Chemistry Ch. 4-6 Review 2 PDF

AEff.cat Properties change in form state of matter when change occurs or dissolving attractive forcesbetween compound remains the same the molecules are broken chemical bonding is preserved or weakened...

AEff.cat Properties change in form state of matter when change occurs or dissolving attractive forcesbetween compound remains the same the molecules are broken chemical bonding is preserved or weakened Reaction Banda forbearer a ffes Atoms of starting materials acid base Ép ties reactants combine in a new way to form products o_0 Changes in State Solid and liquid states have closely packed atoms or molecules Remain close together due to attractive forces In gas phase particles have enough energy to Become spaced overcome attractive forces and apart can escape from opencontainer Attisfftot.cm oppositepartial type of charge interaction chargesattract Polar compounds partial charges on atoms  When attractive forces bring molecules together Energy heat is released To break those forces and separate the molecules Energy is required HEAT Physical and Chemical changes REQUIRE ENERG Endothermic absorb heat in order for a change to occur Exothermic release heat when change occurs The amount of energy released or absorbed by a physical orchemical change is Δ H Chaffin A negative value of 0H signifies a loss or release of heat Exothermic A positive value of 0H signifies a gain or absorption of heat Endothermic Energy beat will affect melting forces or boiling stranger require more point of a substance energy 4 Types of Attractive Forces 1 Ionic charge attraction 2 Hydrogen Bonding 3 Dipole dipole forces Covalent 4 Dispersion forces Compounds Increasing strength 1 Ionic Charge Attraction Ionic Compound Caused by cations and anions with opposite charge Require large amount of energy to break causing HIGH MELTING POINTS 2 Covalent Compounds fed p ins Dispersion Weaker Attractive Forces require less energy to break LOW MELTING POINT Dispersion Forces Weak Attractions between covalentmolecules causes temporary dipole when electrons a are not distributed equally Cottolphinks elements Dipole dipole forces Caused by opposite partial Charges Polarmolecule Dipole dipole attractions Hydrogen Bonding Covalent compounds with G H N H or F H bonds hydrogen bonding can occur Interaction between the partially positive hydrogen atom and a lone pair of electrons on N O or F atoms  To determine BEST FORCES POSSIBLE Use molar mass of the substance to get an idea Periodic Table of its size Atomic Mass Dispersion Force TIE Force gets stronger Size Shape Mass when mass is larger Dissolving Substances Physical Change Collision Dissociation Solvation Reactingparticles Atoms or molecules Salvant molecules must collide of solute separate surround the with one Attractive forces are dissociated solve another beingbroken by ONLY if there collision with is an attraction solvent between them Ionic compounds Charge attraction will dissociate between ions info cations and Ifsaluation anions does not occur Covalent compounds separated salute can rejoin preventin will dissociate into it from dissolving  discrete molecules Collision Chemical Equation KC s k aq Cl Cag If an ionic compound has a or charge consider it soluble in water instead's bisationser General Rule Solubity of Covalent Compounds Like Dissolves Like Polar substances dissolve in polar solvants Non polar substances dissolve in non pdar solvants Carbon Ratio Rule 11,2 1 3 1 Very soluble in Water Polar 4 1 and 5 1 Slightly Soluble Slightly Polar 61 Insoluble NON Polar Summary of Solubility _in order to at iieYk Ih Te For covalent compounds like dissolves like rule use referring to overall polarity Lewis structure must be examined to figure out whether a covalentcompound ispolar or non polar Water is POLAR so only POLAR compounds will dissolve well in water  Concentration ratio of the amount of solute dissolved in a given amount of solution The amount of solute or solvent can be measured by mass weight volume space occupied or moles Percent Concentration as Ratios Concentrations dissolved in water are expressed as percent ratio by mass or volume mlm to m v4 or vluto Gtg mL mLImL Concentration Ratios as Conversion Factors Ex 355mL of AriFse 0.050g Nat 0.18g Nat 100mL solution Molarity 1 mole is a unit equal to 6.022 1023 Mdarityn defined as the number of moles of solute dissolved per 1 litter L of solution Molarity moles of solute or M Moles L solution L 1L 1000mL To find Molar Mass add the atomic mass of the atoms If both volume and mass is presentfor a solvent multiply together to find the actual mass Chapter 5 Chemical Change breaking and forming of chemical O H mustbreak bonds to recombine atoms and HH 0 0 mustform produce different substances Physical Change change state of matter breaking and forming intermolecular forces Chemical Reactions Can be Exothermic and Endothermic More energy is moreenergy is released absorbed tobreakbands when new bonds are formed Balanced reactions obey by the Law of Conversion of Mass the reactants and the products have the same number of elements If the reaction is UNBALANCED we add coefficien number front of the formulas Subscript and the in formula CANNOT BE CHANGED Combustion Reactions substance is burned in the presence of oxygen gas to Complete Combustion etra oxygen CO2 and H2O IncompleteCombustion limitedoxygencreatesCO and H2O Balanced Combustion Reactions Cotte 802 95002 6H20 5 5 C 105 12 12 11 2012 16 20 3916 Factors Affecting Rates of Reaction 1 Concentration of Reactants How easy is it for the reactants to find each other 2 Temperature Molecules atoms move faster at higher temperatures Fast moving particles collide more frequently More kinetic Used to meet activationenergy energy 3 Catalyst Increase the rate of reaction by lowering the activation energy a Nature of Reactants Includes Physical or chemical properties such as state of matter or the internal bonding of the Bigblack slow reaction atoms in the reactant small pieces fasterreaction Energy Diagram depicts a chemical reactions progress graphically Activated Complex the unstable of atoms in group transition from reactants to products High Activation Energy Slow Reaction Energy Fast Reaction Low Activation Exothermic Reaction Produce Heat Endothermic Reaction Absorb Heat Addition Reactions original molecule adds new atoms to it small molecules such as H2o Ck Reactions happen with Alkenes Alkynes Aldehydes Double or triple bonds actants and Ketones that dropto singlebonds Ex CHz CH CH Brz Cl12 CH CHS Br Br Sometimes a Catalyst is needed to make the reaction go faster Written over the arrow O 19 to CH 3 Chz C CHz Hz 0113 CHz CH a Hydrogenation adding two atoms of hydrogen th across the double bond or tripple band Requires a catalyst  112 catalmy Ha Halogenation requires adding X2 such as Cla Does not require a Catalyst Br Bre Hydrohlogenation addin Hx two different atoms across the double bond or tripple band Br HBr Hydration adding water H2o across the double bond Requires a catalyst Water 11 0H OH H2O Hegu Condensation Reactions formation of water O 2types of reactions amidation ester Amide and esterification H2O on said 0 OH Monomer smaller molecular unit buildingblockinsidethe polymer  Esterification esterfunctional groups will be created Reacting a carboxylic acid with an alcohol reactant R C OH R OH R C OR H2O Carboxylic Alcohol wateris e acid always formed Functional Groups of Condensation Acid Amine As Reactants Carboxylic Alcohol and reactant p p R C OH R N H R C N R 1120 Carboxylic Amine Amide Acid R R C N R Amide CarbonylCarbon Nitrogen Hydrolysis Reaction Hydrolysis a reaction that splits a reactant into smaller molecules 2 using water Functional Groups Esters and Amides As Reactants 0 19 11 R C OR H2o R C OH R OH Carboxylic Alcohol Ester acid Ester Hydrolysis  a 0H H2O S an Amide Hydrolysis Product contains an Amine and Carl R C NH R H2o R E on NHz R Oxidation and Reduction Transfer of electrons G Ñ Oxidation the loss or partial loss of electrons cEgaÑ Reduction the gain or partial gain of electrons Both have to happen together Ionic Compounds identify charges of bare electrons look for changes in the charge 2N a Clz 2Nall Na oxidized lost an electron fl Y Y Y Cl reduced gained an electron t 2 KE Callz Catz 2KCI No change 1 121 4 in charges Covalent compounds all nonmetals CANNOT USE charges to figure out REDOX Look at Structure and Banding  Oxidation Carbon increases bands to oxygen decreases bonds to hydrogen Reduction carbon decreases bands to oxygen increases bonds to hydrgen 9 H d 11 n c on n c n H C OH I H blinds y bonds toll 3 toll 2bandston 1 o bands too 1 bandtoo 2 band too 3 2 110 Larger Mdecules If more carbon atoms present only pay attention to ones that change on O H is oxidized gains aband H2 to oxygen Chapter 6 Arrhenius acids produce H or 1130 ions in water Ex H Icg 1120 1 1130 ag Cl Cag Arrhenius Bases produce OH ions in water Ex NH3 1120 a Nhut OH Bronsted Lowry Theory Acids Acids donate a proton H Ex HCl 1120 i 7H30 ag Cl Cag g Donor acidAcceptor Base HCI is the acid H2O is the base that donates H that accepts H Bronsted Lowry Theory Bases Bases accept a proton Ht Ex NHz 1120 Nhut OH acceptorHt Proton donor Ht Proton Base Acid Inorganic Acids will start with H Strong Acid Ex HCI and HNO3 Organic Acids starts with or ends with COOH Weak Acid Ex CH COOH and HzCOz Inorganic Acids with H and a nonmetal are named with the prefix hydro and end with ic acid HCI hydrochloric acid HI hydroiodic acid Inorganic acids with H and polyatomic ion are named with the ending ic acid or ous acid no prefix HCI03 chloric acid HC 02 chlorous acid Ionic Compounds composed of metal cations with  StrongBases hydroxide anions are often bases can dissociate to create 011 Bases with OH ions are named using normal rules for ionic compounds Ex NaOH Sodium hydroxide Organic Compounds with a nitrogen atoms bearing an accessible lane pain such as NHS and CN3N 12 are bases The functional group in an organic mine compound is a base weak Base Hydrocarbons DO NOT PARTICIPATE in Acid Base Reactions They DO NOT ACCEPT DONATE PROTONS Strong Acids completely ionize 100 and completely donate their proton in aqueous solutions Use a single arrow in the chemical reaction Weak Acids dissociate only slightly in water to form a solution of mostly Molecules Weak Acid reacts with Weak Base Use Arrow Strong Acids Form MAXIMUM AMOUNTS of 430 ions Strong Acids Include HCI HBr HI HNOs HzSOy HCIOs HClOn Weak Acids Partially Donate Proton Will React with Water Dissociation consent Ka can be used to rank how strong that acid is The larger the Ka the stronger the 1 10 Acid 10 10 Strong Bases Will accept proton 00 of the time Produce OH_in water 100 of the time Weak Bases Accept proton less than Coo of the time Produce OH in water less than Goato of the time Weak Bases have Kb values that rank their strength Higher Kb value means stronger base Ionic Compounds composed of metal cations with hydroxide anions A are Strong Bases  Some bases completely dissociate to produce more OH Weak Bases include most covalent compounds that have nitrogen bearing a lone pair Ammonia NH3 and Amines CHINA H V H N H H C N H H H H Amphiprotic can act as both basic and acidic Weak Acid and Weak Base Water is Amphiprotic Fittings pH 7 H2O H2O c 11301 OH 11301 OH 3 1.0 10 M Ka formula Neutral solution 430 OH Acids produce more Hot solution will have H3Ot OH_ Bases produce more OH solution will have OH 430T The higher the Hot the pH log Hzot lower the pH value 1 2 34567891011 121314 Acidic Neutral Basic Predicting Acid Base pH Level w o Calculation  Identify if the solution contains strong weak acid or base Which is more Concentrated X O.AM Ka values if molarity is not present 10 10 PH Value Equations PH log Hot POH log OH pH pom 14 Hot 10 PH OH 10 POH Kw HOT OH Conjugate Acid die more H Conjugate Base one less H Ex HCI conjugate acid CI conjugatebase The stronger the acid the weaker its conjugate base Reactions with weak covalent bases a proton H transfer occurs Acid Reactant will lose Ht Base Reactant will gain Ht 0 Ex 0 NHS C NHS on o weak Acid Weak Base Proton Donor Proton Acceptor Equilibrium two opposite processes are occurring at the same time For Acid Base Reaction  If both the reactants are weak acid base the reactant will be equilibrium 3 Two way Arrow c Ex NHS H2O c NHI OH If one strong acid base reactant is a and the second reactant is a weak acid base it will NOT have equilibrium way Arrow One Ex HCI 1120 CI 1130 Ex Strong bases include Metal Hydroxide NaOH which are ionic compounds To predict products combine metal cation with the anion from the acid to achieve when Acid reacts with ionic compounds charge balance double replacement reaction occurs Ex 112503 2K OH 42503 2H20 H 503 kt OH Ht Predicting Products of Acid Base Reaction Determine if the reacting base is covalent or ionic Reactions with strong ionic bases the reaction will be a double replacement reaction the products  are neutral ionic compound salt and water Reactions with weak covalent bases a proton H transfer happens forming conjugate partners of the reactants Carboxylic acids and amines can do condensation reaction called Amidation that requires enzyme catalyst Enamel Hydroxyapatite Caio Paulo 0H12 OH ions can act as a base and react with acids To protect teeth fluoride is used to replace OH with F that protects tooth from acids Acid BaseProperties of Drugs The amine form of the drug is called freebase The form that reacts with it is called the hydrochloride salt NHt C1 N O O HCI Hydrochloride Free Base Salt  Buffer Have the ability to resist changes in pH Contain weak acid conjugate base dissolved in water 0.01M Blood is a BUFFER The weak acid component HA reacts with any base that is being added Ex HCzHz0z NaOH NaCzH30z 1120 he on reacted basseya The conjugate base component A reacts with any acid that is added Ex Nacz 1302 HCI 4624302 NaCl 24302 HCI acid reacted A theaway Buffer pH is controlled by how strong the weak acid HA is Stronger weak acids lead to more strength determined acid low pH values by Ka values pH value for buffer pKa logka weak Acid if the molarity is the same if the molarity is different Approximate