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Chemical Reactions
| Question | Answer |
|---|---|
| synthesis | 2 reactants, 1 product |
| synthesis with reactants: binary salt and oxygen | product:a chlorate |
| synthesis with reactants: metallic oxide and water | product: a hydroxide |
| synthesis with reactants: metallic oxide and carbon dioxide | product: a carbonate |
| decomposition | 1 reactant, 2 products |
| decomposition with reactant: carbonate | products: metallic oxide and carbon dioxide |
| decomposition with reactant: hydroxide | products: metallic oxide and water |
| decomposition with reactant: chlorate | products: binary salt and oxygen |
| single replacement | reactants: element and compound, products: element and compound; switch the element with its same charged ion in the compound (+ with +, - with -) |
| double replacement | reactants: 2 compounds, products: 2 compounds; switch either the cations or the anions with each other |
| combustion | products: hydrocarbon(C_H_) and oxygen, products: carbon dioxide and water |
| double replacement: sulfide and acid | H2S and a salt |
| double replacement: carbonate and acid | CO2 and H2O and a salt |
| double replacement: sulfite and acid | SO2 and H2O and salt |
| double replacement: ammonium salt and soluble strong hydroxide | NH3 and H2O and a salt |
| acid and base | salt and water |
| oxidation number of hydrogen when bonded to metals | -1 |
| oxidation number of hydrogen when not bonded to metal | +1 |
| oxidation number of Group 1A metals | +1 |
| oxidation number of Group 2A metals | +2 |
| oxidation number of F | -1 |
| IMF directly related to | MP, BP, enthalpy of fusion, enthalpy of vaporization |
| strength of IMF depend on | distance btw ion and dipole (closer=stronger attraction), charge on ion (higher charge=stronger attraction), magnitude of dipole (larger=stronger attraction) |
| polarizibility increases with | greater # of electrons, more diffuse electron cloud (bigger), and molar mass (if homologous series) |
| IMF relation to Vapor Pressure | stronger IMF = lower VP |
| Temperature relation to vapor pressure | higher temp = higher VP (more molecules will evaporate) |
| ionic crystal properties | hard, brittle, high melting points, poor conductors of heat and electricity |
| atomic/network crystal properties | stronger than IMF but weaker than ionic crystals, hard, high melting point (lower than ionic), poor conductors of heat and electrcity |
| molecular crystal properties | soft, low melting points, poor conductors of heat and electrcity |
| metallic crystals | soft or hard, low or high melting points, good conductors of heat and electrcity |
| heat of fusion | solid to liquid |
| heat of vaporization | liquid to gas |
| heat of sublimation | solid to gas |
| heat of condensation | gas to liquid |
| atomic radius: down a group | increases: increase in energy levels. force of attraction decreases |
| atomic radius: across a period | decreases: increase in nuclear charge (more protons). force of attraction increases |
| ionization energy: down a group | decreases: larger atomic radius, decrease in force of attraction, decreased hold on electrons |
| ionization energy: across a period | increases: smaller atomic radius, increase in force of attraction, tighter hold on electrons |
| electronegativity: down a group | decreases: atomic radius increases, decrease in force of attraction, looser hold on electrons, not as much energy needed to attract an electron |
| electronegativity: across a period | increases: atomic radius decreases, increase in force of attraction, tighter hold on electrons. more energy needed to attract an electron |
| ionic radius: down a group | increases: number of energy levels increase |
| ionic radius: across a period | decreases, trend repeats at beginning of anions: increased nuclear charge, increased force of attraction |
| electron affinity: down a group | less favorable (more positive): atomic radius increases, force of attraction decreases |
| electron affinity: across a period | more favorable (more negative): atomic radius decreases. force of attraction increases |
| relationship between partial pressure and mole fraction | P1/Ptotal=n1/ntotal |
| Kinetic Molecular Theory | 1) particles are in constant motion 2)collisions between particles are completely elastic, no attraction or repulsions 3) large amount of space between particles 4) speed of particles increases with increasing temp\ |
| non-ideal gas conditions | high pressure (less space, more likely to attract), low temp (not as much KE, move slower, more likely to attract) |
| to find the number to multiply emprical formula by... | molecular formula mass/ empirical formula mass |
| exponents of rates are only coefficients in a | mechanism |
| differential rate law expression | rate= k[A]^x[B]^y (only use reactants) |
| two states of matter not included in rate expression | solids and liquids (concentration has no effect) |
| half life of first order reaction | 0.693/k |
| integrated rate law for zero order reaction | [A]=[A]o-kt plot of [A] vs t gives straight line slope is negative |
| integrated rate law for first order reaction | ln[A]= ln[A]o-kt plot of ln[A] vs t gives straight line slope is negative |
| integrated rate law for second order reaction | 1/[A]= (1/[A]o) +kt plot of 1/[A] vs t gives straight line slope is positive |
| factors affecting reaction progress | KE of colliding particles Orientation of particles Frequency of Collisions Activation Energy (Ea) |
| factors affecting rates | temperature, concentrations of reactants, surface area of reactants, catalysts, pressure of gaseous reactants or products |
| breaking bonds_____ energy | releases (exothermic) |
| forming bonds _____ energy | requires (endothermic) |
| enthalpy of reaction = | products-reactants |
| calorimetry: q= | m(SH)(dT) |
| process is spontaneous when entropy is... | positive |
| entropy increases with | increased randomness of particles (solid to gas), heated, increased molar mass, increased amount of particles |
| dS surr = | -dH/T |
| when dH is neg. and dS is pos., dG is | negative at all temps |
| when both dH and dS are neg., dG is | negative at low temps, positive at high temps |
| when both dH and dS are pos., dG is | negative at high temps, positive at low temps |
| when dH is positive and dS is negative, dG is | positive at all temps |
| at equilibrium, dG = | -RT(lnK) |
| at nonstandard conditions, dG= | dGo + RT(lnQ) |
| at equilibrium dG is | 0 (K=1) |
| in spontaneous reactions, dG is | negative |
| lattice energy is directly related to _____ and inversely related to _____ | charge of ions; size of ions |
| polar molecule is | unequal distribution of electrons throughout the molecule |
| polar bond is | unequal distribution of electrons in one bond in a compound |
| formal charge= | # of VE -(electron in lone pairs + 1/2 bonded electrons) |
| molecule with 2 bonds and 0 lone pairs | linear |
| molecule with 1 bond and 1 lone pair | linear |
| molecule with 3 bonds and 0 lone pairs | trigonal planar |
| molecule with 2 bonds and 1 lone pair | bent |
| molecule with 1 bond and 2 lone pairs | linear |
| molecule with 4 bonds and 0 lone pairs | tetrahedral |
| molecule with 3 bonds and 1 lone pair | trigonal pyramidal |
| molecule with 2 bonds and 2 lone pairs | bent |
| molecule with 1 bond and 3 lone pairs | linear |
| molecule with 5 bonds and 0 lone pairs | trigonal bipyramidal |
| molecule with 4 bonds and 1 lone pair | see-saw |
| molecule with 3 bonds and 2 lone pairs | t-shaped |
| molecule with 2 bonds and 3 lone pairs | linear |
| molecule with 6 bonds and 0 lone pairs | octahedral |
| molecule with 5 bonds and 1 lone pairs | square pyramidal |
| molecule with 4 bonds and 2 lone pairs | square planar |
| when using bond energy to find enthalpy... | reactants-products |
| increasing concentration of a reactant results in shift toward | products |
| increasing concentration of a product results in shift toward | reactants |
| decreasing conc. of reactants results in shift toward | reactants |
| decreasing conc. of product results in shift toward | products |
| increasing pressure by decreasing volume results in shift toward | side with fewer gaseous molecules |
| adding an inert gas results in shift toward | neither, no effect |
| increasing temperature results in shift toward | products (exothermic favored) |
| decreasing temperature results in shift toward | reactants (endothermic favored) |
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