Front Back
Solution
Homogenous substance -may be gas, liquid, or solid
Solvent
component present in the greatest quantity in a solution
Solute
components of a solution in lesser quantities than solvent
Molarity (molar concentration)
Number of moles of solute divided by liters of solution
Dilution
creating a less concentrated solution by adding more solvent
M of solute=
Molarity x Volume (Mi x Vi= Mf x Vf)
Water
-polar molecule with a dipole -bent molecular shape -uneven distribution of electrons
Electron distribution in H2 and H2O
H2: symmetrical H2O: asymmetrical, each bond is polar, entire molecule is polar
Strong electrolytes
dissociate almost completely into ions in water. Ions are hydrated (surrounded by water molecules). Charge carriers in solution lead to good conductivity. (soluble ionic compounds, strong acids, strong bases, most molecular hydrogen halides)
Nonelectrolyte
Does not dissociate into ions in a water solution. Solution does not conduct electricity. (most molecular compounds)
Weak Electrolytes
dissociates only partially to ions in solution of water. Only partial conductivity of electrical currents. (create weak acids + bases such as HF, NH3)
Ways to write molecular equations
All reactants and products written as chemical formulas
Ways to write Ionic equations
compounds that dissociate are written in ionic form. spectator ions appear on both sides of the equation
Ways to write a net ionic equation
eliminate spectator ions; shows net reaction
Net Ionic Equation
Must be balanced both by atoms and charge. Focuses only on net chemical change. Emphasizes similarities in chemistry.
Types of reactions in solutions
precipitation acid-base oxidation-reduction
Precipitation reactions
soluble reactants yield an insoluble product. also known as double displacement or metathesis
Acid-base reactions
acid reacts with base to afford water and salt. also called a neutralization. can be viewed as a proton (H+) transfer reaction.
Oxidation-reduction reactions
involves transfer of electrons between reaction partners. charges on atoms in reactants can change. O atoms can appear to be transferred. also called redox. reactions can be run so electrons flow in external wire as electricity.
Solubility rules (predict precipitation reactions)
-All NH4+ & alkali metal compounds (Li+,Na+,K+,Rb+,Cs+) are soluble -all NO3-,C2H3O2-,HCO3-,ClO4- compounds soluble -all Cl-,Br-, I- compounds are soluble, except for Ag+, Hg22+, Pb2+ -All SO42- compounds are soluble except for Ba2+, Sr2+, Pb2+, Ag+, and Ca2+ -Most O2-, OH0, CO32-, an…
Balanced Chemical Equations
-total number of atoms unchanged -net charge unchanged -only adjust coefficients
Combustion reaction
reactants: Compound + O2 Products: CO2+H2O+ other element oxides
Precipitation reaction
reactants: two or more ionic compounds products: pairwise exchange of ions
general procedure for stoichiometry problems
mass known/MW=mol known mol unknown x MW= mass unknown
Limiting reagents
-reactions eventually consume all of one reactant and stop -other reactants are in excess and called excess reactants
Percent yield
(actual yield/theoretical yield) x 100
Concentration
-number of grams of solute per 100 g of solution
Solubility
-number of grams of solute that can dissolve in 100g of solvent at a given temperature -often increases with temp -supersaturated solutions are unstable and often result in the formation of a precipitate
Molarity
molar concentration (M)= number of mol solute/number of L solution
Dilutions
*moles of solute are constant Moles of solute= molarity x volume (Mi x Vi = Mf x Vf)
Solubility Rules Predict Precipitation Reactions
1. identify all cations and anions present 2. apply solubility rules to each possible pair 3. any insoluble pair will precipitate
Acids
react with water to produce H+ (aq) generally molecular compounds that ionize
Bases
substances that react with water to produce OH- (aq) tend to be ionic compounds
Titration
quantitative, volumetric technique used to determine concentration of 'unknown' solution. Mb x Vb = Ma x Va
Oxidation-reduction reaction
oxidation-
OILRIG
Oxidation Involves Loss of electrons Reduction Involves Gain of electrons

Access the best Study Guides, Lecture Notes and Practice Exams

Login

Join to view and access 3M+ class-specific study document.

or
We will never post anything without your permission.
Don't have an account?
Sign Up

Join to view 2 2 and access 3M+ class-specific study document.

or

By creating an account you agree to our Privacy Policy and Terms Of Use

Already a member?