General Facts from entire course
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| Calculate Oxidation # of an element | Molecule charge = (# of O)(oxygen's oxidation #: -2)+element in questionEX: SO3^2- calculate oxidation # of S-2=3(-2)+S; -2=-6+S; add 6 to both side to cancel; S=4
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| LEO the lion says GER | loose electrons oxidize; gain electrons reduce
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| Base | Proton acceptor
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| Acid | Proton donor
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| Reactions in solutions | Write equation from species present; balance equation; determine moles of reactants; identify limiting reactant; determine moles of products
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| To determine molarity of a compound | M=moles of solute/L of solution
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| To determine molality | Molal=moles of solute/mass of solvent(kg)
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| To determine % yield | %yield=actual yield/theoretical yield x 100
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| To convert mL to L | Multiply by 1000
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| To figure mols/L | L x moles reactant/L
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| Oxidation Agent | Species involved in the reduction reaction
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| Reduction Agent | Species involved in the oxidation reaction
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| Anions | Negative charge; Larger than neutral element because electron cloud is screened by electrons and pull toward nucleus is less
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| Cations | positive charge; Smaller than neutral element because more electrons in electron cloud causes nuclear pull to be stronger
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| Periodic Trend: Atomic Size | →decreasing↓increasing
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| acceleration | the rate of change of velocity; distance/time2
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| Alcohol | a class of organic compounds with the general structure R-OH
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| Alkane | a saturated hydrocarbon with the general formula CnH2n + 2
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| Alkene | an unsaturated hydrocarbon that contains a carbon-carbon double bond and has the general formula CnH2n
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| ampere (A) | the SI base unit of electric current; 1 A = 1 C/s
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| atmosphere (atm) | a non-SI unit of pressure; 1 atm = 1.013250 x 105 Pa
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| Avogadro's number (NA) | the number of atoms in exactly 12 grams of carbon-12; NA = 6.0221367 x 1023; the number of things in a mole
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| Cation | a positively charged ion
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| base SI unit | one of the seven fundamental SI units; the meter (m) for length
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| combustion reaction | an exothermic reaction in which a substance is combined with oxygen gas
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| density | mass/volume
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| dimensional analysis | a method for solving for a quantity by multiplication by conversion factors
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| electron | a subatomic particle with a negative charge and a mass of 9.1092897 x 10-31 kg
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| exothermic | a process in which energy is given off by a system; q < 0
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| ion | an atom or group of atoms with a net positive or negative charge
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| energy | the capacity to do work or transfer heat
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| excited state | any energy state of the electron higher than the ground state
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| ground state | the lowest available energy state for a given electron
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| hydrocarbon | a molecule made up entirely of hydrogen and carbon atoms
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| ionic compound | a compound composed of anions and cations
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| isomers | compounds with the same molecular formula but with different atomic structures
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| isotopes | atoms that have the same number of protons but different numbers of neutrons
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| kinetic energy (KE or Ek) | the energy associated with particles in motion; KE = (1/2)mv2
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| linear relationship | a mathematical relationship between two quantities such that as one increases
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| mass number | the number of protons and neutrons in the nucleus of a given isotope; the relative atomic mass of a given isotope; the total number of nucleons in an atom
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| mole | the amount of substance that contains as many particles as exactly 12 grams of carbon-12; 6.0221367 x 1023 things
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| Newton (N) | the SI unit of force; 1 N = 1 kg•m/s2
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| Noble gas | an element from group 18(VIIIA) on the periodic table; an nonreactive element with an entirely filled valence shell
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| Oxoacid | an acid that contains oxygen; oxyacid
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| pascal (Pa) | the SI unit of pressure; 1 Pa = 1 N/m2 = 9.869233 x 10-6 atm
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| HSO3 - | bisulfite
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| CO3 2- | carbonate
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| C2H3O2 - | acetate
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| C2O4 2- | oxalate
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| Cr2O7 2- | dichromate
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| ClO4 - | perchlorate
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| S2O3 2- | thiosulfate
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| HClO4 | perchloric acid
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| H2SO4 | sulfuric acid
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| HSO4 - | bisulfate
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| NH4 + | ammonium ion
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| CrO4 2- | chromate
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| OH- | hydroxide
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| O2 2- | peroxide
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| HCOO- | formate
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| SO4 2- | sulfate
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| SO3 2- | sulfite
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| CN- | cyanide
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| MnO4 - | permanganate
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| HNO3 | nitric acid
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| HCl | hydrochloric acid
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| BaSO4 | barium sulfate – not soluble
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| PbSO4 | lead sulfate – not soluble
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| CaSO4 | calcium sulfate – not soluble
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| Sr(OH)2 | Strontium hydroxide – base - mostly soluble
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| Ba(OH)2 | barium hydroxide – base – mostly soluble
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| HBr | hydrobromic acid
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| HI | hydroiodic acid
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| Rb+ | rubidium ion – soluble
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| Cs+ | cesium ion – soluble
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| K+ | potassium ion – soluble
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| Na+ | sodium ion – soluble
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| Li+ | lithium ion – soluble
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| NO3 - | nitrate – soluble
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| HCO3 - | bicarbonate
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| SCN - | thiocyanide
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| S2O2 2- | thiosulfate
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| HgSO4 | mercury sulfate – not soluble
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| Pb+ | lead ion – not soluble
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| Hg2 2+ | mercury salt – not soluble
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| S 2- | Sulfur – slightly soluble
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| Ca(OH)2 | calcium hydroxide – strong base – mostly soluble
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| PO4 3- | phosphate
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| Ideal Gas Law | PV=nRT where P is pressure(atm); V is volume(in L); n is # of moles of gas; R is 0.08206; T is temperature (in K)
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| STP | standard temperature and pressure; T is 0°C or 273K; P is 1 atm
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| Periodic Trend: electronegativity | →increases ↓decreases
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| Periodic Trend: Ionization energy | →increases ↓decreases
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| Periodic Trend: electron affinity | →increasingly negative ↓decreasingly negative
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| Covalent Bond | when two atoms share electrons
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| Ionic bond | when a atom transfers one of it’s electrons to another atom
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| Parts per million | mass of solute/total mass of solution x 1
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| Percent by mass | mass of solute/total mass of solution x 100
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| Steps to balance Reduction Oxidation equations in acid | 1.write 2 ½ equations; 2. balance all not O or H; 3. add H20 to balance O; 4. add H+ to balance H in H2O; 5. add electrons to balance charges; 6. balance e- on both sides by multiplying whole ½ equation as needed; 7. Cancel out and re-write.
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| Steps to balance Reduction Oxidation equations in base | follow steps for acid and then 1. add OH- to both sides to cancel all H+; 2. combine H+ and OH- to form H2O; 3. add H2O; 4. check atoms and charge for balance.
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| Ionization energy | the energy it takes to remove an electron from an atom and make it into an ion.
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| Electron affinity | the energy change in an atom when it gains an electron.
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| Electronegativity | the ability of an atom to attract an electron of another atom when they are associated through a bond
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| Octet rule | states that an atom is more likely to gain electrons the more full it’s valence shell becomes.
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| Ionic compounds | high electricity conductors when dissolved in H2O; hard crystals; mostly soluble
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| Dissociation | when ionic compounds dissolve into their separate ions in water.
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| Sublimation | when a solid is taken into is gaseous form
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| Titration | used to find the amount of an unknown substance by adding a known substance to neutralize the unknown.
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| Net ionic equation | includes only the species of an equation that is involved in the reaction (reactants → precipitates)
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| Enthalpy | E=PV
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| Exothermic reaction | when energy is given off by reaction (& heats surroundings)
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| Endothermic reaction | when energy is used up by a reaction (& cools surroundings)
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