-
-
HCO3- reaction with H+ or OH-
HCO3- +H+ yields CO2(g) + H2O(l)
-
CO32- reaction with H+ or OH-
CO32- + 2H+ yields CO2(g) + H2O(l)
-
HSO3- reaction with H+ or OH-
HSO3- + H+ yields SO2 (g) + H2O(l)
-
SO32- reaction with H+ or OH-
SO32- + 2H+ yields SO2 (g) + H2O(l)
-
HS- reaction with H+ or OH-
HS- + H+ yields H2S(g)
-
S2- reaction with H+ or OH-
S2- + 2H+ yields H2S(g)
-
NH4+ reaction with H+ or OH-
NH4+ + OH- yields NH3 (g) + H2O(l)
-
the oxidation number of a free element is always
0
-
The oxidation number of a monatomic ion equals the
charge of the ion
-
The oxidation number of oxygen in compounds is
-2
-
The oxidation number of a Group IA element in a compound is
+1
-
The oxidation number of a Group 2A element in a compound is
+2
-
The oxidation number of a Group 7A element in a compound is
-1
-
The sum of the oxidation numbers of all of the atoms in a neutral compound is
0
-
The sum of the oxidation numbers in a polyatomic ion is equal to
the charge of the ion
-
The oxidation number of Hydrogen when bonded to a nonmetal
+1
-
The oxidation number of Hydrogen
when bonded to a metal
-1
-
Electrolytes
attraction between ion and water is greater that attraction between cation and anion
-
Strong electrolytes
- dissolve in water and produce ions
- strong acids and strong bases (group 1A and 2A are strong bases if they dissolve in water)
- HCl, HBr, HI, HNO3, H2SO4, HClO4
-
nonelectrolytes
- do not dissolve in water (no polar bonds)
- cations and anion stay together
- do dissolve in water but give no ions (sugars and esters and polar OH bonds interact with water)
-
Weak electrolytes
- weak base, not all will seperate to form ions
- HF, NH3, Carboxylic acid (HC2H3O2)
-
Precipitation Reactions
two soluble compounds react to form an insoluble product
-
Driving Force
removal of ions from solution of a preciptate (as gas or H2O)
-
Total Ionic Equation
shows soluble substances that ionize or dissociate as ions
-
Spectator ions
ions not involved in chemical change
-
net ionic equation
elinimates spectator ions and shows actual chemical change
-
Neutralization
occurs when an acid reacts with a base
-
Polyprotic acids
contain more than one ionizable proton
-
Strong acid-base reaction
dissociate completely into ions when dissolved in water
-
weak acid-base reactions
dissociate very little in water
-
Driving force of an acid-base reaction
- electrostatic attraction of ions and their removal from their solution
- formation of water and salt
-
Titration
process whereby one solution of known concentration is used to determine the concentration of another solution containing the analyte
-
Titrant
known concentration
-
Analyte
Unknown concentration
-
Titration Indicator
substance that changes color at the endpoint
-
titration: equivalence point
stoichiometrically equivalent amounts of titrant and analyte present (moles H+=moles OH-)
-
titration endpoint
where indicator changes color (slight excess of titrant present)
-
Redox Reaction
electron transfer reaction
-
Oxidation
- LEO
- loss of electrons
- increases in oxidation number
-
Oxidizing agent
- takes on electrons
- undergoes reduction
-
Reduction
- GER
- gains electrons
- decresases in oxidation number
-
Reducing Agent
- gives away electrons
- undergoes oxidation
-
Oxidation Number
number used to keep track of which species loses electrons and which species gains them
-
Ionic compounds
oxidation numbers for elements (ions) usually equals ionic charge
-
Covalent Compounds
oxidation numbers more dependent upon other species in compound
-
Commonly used oxidizing agents
MnO4 and Cr2O7
-
naming equations: classical system
use metallic root plus suffix to indicate oxidation state of cation
-
naming equations: classical system: ion with lower charge
ous
-
naming equations: classical system: ion with higher charge
ic
-
arrhenius acid
- H conatining molecular compound that yields H+ when dissolved in water
- ex: HCl
-
arrhenius base
- OH containing compound that yields OH- when dissolved in water
- ex: NaOH
-
salt
ionic compound formed when a base and an acid undergo neutralization
-
binary acids
- formed when some gaseous compounds dissovle in water
- prefix+nonmetal root+suffix+acid
- Hydrochloric acid
-
Oxoacids
- acids of oxoanions
- oxoanion root+suffix+acid
- nitrous acid
-
Oxoacids: "ate" in anion becomes
"ic"
-
oxoacids: "ite" in anion becomes
"ous"
-
molecular mass
sum of atomic masses of elements in a covalent compound (mass of a molecule)
-
Formula Mass
sum of atomic masses of elements in an ionic compound
-
unit usually used to express molar mass
grams (g)
-
unit usually used to express formula mass
Daltons (D) or amu
-
mass percent
= (mass of A/mass compound) * 100
-
Molecular Formula can be determined if
the molar mass and the empirical formula are known
-
equation to find molecular formula
= (molecular mass/empirical formula mass) * empirical formula
-
Combustion
compound + O2 yields CO2 + H2O
-
Hydrocarbons
compounds containing only carbon and hydrogen
-
alkanes
- saturated hydrocarbons
- maximum number of H atoms
- contains only single bonds
- ___ane
-
Alkenes
- unsaturated hydrocarbons
- less than maximum number of H atoms
- at least one double bond
- ____ene
-
-
-
-
-
-
-
-
-
-
-
Alkynes
- unsaturated hydrocarbon
- less than maximum H atoms
- contains at leas one carbon-carbon triple bond
- ___yne
-
Alcohols
- functionalized hydrocarbon
- OH (hydroxyl group)
- uses word stem to indicate number of carbon atoms plus suffix "ol"
- ___anol
-
Carboxylic Acids
- hydrocarbon
- COOH
- in water yield H+
- weak acid
- name: uses Latin root plus "ic" suffix
- ___anoic acid
-
Amines
- hyderocarbon
- NH2
- in water yield OH-
- weak base
- name: uses word stem to indicate number of carbon atoms plus "amine"
- ___ylamine
-
Stoichiometry
calculating amounts of reactants and products
-
Steps for stoichiometry problems
- 1) write balanced equation
- 2) convert amount of a given substance to moles
- 3) set up and perform conversion
- 4) convert result to desired unit
-
limiting reactant
reactant that determines how much product can be produced
-
steps for limiting reactant problems
- write balanced equation and overall equation if applicable
- determine limiting reactant
- relate each reactant given to product formed or relate one reactant to other reactant
-
percent yield
(actual yield/theoretical yield) * 100
-
overall percent yield
(%yield A/100) * (% yield B/100) .... *100
-
Molarity
= moles of solute/ liters of solution
-
Calculating reactants and products
use same techniques but convert volume to moles of reactants using concentration as a conversion factor
|
|