ACS GENERAL CHEMISTRY FINAL
• Oxidizing agent=: substance that is reduced
• Endothermic reaction=: positive ”H
• Exothermic reaction=: negative ”H
• qcal=: C(cal)”T
• q=: mCs”T
• Volume and pressure have a relationship: inverse
• Volume and temperature have a relationship: direct
• IM forces of gas: weak
• IM forces of liquid: moderate
• IM forces of solid: strong
• Hydrogen Bonding: When hydrogen bonds to C,N,F, or O, strongest, increasein
melting/boiling point
• Ion-Dipole: a mixture of ionic and polar compounds, strength of attraction de-termines
solubility
• Higher Viscosity: higher intermolecular forces and lower temperature
• Vaporization: liquid to gas (endothermic)
• Condensation: gas to liquid (exothermic)
• Increase in Vaporization: Increase in temperature, increase in surface
• van't Hoff Factor (i): the ratio of moles of solute particles to moles of formulaunits
dissolved
• Rate law=: the relationship between concentration and rateK[A]^n
• Zero Order Reaction: Independent of concentration, K[A]^0, decreases over-time
• First Order Reaction: Directly proportional to concentration, K[A]^1, doublingrate
• Second Order Reaction: Directly proportional to ([ ])^2, K[A]^2, quadruplingrate
• Rate of reaction for multiple reactions: Rate = k[A]^n[B]^n
• Dynamic equilibrium for a chemical reaction...: is the condition in which therate of the
forward reaction equals the rate of the reverse reaction
• Q=Ksp: solution = saturated; no precipitate
• Q<Ksp: solution = unsaturated; no preciptiate
• Q>Ksp: solution = above saturated: precipitate forms
, • ”S: Entropy, disorder
• ”H: Enthalpy, heat
• -”H: exothermic, more favorable
• +”H: endothermic
• +”S: more favorable
• Gibb's Free Energy Equation: ”G=”H-T”S
• ”G=0: the reaction is at equilibrium
• -”G: more favorable
• Ways to increase entropy: -increase molar mass
-allotropies: less constrained mass
-states: more ways to move
-large, more complex molecules
-dissolved solids
• Anode: oxidized, anion attracted, loses mass, positive end
• Cathode: reduced, cations attracted, negative end, gains mass
• Dipole-Dipole foreces: occur in all POLAR molecules, increase in melting/boil-ing point
• Dispersion Foreces: fluctuations in electron distribution
• Ideal gas law: PV=nRT
• ”ESystem=: -”ESurroundings
• Percent by Mass: mass of solute
x 100mass solution
• Reducing agent: substance that is oxidized
• Net ionic equation: shows only the species that change during the reaction
• Insoluble: doesn't dissolve in water, reaction will occur
• Triple Bond: sigma overlap+2 pi bonds
• Single bond=: sigma overlap
• Formal Charge=: valence electrons-[lone pairs+1/2(bonding pairs)]
• Bond type when ”E=0-0.4: Covalent Bond
• Electronegativitiy: ability of an atom to attract electrons to itself in a chemicalbond
• Oxidizing agent=: substance that is reduced
• Endothermic reaction=: positive ”H
• Exothermic reaction=: negative ”H
• qcal=: C(cal)”T
• q=: mCs”T
• Volume and pressure have a relationship: inverse
• Volume and temperature have a relationship: direct
• IM forces of gas: weak
• IM forces of liquid: moderate
• IM forces of solid: strong
• Hydrogen Bonding: When hydrogen bonds to C,N,F, or O, strongest, increasein
melting/boiling point
• Ion-Dipole: a mixture of ionic and polar compounds, strength of attraction de-termines
solubility
• Higher Viscosity: higher intermolecular forces and lower temperature
• Vaporization: liquid to gas (endothermic)
• Condensation: gas to liquid (exothermic)
• Increase in Vaporization: Increase in temperature, increase in surface
• van't Hoff Factor (i): the ratio of moles of solute particles to moles of formulaunits
dissolved
• Rate law=: the relationship between concentration and rateK[A]^n
• Zero Order Reaction: Independent of concentration, K[A]^0, decreases over-time
• First Order Reaction: Directly proportional to concentration, K[A]^1, doublingrate
• Second Order Reaction: Directly proportional to ([ ])^2, K[A]^2, quadruplingrate
• Rate of reaction for multiple reactions: Rate = k[A]^n[B]^n
• Dynamic equilibrium for a chemical reaction...: is the condition in which therate of the
forward reaction equals the rate of the reverse reaction
• Q=Ksp: solution = saturated; no precipitate
• Q<Ksp: solution = unsaturated; no preciptiate
• Q>Ksp: solution = above saturated: precipitate forms
, • ”S: Entropy, disorder
• ”H: Enthalpy, heat
• -”H: exothermic, more favorable
• +”H: endothermic
• +”S: more favorable
• Gibb's Free Energy Equation: ”G=”H-T”S
• ”G=0: the reaction is at equilibrium
• -”G: more favorable
• Ways to increase entropy: -increase molar mass
-allotropies: less constrained mass
-states: more ways to move
-large, more complex molecules
-dissolved solids
• Anode: oxidized, anion attracted, loses mass, positive end
• Cathode: reduced, cations attracted, negative end, gains mass
• Dipole-Dipole foreces: occur in all POLAR molecules, increase in melting/boil-ing point
• Dispersion Foreces: fluctuations in electron distribution
• Ideal gas law: PV=nRT
• ”ESystem=: -”ESurroundings
• Percent by Mass: mass of solute
x 100mass solution
• Reducing agent: substance that is oxidized
• Net ionic equation: shows only the species that change during the reaction
• Insoluble: doesn't dissolve in water, reaction will occur
• Triple Bond: sigma overlap+2 pi bonds
• Single bond=: sigma overlap
• Formal Charge=: valence electrons-[lone pairs+1/2(bonding pairs)]
• Bond type when ”E=0-0.4: Covalent Bond
• Electronegativitiy: ability of an atom to attract electrons to itself in a chemicalbond
