ࡱ> vxu'` wXbjbjLULU \.?.?]"D T=T=T=T=4= W>>>>>>>>NNNN_"OSW$Xh[t6WQ@>>@@6W>>WaNaNaN@>>NaN@NaNaNaN> > t<T=_Aj aNNW0WaN[M[aN[aNL>h[?JaN?<?>>>6W6WWN >>>W@@@@   18d   8    Honors Chemistry Final Exam Chapter Summaries FIRST SEMESTER Chapter 1: Chemical Foundations SI units: meters, liters, grams metric prefixes: kilo, centi, milli, micro precision & accuracy percent accuracy error (formula) random and systematic error significant figures: counting & in calculations exponential notation dimensional analysis (conversion factors) density classification of matter: pure substances, mixtures, solutions, elements, compounds physical & chemical changes physical & chemical properties Chapter 2: Atoms, Molecules and Ions atomic theory Rutherfords experiment structure of atom nucleus protons, electrons, neutrons atomic number, mass number isotopes nuclear symbol molecules & ions periods & groups regions of the Periodic Table: main groups, transition metals, inner transition metals noble gases, halogens, alkali metals, alkaline earth metals metals, nonmetals, metalloids ionic & covalent compounds names of ionic compounds names of binary covalent compounds names of acids formulas of compounds from name Chapter 3: Stoichiometry atomic mass molar mass (molecular mass) moles Avogadro's number conversions: # particles ( moles ( mass percent composition (mass percent) empirical formula percent composition ( formula finding molecular formula from simplest formula and molar mass formula from experimental data percent composition conversions writing and balancing chemical equations reactants, products, coefficients types of chemical reactions composition, decomposition, single replacement, double replacement mass/mole conversions in chemical reactions (stoichiometry) limiting reactant, excess reactant theoretical yield, experimental yield percent yield Chapter 4: Chemical Reactions in Water Solutions electrolytes & nonelectrolytes strong vs. weak electrolytes ionization equations molarity calculations involving molarity finding the molarity of a solution using molarity as a conversion factor solution preparation dilution: V1 x M1 = V2 x M2 precipitation reactions reading a solubility table molecular equations net ionic equations stoichiometry of precipitation reactions common strong & weak acids & bases Chapter 7: Atomic Structure & Periodicity wavelength (l), frequency (() l( = c atomic spectra Bohr model of the hydrogen atom ground state, excited states quantum theory electron clouds orbitals principle energy levels (n) sublevels (s, p, d, f): electron capacity and relative energies possible values for 4 quantum numbers (n, l, ml, ms) ground state electron configuration of atoms abbreviated electron configurations outer electron configuration valence electrons orbital diagrams atomic radius ionization energy electron configuration & the Periodic Table reactivity of elements & the Periodic Table Chapter 8: Bonding Concepts valence electrons ionic bonding covalent bonding electronegativity dipoles electron configuration of ions sizes of ions lone pairs of electrons, bonding pairs Lewis structures Octet rule exceptions to Octet rule resonance formal charge molecular geometry: linear, tetrahedral, trigonal pyramid, bent, trigonal planar, trigonal bipyramid, octahedral, see-saw, T-shaped, square pyramid, square planar polarity Chapter 22: Organic Chemistry properties of organic compounds saturated and unsaturated hydrocarbons alkanes, alkenes, alkynes name alkanes prefixes for 1-10 carbons draw structures structural isomers aromatic hydrocarbons functional groups alcohols carboxylic acids formic acid, acetic acid amines esters amides condensation reactions (formation of esters and amides) addition polymers condensation polymers polyesters and polyamides homopolymers & copolymers draw monomer from polymer and vice versa polypeptides SECOND SEMESTER Chapter 6: Thermochemistry heat content = enthalpy change in heat content (DH) heat content diagrams endothermic & exothermic processes thermochemical equations calorimetry: Q = c x m x DT joules, calories specific heat (Hf(, definition & use of table Hess Law complete combustion (H/mole conversions Chapter 5: Gases Kinetic-molecular theory pressure barometer, manometer temperature absolute zero temperature relationship between pressure, volume, temperature Boyles Law Charles Law Ideal Gas Law R = 0.08206 L atm/mol K molar volume STP molar volume @ STP = 22.4 L molar mass and density of a gas gas stoichiometry partial pressure formulas: Ptotal = Px + Py + . . .  PV = nRT d =   Chapter 10: Liquids and Solids Differences between gas, liquid, solid sublimation Relationship of interparticle forces and (Hfus, (Hvap, melting pt and boiling pt vapor pressure equilibrium vapor pressure of water as f(T) relative humidity dew point boiling point heating curve critical temperature & pressure phase diagrams triple point, critical point Intermolecular forces: London dispersion forces, dipole forces, hydrogen bonds Properties of the following types of solids (conductivity, melting points, solubility): molecular, network covalent, ionic, metallic Chapter 11: Properties of Solutions solute solvent concentration molarity mass percent mole fraction molality conversions between concentration units molecular and ionic solutes nonpolar and polar solutes and solvents hydrophobic and hydrophilic substances electrolytes and nonelectrolytes Saturated, supersaturated and unsaturated solutions solubility and temperature solubility and pressure colligative properties vapor pressure lowering boiling point elevation freezing point depression vant Hoff factor calculate number of moles, concentration or molar mass from freezing point Chapter 19: Radioactivity what makes elements radioactive alpha emission beta emission nuclear equations half-life nuclear fission production of radioactive waste chain reaction nuclear fusion Chapter 12: Chemical Kinetics reaction rate definition average rate for a time interval rate laws order calculation of order and k from concentration and rate factors affecting rate (and why) concentrations of reactants, temperature, surface area, catalysts reaction mechanisms elementary steps rate equations for single step reactions multistep reactions rate determining step activation energy relation to temperature relation to rate energy diagrams activated complex (transition state) catalysis Chapter 13: Equilibrium definition of equilibrium factors affecting equilibrium: temperature equilibrium constant, K expression for K from equation only gases and aqueous relate to extent of reaction find K for a reaction from K of related reactions Reaction quotient, Q, & its relationship to K calculation of K from concentrations at equilibrium and vice versa LeChateliers Principle statement of principle effect of adding or removing product or reactant effect of changing volume or pressure effect of changing temperature relationship between temperature and K for endothermic and exothermic reactions effect of changes on yield and rate Chapter 14: Acids and Bases properties of acids and bases Bronsted-Lowry model conjugate acid/base pairs amphoteric substances Kw: relationship between [H+] and [OH-] definitions of pH and pOH defining acids and bases in terms of pH, [H+], pOH, and [OH-] find pH from [H+] and [OH-] strong and weak acids and bases ionization equations Ka and Kb expressions for Ka and Kb relationship to strength of acid or base relationship between Ka and Kb calculation of Ka or Kb from pH and concentration calculation of pH from Ka or Kb and concentration acid-base properties of salt solutions Chapter 15: Applications of Aqueous Equilibria acid-base reactions buffers how they work significance of pKa of buffer Henderson-Hasselbach equation calculations relating [A-]/[HA] to pH how to prepare buffers acid-base titrations equivalence point shape of titration curves relation of strength of acid or base to pH of equivalence point pH indicators relevance of pKa of indicator Chapter 16: Ksp expression for Ksp calculations of equilibrium concentrations from Ksp and vice versa relationship to extent of solubility calculations of concentrations of ions that form precipitates common ion effect Chapter 4/18: Electrochemistry definitions from Chapter 4 oxidation and reduction oxidizing and reducing agents oxidation number oxidation-reduction reactions balancing oxidation-reduction reactions voltaic cells anode and cathode direction of electron and ion flow porous barrier/salt bridge standard reduction potentials relationship to Eoox and Eored applications of values for Eo: -./0=>?@`a /    7 ǹף|tititatatit|thMOJQJ jhQ'OJQJhQ'OJQJhQ'5>*OJQJhMhHh>ahQ' hQ'>* hQ'5>*hMhQ'CJaJh;5:OJQJhMhM5:OJQJhMhM5CJOJQJaJhQ'5OJQJh S5OJQJhQ'5CJOJQJhQ'6CJOJQJ$./>?@a 1 F p x  0 > V h q  $ ^ `a$  ^ `wXq ; w    7 C _ e w 2 Q q  ^ `q Y|4=]$Lt b h^h`  ^ ` bz|efs}/L&㴬㗐㗐㴅ہz hQ'5>*hHhMhMOJQJ hQ'6EHhQ'6OJQJ jnhM6OJQJhMOJQJhMOJQJ jnhQ'6OJQJhQ'OJQJhQ'5>*OJQJhMhQ'hQ'OJQJhQ'5OJQJhQ'5EHOJQJ,$3CLh /L^o}&7 P^`P  ^ `gdM  ^ `7IQp~,GWk  ^ `DF   "(*,.lnprt #uޛޔyslyިe h^q5>* jhH hHEH jDhHhH5CJOJQJhH56CJ hH5CJhHOJQJ hH>* hH5>*h;5>*OJQJ h&h;h;5OJQJ\hH5OJQJ\ hHhHhHhQ'hHhQ'OJQJ hQ'5>*hHOJQJ%,B]x  ^ `gdH  ^ `Lx .Pl     gdH  ^ `gd;$ ^ `a$gd;  ^ `gdH$=G^k &FXijt  ^ `uz~!"#&()*-; < > Y !!! 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