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It looks like your browser needs updating. For the best experience on Quizlet, please update your browser. Learn More. If they don't, multiply them both by a number that will get them to come out nice. It looks like your browser needs updating. For the best experience on Quizlet, please update your browser. Learn More. This produces a chemical change. Converting word equations to chemical equations Ex. Balancing chemical equations a. Counting atoms of each element in a chemical equation i. Within a formula, the subscript numbers refer to how many atoms of a particular element are found in a formula. Ex. H?O refers to two atoms of hydrogen bonded to one atom of oxygen. b. The coefficient is a number that occurs before a chemical formula, and refers to how many molecules or formula units are presented. Ex. 2H?O refers to two molecules of water. ii. The coefficient refers to the entire formula, and multiplies all atoms in the formula. To balance chemical equations a. Locate an element that is out of balance.Stoichiometry: mole and mole conversions 1. If you measure out a number of grams equal to the atomic mass of an element, you will always get the same number of atoms. This number is called a mole. 2. As it happens, a mole of atoms equals 6.02 x 1o?? atoms, a number you don't need to memorize. 3. If you add up the atomic weights of all the atoms in a compound, you can get the formula weight of a compound. 4. You can measure out a mole of a compound (6.02 x 10?? molecules or formula units) by measuring out the formula weight in grams. 5. You can convert between the mass of a substance and the number of mole by using a conversion factor. 6. You can use this concept to figure out how much of a product you expect to get from a chemical reaction if you know how much reactant you have. Mole Is a unit for counting atoms. Synthesis There are more reactants than products. It can be measure as the rate at which reactants disappear or a rate at which products accumulate.
It's effectively the same thing, and the choice often depends on which is easiest to measure. 1. The Collision Theory of chemical reactions says that a reaction can only take place if two reactants particles collide in the right way. a. Collisions must be alligned correctly. b. Collisions must be sufficiently energetic to break chemical bonds. 2. Reactions occur most rapidly in the gas phase, as molecules move quickly and collide frequently. Next, reactions occur most rapidly in the liquid phase. Usually solids don't react with other solids, although they can react with a surrounding liquid or gas. Temperature (tends to increase the rate of a chemical reaction) Measures the average kinetic energy of colecular motions. Higher temperatures mean that molecules are moving faster. i. Collisions are more frequent at higher temperatures. ii. Collisions are also more energetic at higher temperatures. iii. Both of these factors cause reactions to happen faster at higher temperatures. Concentration The more concentrated reactions are (that is, the more molecules per unit volume), the more frequent collisions will be. As a result, reactions take place more rapidly in concentrated solutions that in dilute solutions. Activation Energy The energy required to break chemical bonds, starting a chemical reaction. i. Often, activation energy comes in the form of heat-- such as lighting fire. This gets the molecules colliding hard enough to break bonds. ii. Sometimes activation energy can come in the form of light. iii. Activation energy is a necessary first step in starting a chemical reaction. It is a sort of energy barrier that must be overcome before a reaction can start. Energy is not a catalyst. Bond Energy a. The energy required to break a chemical bond. i. It takes energy to break chemical bonds. Each type of chemical bond has its own bond energy. ii. The same amount of energy is released if the same kind of bond is formed. Exothermic Energy A reaction gives off energy.
If energy is released in forming the products is greater than the energy required to break apart the reactants. Endothermic Energy A reaction absorbs energy. If the energy it takes to break apart the reactant atoms is greater than the energy released in forming the products. To determine if a reaction is exothermic or endothermic i. Determine how many bonds of each type are present in the reactants. ii. Add up the total bond energy required to break apart the reactants. iii. Do the same with the products, determining how much energy will be released when the products form. iv. If the energy released in forming the products is greater than the energy required to break apart the reactants, the reaction is exothermic. v. If the energy required to break apart the reactants is greater than the energy released by the formation of products, then the reaction is endothermic. Solution Smallest particles (homogeneous). Light passes through without reflection. Colloid Larger particles but stay suspended. Identified by Tyndall Effect. Light creates a line. Suspension Large particles are subject to gravity and will fall out of solution. Light is scattered over broad area. Like dissolves like i. Polar solutes will dissolve or are miscible in polar solvents like water. ii. Nonpolar solutes will dissolve or are miscible in nonpolar solvents like oil. iii. If they do not dissolve, they are immiscible. Solubility i. A serial dilution dilutes a solution by a factor of 10 each time, illustrating ppm and ppb. Colligative Properties Those properties of a solution that are different than those of the solvent. They depend only upon solute number, not identity. Freezing Point goes down in a solution. Boiling Point goes up in a solution. Vapor Pressure goes down in a solution Osmotic Pressure water will move in the direction of more solutes.They don't fully go to completion. All reversible reactions are exothermic one way and exothermic the other way.
Increase temperature favors endothermic reaction. Pressure decreases the side with more moles of gas is favored. Buffers Buffers maintain pH - 7.4 (blood) 10, 4 - Take advantage and they work because of LeChatelier's Principles. Despite adding, acids or bases, buffers keep the pH where it is. They are made of either a weak acid and salt of its conjugate base or a weak base and salt of its conjugate acid - Buffers require a reversible reaction and since strong acids and bases ionize completely, there is no reverse reaction.Smog is common in large urban areas, especially during hot, sunny weather, where it appears as a brownish haze that can irritate the eyes and lungs. Ozone, a toxic gas that is not normally produced at lower atmospheric levels, is one of the primary pollutants created in this kind of smog. Greenhouse gases Gases such as carbon dioxide, methane, nitrous oxide, water vapor, and ozone in the atmosphere which are involved in the greenhouse effect. Our library is the biggest of these that have literally hundreds of thousands of different products represented. I get my most wanted eBook Many thanks If there is a survey it only takes 5 minutes, try any survey which works for you. Our library is the biggest of these that have literally hundreds of thousands of different products represented. I get my most wanted eBook Many thanks If there is a survey it only takes 5 minutes, try any survey which works for you. Our library is the biggest of these that have literally hundreds of thousands of different products represented. I get my most wanted eBook Many thanks If there is a survey it only takes 5 minutes, try any survey which works for you. Our library is the biggest of these that have literally hundreds of thousands of different products represented. I get my most wanted eBook Many thanks If there is a survey it only takes 5 minutes, try any survey which works for you.
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And by having access to our ebooks online or by storing it on your computer, you have convenient answers with Spring Semester Final Study Guide Honors Chem. To get started finding Spring Semester Final Study Guide Honors Chem, you are right to find our website which has a comprehensive collection of manuals listed. Our library is the biggest of these that have literally hundreds of thousands of different products represented. I get my most wanted eBook Many thanks If there is a survey it only takes 5 minutes, try any survey which works for you. And by having access to our ebooks online or by storing it on your computer, you have convenient answers with Chemistry 1 Final Exam Study Guide Spring 2013. To get started finding Chemistry 1 Final Exam Study Guide Spring 2013, you are right to find our website which has a comprehensive collection of manuals listed. Our library is the biggest of these that have literally hundreds of thousands of different products represented. I get my most wanted eBook Many thanks If there is a survey it only takes 5 minutes, try any survey which works for you. Multiple Covalent Bonds between 2 atomsCannot have a covalent bond with ions, just atoms Drawing Lewis StructuresEach line represents 2 electrons.Geometries of moleculesAn electron chargePhase is (s). Same number as molecular mass Spontaneous Occuring without external influence. Non-spontaneous Must have a continuous external influence inEntropy (s) The measure of chaos (disorder) in a systemALL moleculesDipole-dipole Typically stronger than LD forces. ONLY occurHydrogen bonding The strongest intermolecular force. ONLY occursNO energy is lost during collisions, so KE particles remainCrystalline Solids Activation energy (Ea or Eact) The energy required for a reaction to occur. Rate of Reaction The measure of how quickly a reaction occurs.
Temperature An increase in temperature increases frequencyConcentration An increase in concentration increases theCatalysis Adding a catalyst lowers activation energy,Phase change Matter changing from one phase to another. Melting Phase change from liquid to solid. Freezing Phase change from liquid to solid Neutralizations Reactions with hydroxides. Co2 (g) producing reactions Reactions with hydrogen carbonates orAmmonium salt producing reactions Reactions with nitrogen-containing compounds. Acidity and Basicity of Salt Solutions Weak Strong Basic. Strong Strong Neutral. Weak Weak More information needed One concentration is known, the other isYou need a Premium account to see the full document. Option 1 Share your documents to get free Premium access Upload Option 2 Upgrade to Premium to read the full document Get a free 30 day trial Already have an account. Sign in here Help. And by having access to our ebooks online or by storing it on your computer, you have convenient answers with Chemistry Spring Semester Final Exam Review Sheet. To get started finding Chemistry Spring Semester Final Exam Review Sheet, you are right to find our website which has a comprehensive collection of manuals listed. Our library is the biggest of these that have literally hundreds of thousands of different products represented. I get my most wanted eBook Many thanks If there is a survey it only takes 5 minutes, try any survey which works for you. Our library is the biggest of these that have literally hundreds of thousands of different products represented. I get my most wanted eBook Many thanks If there is a survey it only takes 5 minutes, try any survey which works for you. And by having access to our ebooks online or by storing it on your computer, you have convenient answers with Chemistry Final Exam Study Guide Spring 2012. To get started finding Chemistry Final Exam Study Guide Spring 2012, you are right to find our website which has a comprehensive collection of manuals listed.
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