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Chemistry Notes

by: Ali Miller

Chemistry Notes Chemistry 151

Ali Miller
GPA 3.43
Chemistry 151
Jeffery Pyun

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About this Document

Here are notes for Unit one Module 1 and 2 of Chemistry 151. This includes the important part of the modules and important comments my Professor has said.
Chemistry 151
Jeffery Pyun
Class Notes
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This 6 page Class Notes was uploaded by Ali Miller on Friday January 30, 2015. The Class Notes belongs to Chemistry 151 at University of Arizona taught by Jeffery Pyun in Spring2015. Since its upload, it has received 176 views. For similar materials see Chemistry 151 in Chemistry at University of Arizona.


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Date Created: 01/30/15
12215 Chem 151 Distilation take a substance that is a mix of different liquids and try to separate them REMEMBER each substance has its own boiling point like a nger print Boiling off each substance separately by its separate boiling point QUESTION think about other properties besides the boiling point to separate things Unit 1 Module 2 Modeling Matter How do we distinguish substances The central goal of this unit is to help you understand and apply the basic ideas that can be used to distinguish the different substances present in a system Why do water for clouds on earth in the atmosphere but not nitrogen or carbon dioxide Our earth favors water Particulate model of matter One of the most powerful models we have to explain snd predict the physical properties and behavior of substances is the particulate model of matter Basic assumptions 1 Any microscopic sample of a substance is composed of a large number of very small particles 1 mL of water 3444444444444444444444444 particles 334 x 10quot22 How Small Most substances are made of particles of quotnanometerquot size Dvnamic Nature Basic Assumptions LParticles are constantly moving in random directions through empty space Pressure P is determined by the force of particle collisions on the walls Pressure ForceArea Temperature is a measure of kinetic energy KE 12 mvquot2 per particle What determines the speed of particles Temperature Speed distribution T KE avg 12 mv avgquot2 Interactions Basic Assumptions 3 Particles interact with each other The strength of the interactions depend on the distance between particles 12715 Chem Unit 1 M2 notes Today Finishing module 2 Starting module 3 Last week We focus on gasses because they are the most random and most abundant Easiest phase of matter to understand Simplest stare to picture Trying to gure out properties and why thing happen example Pyun coke bottle Pressure the more particles move the more pressure builds up We looked at purely elastic collisions Energy coming in vs energy out Todays class Ideal gases what we will focus on Volume Temperature and number of particles affect pressure we need to explain why different substances have different properties Boiling points KNOW 02 183 AND N2 195 Composition in matter Potential energy con gurations Both sides of the quotwellquot give us increase potential energy If you keep pushing the 2 things together it builds resistence The energy at a phase transition stays constant Types of matter Describing what the quotballsquot are Ideal gas law The particulate model of matter a relationship of the following type for gases at high T and Low P P kB NTV The ideal gas law does not allow us to account for phase transitions How is a liquid different from a gas We must have intermolecular interactions because that is the only way particles can stay together Kinetic vs potential enerdv Why does energy platue As attractions get farther apart they no longer feel the range of attraction If you force the chemicals apart they don39t feel the attractions between them Solid has lower potential energy and fewer con gurations Gas has the most con gurations high potential energy Need high energy and high pressure to turn graphite into diamonds What makes intermocular forces different lts composition what it is made of Molecules are ensembles of atoms a bunch of them connected together 12915 Chem Unit 1 EXAM ONE IS FRIDAY modules 14 Last time Collisions with the gas on the wall Idealgas 0 Lower volume 0 Lower pressure 0 Increase inter molecular forces Needed to de ne quotthe ballsquot 0 Types of matter Elemental substances 0 C gt diamonds graphite bonding 0 Atom gt C Covalent compunds 0 C02 Molecules Salts o lons Module 3 Masses of substances gt composition structure correlatecompare Periodic Table Atomic mass units gt AMU o Mole the quotcurrencyquot of chemistry 6022 x 10 quot23 Avogadro s number Mass gt moles gt of molecules P KBNT PVnRT Chemical compunds Most substances in nature ar chemical compunds 0 They are composed of identical particles of bonded atoms of 2 or more different types Molecular compounds 0 Made of molecules H20 C02 Models and formulas 0 Space lling 0 Ball and stick 0 Molecular formula 0 Structural formula Ionic compounds Comparing Masses Characterize the differences in particles mass and number Indirect measurements 0 Atoms and molecules have masses and sizes so small that cannot be measured directly P KB NTV Avooadro39s law Equal volumes of different gasses at the same temp and pressure should contain the same amount of particles Relative atomic mass The average relative atomic mass of all atoms is listed in the periodic table 0 The largest number on the PT 0 Atomic mass is equal to the mass of a substance if you have one mole molar mass gmole mass of 1 atom over 1 mole What is a mole 0 Related Avogadro s 6022 x 10 23 of molecules


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