquid water. The hexagonal symmetry of a snowflakes reflects the structure of the ice crystal. A layer of ice acts like an insulator acts. 15.2 Homogeneous Aqueous Systems Solutions Substances that dissolve most readily in water include ionic compounds and polar covalent compounds. Aqueous solution: water that contains dissolved substances Solvent: In a solution, the dissolving medium Solute: The dissolved particles in a solution. Salvation: The process by which the positive and negative ions of an ionic solid become surrounded by solvent molecules Water dissolves so many of the substances that in comes in contact with making it an aqueous solution. A solvent dissolves the solute, and the solute becomes dispersed in the solvent. They can be any state of matter. Solutions are homogeneous mixtures and stable mixtures. Nonpolar covalent compounds, such as
methane and compounds found in oil, grease and gasoline don’t dissolve in water but in gasoline. When an ionic solid dissolves, the ions become solvated or surrounded by solvent molecules. Water molecules are in continuous motion because they have kinetic energy. Some ionic compounds, the attractions among the ions in the crystals are stronger than the attractions exerted by water. These compounds cannot be solvated to any significant extent and are therefore nearly insoluble. Oil and gasoline do not mix with water because they are composed of nonpolar molecules. The attractive forces that hold two molecules in oil together are similar in magnitude to the forces that hold two molecules in gasoline together. Molecules in oil can easily separate and replace molecules in gasoline to form a solution. Polar solvents dissolve ionic compounds and nonpolar compounds - like dissolves like. Electrolytes and Nonelectrolytes All ionic compounds are electrolytes because they dissociate into ions. Electrolyte: A compound that conducts an electric current when it is in an aqueous solution or in the molten state. Nonelectrolyte: A compound that conduct an electric current in either an aqueous solution or the molten state. Strong electrolyte: . Weak electrolyte: Conducts an electric current poorly because only a fraction of the solute in the solution exists as ions. Conduction of an electric current requires ions that are mobile and thus able to carry changes through a liquid. The solution conducts an electric current if it contains ions. Some polar molecular compounds are nonelectrolytes in the pure state but become electrolytes when they dissolve in water. This change occurs because such compounds ionize in solutions. Not all electrolytes conduct an electric current to the same degree. In a solution that contains a strong electrolyte all or nearly all of the solute exists as ions. The ions move in solution and conduct an electric current. Inorganic bases and acids are strong electrolytes. Organic acid and bases are weak electrolytes. Electrolytes are essential to metabolic processes as it carries electrical impulses internally and to other cells. However, an electrolyte imbalance can occur if you become dehydrated. Hydrates The forces holding the water molecules in hydrates are not very strong, so the water is easily lost and regained. Water of hydration: Water contained in a crystal. Hydrate: A compound that contains water of hydration. Effloresce: . Anhydrous: A substance that does not contain water. Hygroscopic: Hydrates or other compounds that remove moisture from air. Desiccant: Substance sued to absorb moisture from air and create dry atmosphere. Deliquescent: They remove sufficient water from the air to dissolve completely and form solutions. Water can be driven from a hydrate from heating it. Water molecules are an integral part of the crystal structures. In writing the formula of a hydrate, use a dot to connect the formula of the compound and the number of water molecules per formula unit. The water molecules in hydrates are held by weak forces so hydrates often have vapor pressure. As the crystals lose water of hydration, they effloresce and become coated with a white powder of anhydrous sodium carbonate. Hydrated ionic compounds that have a low vapor pressure remove water from moist air to form higher hydrates. A desiccator may contain calcium chloride. Substance that must be kept dry are stored inside. 15.3 Heterogeneous Aqueous Systems Suspensions A suspension differs from a solution because the particles of a suspension are much larger and do not stay suspended indefinitely. Suspension: A mixture from which particles settle out upon standing Suspension are heterogeneous because at least two substances can be identified. Colloids Colloids have particles smaller than those in suspensions and larger than those in solutions. Colloids: A heterogeneous mixture containing particles that range in size from 1 n to 1000 nm. Typical effect: the scattering of visible light by colloidal particles. Brownian motion: Chaotic movement of colloidal particles. Emulsion: A colloidal dispersion of a liquid in a liquid. Particles are spread or dispersed. They’re cloudy so they can be distinguished by Tyndall effect and by the observation of Brownian motion. They are also subject to coagulation or clumping together and they can be emulsified or made stable. Coagulation are when they absorb ions from the from the dispersing medium onto the surface. Page 125
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Honors Chemistry Class Policies and
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Unit 1 (22 days) Chapter 1 Introduc
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Lorenzo Walker Technical High Schoo
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MUSTANG LABORATORIES COMMITMENT TO
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Chapter 1 Unit 1 Introduction to Ch
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K H D B D C M KING HENRY DIED DRINK
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2. One cereal bar has a mass of 37
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1. How many meters are in one kilom
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The Learning Goal for this assignme
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RULE #3: To add/subtract in scienti
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Rule 3: A final zero or trailing ze
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For addition and subtraction, look
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Dimensional Analysis This is a way
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Chapter 4 Unit 2 Atomic Structure T
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Looking at Ions We haven’t talked
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Neutron Madness We have already lea
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In the space below, write the unabb
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Create groups for these Scientist a
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The Learning Goal for this Assignme
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Atomic Size Define Atomic Size: The
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Define Electronegativity: Electrone
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Unit 3 Chapter 25 Nuclear Chemistry
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Name ____________________ Juan Roqu
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Learning Goal for this section: The
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Beta Particle Decay Beta decay is a
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Ion Charge? What is the charge on f
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C 2 H 6 O Ethanol CH 3 CH 2 O Step
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Linear Molecular Geometry Orbital E
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Trigonal planar Molecular Geometry
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Trigonal Pyramidal Molecular Geomet
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Page 78 and 79: Orbitals Equation Lone Pairs Angle
Page 80 and 81: Chapter 9 Unit 4 Chemical Names and
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Page 88 and 89: Categories of Reactions All chemica
Page 90 and 91: List what type the following reacti
Page 92 and 93: How to Balance Chemical Equations A
Page 94 and 95: Step 5 Balance the hydrogen atoms n
Page 96 and 97: 6) ___ 1 Mn(NO2)2 + ___ 1 BeCl2 __
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Page 100 and 101: Stoichiometry and Balanced Equation
Page 102 and 103: Step 1: 200g C3H8 is equal to 4.54
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Page 106 and 107: %yield = 6.1 tons × 100 = 64% 9.6t
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Page 116 and 117: temperature average kinetic energy
Page 118 and 119: keep the pressure constant heat up
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Page 122 and 123: kelvin equals everything stops K= t
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Page 130 and 131: Part 5: Molarity Molarity (M) is th
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Page 136 and 137: Step Two: solid ice melts Now, we c
Page 138 and 139: Step Four: liquid water boils Now,
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Page 142 and 143: The Learning Goal for this section
Page 144 and 145: moving from one side to another, an
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Page 148 and 149: Unit 8 Chapter 19 Acid and Bases Th
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Page 154 and 155: HCl + H2O ⇌ H3O + + Cl¯ HCl - th
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Page 168 and 169: 150. 140. Table G Solubility Curves
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0 6.941 +1 Li 3 2-1 Na 39.0983 K +1
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First Atomic Symbol Name Ionization
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Collier County CHEMISTRY EXAM FORMU
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CHEMISTRY EXAM FORMULA AND RESOURCE
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