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| An insoluable solid product that seperates from a solution |
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| The maximum amount of solute that will dissolve in a given quantity of a solvent @ a specific temperature |
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Soluability Rules
CASHIN N 1's |
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+1 charge = soluable
Chlorates
Acetates
Sulfates
Halogens
N²: Nirates & Ammonium (NH4)
1's: goup 1 elements |
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Insoluablity Rules
SCOOP-Choclate |
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Sulfide
Carbonates
O²: salts
OH: salts
Phosphates
Chromates
*larger the charge less soluable* |
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Dissolving Properties
Solids vs. Gases |
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Solids: some dissolve eaiser @ higher temps
Gases: Dissolve easier @ lower temps |
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- Keeps precipitant together
- gets rid of ions that don't contribute to the equation
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| ions that don't contribute anything to the reaction |
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| a homogeneous mixture of 2+ substances |
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a substance that dissolves into water to yield a solution that conducts electricity
* presence of ions allows it to conduct electricity* |
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| A substance that dissolves in water to yield a soltion that dosen't conduct electricity |
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| When an ionic compound breaks into its ions |
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| When a covalent molecular compound forms into it's ions |
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| When a molecular compound stays intact |
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| An electrolyte that dissociates comletely |
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Metals in groups 1&2
LiOH, NaOH, KOH, RbOH, CaOH,
Ca(OH)2, Sr(OH)2, Ba(OH)2 |
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| strong acids wher each mlecule has 1 proton to donate |
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Each acid milecule has 2 protons that it can donate
*only strong during first ionization* |
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- Those w/ many protons
- each ionization is incomplete
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A reaction between an acid and a base that produces water and salt
*anion from the acid & cation from the base* |
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| Oxidation-Reduction Reaction/Redox Reactions |
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| chemical rection in which high energy electons are transferred from 1 reactant to a lower energy reactant |
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OIL: Oxidation is the loss of electrons
RIG: Reduction is the gain of electrons
*when you gain an electron the oxidation # decreases* |
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Free elements are 0 (neutral)
Ions: thier charge from PT
Oxygen is -2
Hydrogen is +1
Sum of the molecule is 0 or change indicted on the molecule
Outside first Inside Last |
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Type of Redox Reaction
Displacement Reaction |
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metals are switched out
Zn + CuCl2 --> ZnCl + Cu |
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Type of Redox Reaction
Combination Reaction |
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two ions come together
N2 + 3H2 --> 2NH3 |
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Type of Redox Reaction
Decomposition |
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Start with a compound and break down into ions
2NaH --> Na = H2 |
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Type of Redox Reaction
Disproportion Reaction |
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when a substance is reduced and oxidized at the same time
2H2O2 --> 2H2O2 + O2 |
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Type of Redox Reaction
Combustion Reaction |
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when something burns in the presence of oxygen and creates carbon dioxide and water
CH4 + 2O2 --> CO2 + 2H2O
(C1)(V1) = (C2)(V2) |
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the # of moles of solute per liter of solution
Symbol: M
Equation: M = Moles of solute/liters solution
g=MW (g/mol) x M (mol/L) x V(L) |
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| Titration of an acid w/ a base |
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| base of the known concentration is added to an acid of unknown concentration |
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| the process of preparing a less concentrated solution from a more concentrated one |
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| The capacity to do work or transfer heat |
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| energy that results from motion |
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| energy possessed by an object by virtue of its position |
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| a form of kinetic energy when energy associated w/ the random motion of atoms & molecules |
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| How does thermal energy measured? |
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| measures changes by monitoring temp changes |
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| energy stored w/in the structure units (molecules/polyatomic ions) of chemical substances |
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| potential energy that results from the interaction of charged particles |
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| law of conservation of energy |
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| when energy of one form disappears, the same amount of energy must appear in another form(s) |
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the specific part of the universe that is of interest
Where the chemical reaction takes place |
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| rest of the universe outside of the systems |
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process that gives off energy
ex) handwarmers, burning a log |
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process that absobrs thermal energy as heat
ex) cold packs |
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| What is the SI unit of energy and what does it measure? |
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| Joules & amount of kinetic energy |
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| study of the effects of work, heat, and energy (E) of a system |
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| chain exchange mass & energy w/ its surroundings |
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| allows the transfer of energy nut not mass |
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| does not exchange either mass or energy w/ its surroundings |
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| First Law of Thermodynamics |
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| mass & energy can't be created or destroyed |
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the system = delta U
Delta U = Uf - Ui
total must be 0
one +, one - |
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| when a system releases of absorbs heat it's internal energy (delta U) changes |
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releasing heat = q<0
doing work ON the surrounding
work ON the surrounding = w<0 |
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heat is absorbed by the system q>0
work done on the system w>0 |
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H = U+PV
internal E of system + (pressure x vol of system) |
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| delta H = delta U + delta(PV) |
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| the different between the enthapies of the products & the enthapies of the reactants |
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| chemical equations that show the enthalpy changes & the mass relationships |
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| Guidelines of thermochemical equations |
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1. always specify the physical states of all reactant & products becasue they help determine actual enthropy stages
2. multiply both sides of a thermochemical equation by a factor n
3. when we reverse a chemical equation we have to reverse the rules of delta H |
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Calorimetry
Specific Heat (s) of a substance |
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| the amount of heat required to change 1g of the substance by 1 degree C |
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| heat required to raise the temp of an object by 1 degree C |
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| Exothermic reactions what do they do to the specific heat equation? |
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| Change in enthalpy that occurs when reactants are converted to products in a reaction is the same where they reaction takes place in one step or 3 |
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