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141 Cards in this Set
- Front
- Back
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molecule
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an aggregate of at least two atoms in a definite arrangement held together by covalent chemical bonds
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Diatomic elements
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naturally occur in molecules containing two atoms
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acids
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hydrogen containing compounds that give off H+ in water
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____________ide =>add H+ ions
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hydro_______ic acid
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____ate => add H+ ions
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_____ic acid
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______ite => add H+ ions
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______ous acid
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HCl (g)
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hydrogen chloride
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HCl (aq)
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hydrochloric acid
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HF (g)
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hydrogen flouride
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HF (aq)
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hydroflouric acid
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HCN (q)
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hydrogen cyanide
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HCN (aq)
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hydrocyanic acid
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H2S (g)
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hydrogen sulfide
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H2S (aq)
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hydrosulfuric acid
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PCl3
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phosphorous trichloride
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CO2
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carbon dioxide
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N2O5
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dinitrogen pentaoxide
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SO2
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sulfur dioxide
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CO
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carbon monoxide
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NH3
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ammonia
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PH3
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phosphine
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NO
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nitric oxide
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N2O
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nitrous oxide
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H20
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water
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N2H4
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hydrazine
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chemical compounds
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formed from fixed rations of atoms or ions
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ionic compounds
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are formed between cations and anions
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covalent compounds
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are formed between nonmetal atoms
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nonmetal+nonmetal
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covalent compounds
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metal ion + nonmetal ion
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ionic compounds
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metal ion + polyanion
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ionic compound
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polyanion + polycation
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ionic compound
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molecular weights (MW)
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sum of atomic weights for atoms in molecule or the weight of the molecular formula
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Formula weights (FW)
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sum of AW for atoms in formula
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percent composition
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percent by mass of each element in the compound
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formula for determining the molecular formula
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whole number multiple=molecular weight/empirical formula weight
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product-favored reaction
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reactants turn mostly into products
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reactant-favored reaction
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reactants only form a small amount of product; they reymain mostly as reactants
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combustion reaction
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____ + O2 -> H20 + ____
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combustion definition
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burning of a fuel in oxygen is acocompanied by the evolution of energy
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Stoichiometry
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relationships between the quantities of chemical reactant and products
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Stoichiometric coefficients
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coefficients in a balanced equation
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dynamic equilibrium
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reaction when both the forward and reverse processes are still occurring at equal rates
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Do chemical reactions always proceed spontaneously toward equilibrium
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true
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solution
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homogenous mixture of 2 or more substances, solutions may be liquid solid or gaseous
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solvent
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substance present in the greates quantity
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solute
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substances other than the solvent, solutes are said to be dissolved in the solvent
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aqueous solution (aq)
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a liquid solution in which the solvent is water
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Is water the universal solvent?
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yes
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A compound that dissolves in water to an appreciable extent is _____________ if not it is _________
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soluble.....insolubule
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electrolytes
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compounds whose aqueous solutions conduct electricity
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strong electroyle----->
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conducts electricity
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weak electrolyte------>
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conducts electricity poorly
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nonelectrolyte---->
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doesn't conduct electricity
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exchange reactions
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ions of the reactants change partners
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precipitation reaction
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produces a water insoluble solids produt known as precipitate or ppt
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acid
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substance that produces hydrogen ions, H+ in aqeous solutions
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base
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substance that produces hydroxide ions (OH-) in aqeous solutions
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Salt
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compound that contains a cation other than H+ and an anion other than OH- or O2-
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common acids/bases
HCl (aq) |
strong acid/strong electrolyte
Hydrochloric acid |
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common acids/bases
HBr (aq) |
strong acid/strong electrolyte
Hydrobromic acid |
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common acids/bases
HI (aq) |
strong acid/strong electrolyte
Hydroiodic acid |
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common acids/bases
HNO3 |
strong acid/strong electrolyte
Nitric acid |
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common acids/bases
HClO4 |
strong acid/strong electrolyte
Perchloric acid |
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common acids/bases
H2SO4 |
strong acid/strong electrolyte
Sulfuric acid |
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common acids/bases
LiOH |
soluble strong base
lithium hydroxide |
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common acids/bases
NaOH |
soluble strong base
Sodium hydroxide |
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common acids/bases
KOH |
soluble strong base
Potassium hydroxide |
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common acids/bases
Ba(OH)2 |
soluble strong base
barium hydroxide |
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common acids/bases
H3PO4 |
weak acids (weak electrolytes)
phosphoric acid |
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common acids/bases
H2CO3 |
weak acids (weak electrolytes)
carbonic acid |
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common acids/bases
CH3CO2H |
weak acids (weak electrolytes)
acetic acid |
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common acids/bases
H2C2O4 |
weak acids (weak electrolytes)
oxalic acid |
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common acids/bases
H2C4H4O6 |
weak acids (weak electrolytes)
tartaric acid |
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common acids/bases
H3C6H5O7 |
weak acids (weak electrolytes)
citric acid |
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common acids/bases
HC9H8O4 |
weak acids (weak electrolytes)
aspirin |
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common acids/bases
NH3 |
weak base (weak electrolytes)
ammonia |
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nonelectrolytes
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sugar, CH4, other compounds that remain as molecules in H20
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how do electrolytes conduct electricity?
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they ionize (separate or dissociate into ions) in aqueous solution
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who carries electricity in electrolytes?
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ions carry the electricity (since they are charged species)
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strong electrolyte
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dissociate (ionize) completely or nearly completely
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weak electrolyte
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dissociate (ionize) slightly
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in an equation double arrow means
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slight dissociation/ionization
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in an equation single arrow means
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complete or near complete ionization/dissociation
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2 types of reactions for reactions prediction
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precipitation reaction and acid-base reaction
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precipitation reaction
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a solid is one of the products
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precipitate
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insoluble compound
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acid:Arrhenius definition
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an acid is a substance that when dissolved in H2O increases the concentration of hydrogen ion (H+) in solution
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base: Arrhenius definition
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a base is a substance that when dissolved in water increases the concentration of hydroxide ions OH- in the solution
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hydronium ion
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a proton in water or H+ (aq) is best represented as H30+, sometimes we will write it as H+ (aq) and sometimes H30+, HCl is best represented as a solution of H30+ and Cl-
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acid: bronsted-lowry definition
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an acid is a proton donor
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base: bronsted-lowry definition
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a base is a proton acceptor
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why do acids/bases burn
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they acid/base react with the molecules on our skin and literally a combustion reaction occurs giving us a burn
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acid-base reaction (neutralization reaction)
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reaction: acid +base -> salt +water
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will NH3 form in water?
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no
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oxides of nonmetals
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oxides of nonmetals (Co2 and SO3) have no hydrogen atoms but react with water to product H30+ ions
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Gas forming reactions most common
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most common are those leading to CO2 formation
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gas-forming reactions
metal carbonate/bicarbonate + acid -> |
metal salt + CO2 (g) + H2O (l)
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gas-forming reactions
metal sulfide + acid -> |
metal salt + H2S (g)
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gas-forming reactions
metal sulfite + acid -> |
metal salt + SO2 (g) + H2O (l)
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gas-forming reactions
ammonium salt + strong base -> |
metal salt + NH3 (g) + H2O (l)
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oxidation reduction reaction definition
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involve the transfer of electrons from one species to another
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do acid base and precipitation reactions involve redox?
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NO they DO NOT
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why use oxidation numbers? (3 reasons)
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1) provides a way to divide up the e- among the atoms
2) can be used to decide if a redox reaction has occurred 3)distinguish oxidizing and reducing agents |
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definition oxidized
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when an atom loses electrons
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definition reduced
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when an atom gains electrons
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OIL
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oxidation is loss
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RIG
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redution is gain
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elements in their elemental form have an oxidation number of ___
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zero
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the oxidation number of monatomic ion is ____
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the same as its charge
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when combines with other elements fluorine always has an oxidation number of ____
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-1
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the oxidation state of oxygen is ____ in most compounds
(except when combines with fluorine and compounds called peroxides and superoxides in which the oxidation states are -1 and -1/2 respectivily |
-2
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Cl, Br, and I have an oxidation number of _____
except when combined with oxygen and fluorine |
-1
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Cl has an oxidation state of ___ in NaCl
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-1
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Cl has an oxidation state of __ in ClO- ion
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+1
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The oxidation state of H is ____ in most compounds
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+1
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When hydrogen is bound to a metal the oxidation number is ____
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-1
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The algebraic sum of the oxidation numbers for the atoms in a neutral compound must be ____
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0
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The algebraic sum of the oxidation numbers for the atoms in a polyatomic ion must be ____
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equal to the ion charge
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oxidizing agent
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species being reduced
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reducing agent
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species being oxidized
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oxidizing agent
O2, oxygen |
reaction product
O2-, oxide ion or O combined with H2O |
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oxidizing agent
Halogen, F2, Cl2, Br2, I2 |
reaction product
halide ion, F-, Cl-, Br-, or I- |
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oxidizing agent
HNO3, nitric acid |
reaction product
nitrogen oxides, such as NO and NO2 |
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oxidizing agent
Cr2O7 2-, dichromate ion |
reaction product
Cr 3+, chromium (III) ion in acid solution |
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oxidizing agent
MnO4- permanganate ion |
reaction product
Mn2+, manganese (II) ion in acid solution |
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reducing agent
H2, hydrogen |
reaction product
H+ (aq), hydrogen ion or H combined in H2O or other molecule |
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reducing agent
M, metals such as Na, K, Fe Al |
reaction product
M^n+, metail ions such as Na+, K+, Fe 2+, Fe 3+, Al 3+ |
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reducing agent
C, carbon (used to reduce metal oxides) |
CO and CO2
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recognizing oxidation in terms of oxidation number
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increase in oxidation number of an atom
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recognizing reduction in terms of oxidation number
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decrease in oxidation number of an atom
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recognizing oxidation in terms of electrons
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loss of e- by an atom
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recognizing reduction in terms of electrons
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gain of e- by an atom
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recognizing oxidation in terms of oxygen
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gain of 1+ O atoms
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recognizing reduction in terms of oxygen
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loss of 1+ O atoms
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stoichiometry definition
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the study of the quantitative aspects of chemical reactions
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steps for stoichiometric calculations (4)
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mass reactant to moles reactant (stoichiometric factor) to moles product to mass product
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do many reactions in real life go to completion?
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nope
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2 reasons why many reactions in real life do not go to completion
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1) reactants didn't react entirely
2) reactants did react 100% but formed "undesirable" products by "side reactions" as well as the wanted products |
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theoretical yield
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R1+R2->P1 100% completion
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percent yield =
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actual yield/theoretical yield x 100%
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