chapter 3/4 review Flashcards
chemical equilibruim
reached when a chemical reaction reaches a state where the reactants and products stop undergoing any change
the chemical reaction is still going on, but without any change
all chemical reactions try to
reach equilibrium
solutions
homogeneous mixtures involving solvent (does the dissolving) and solute (thing that is dissolved)
when an ionic compound goes into an aqueous solution…
it is hydrated and breaks up into individual ions
electrolytes
ionic solutions that are good conductors of electricity
strong electrolytes
soluble and dissolve
weak electrolytes
insoluble and don’t really dissolve
non electrolytes
solutions of molecular/covalent compounds and do not conduct electricity
does insoluble mean that you will never dissolve
no, it creates a solid (precipitate)
salts containing _________ are soluble (no exceptions)
Na+, NH4+, NO3-, ClO3-, ClO4-. CH3CO2-
almost all salts of ____ are soluble EXCEPT WITH
Cl-, Br-, I- (aq)
Ag+, Hg2 2+, Pb 2+ (exceptions=insoluble)
almost all salts containing __ are soluble (aq)
F- (aq)
exceptions= Mg2+, Ca2+, Sr2+. Ba2+, Pb2+
almost all salts containing SO4 2- are soluble except with
exceptions= Ca2+, Sr2+, Ba2+, Pb2+, Ag+
most salts with _______ are INSOLUBLE except with
CO3 2-, PO4 3-, C2O4 2-, CrO4 2-, S2-
exceptions (aq)= NH4+, group 1 metals, BaS
most metal hydroxides and oxides are insoluble except with
exceptions (aq)= group 1 hydroxides, Ba(OH)2 and Sr(OH)2
precipitation reaction (double displacement)
the cation and anion pairs swap to make new ionic compounds
the insoluble compound precipitates out (s)
Arrhenius def of an acid and base
acid= a substance that when dissolved in water produces H+
base= a substance that when dissolved in water produces OH-
bronsted-lowry definition of an acid and a base
acids= H+ donor
base- H+ acceptor
strong acids
HCl, HI, HBr, H2SO4, HClO3, HClO4, HNO3
weak acids
carboxylic acids (-COOH) and oxyacid’s NOT on the strong list
strong base pneumonic
Larry Never Kicked Can Straight Beautifully
strong bases
LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
weak bases
any bases not on the strong list and often include an NH bond
strong base and strong acid=
strong electrolyte
weak base and a weak acid=
weak electrolyte
acid-base reactions (neutralization reactions)
Acid + Base —> H2O + Salt
redox reactions
involve atoms that change their oxidation states
oxidation rule 1
atoms in their elemental form have oxidation state of zero
oxidation rule 2
a monoatomic ion has the same oxidation as its charge
oxidation rule 3
fluorine has a -1 oxidation state
oxidation rule 4
oxygen has a -2 oxidation state (except for H2O2 which has a -1 oxidation state)
oxidation rule 5
hydrogen has a +1 oxidation state
oxidation rule 6
halogens other than fluorine have a -1 oxidation state
reduction
is GAINING an electron
it is the oxidizing agent
oxidation
is LOSING an electron
is the reducing agent
combustion reactions are usually
redox reactions
percent yeild
actual (g)/ theoretical (g) times 100
concentration/ molarity (M)
mole of solute/ liters of solution
dilution eq
M1V1 = M2V2
