Chemistry Unit 2 – Flashcards
Unlock all answers in this set
Unlock answersStrong Acids
HCl |
| Hydrochloric Acid |
Strong Acids
HBr |
| Hydrobronic Acid |
Strong Acids
HI |
| Hydroiodic Acid |
Strong Acid
HNO? |
| Nitric Acid |
Strong Acid
HclO? |
| Chloric Acid |
Strong Acid
HClO4 |
| Perchloric Acid |
Strong Acid
H2SO4 |
| Sulfuric Acid |
| Percipitate |
| An insoluable solid product that seperates from a solution |
| Soluability |
| The maximum amount of solute that will dissolve in a given quantity of a solvent @ a specific temperature |
Soluability Rules CASHIN N 1's |
+1 charge = soluable Chlorates Acetates Sulfates Halogens N?: Nirates ; Ammonium (NH4) 1's: goup 1 elements |
Insoluablity Rules SCOOP-Choclate |
Sulfide Carbonates O?: salts OH: salts Phosphates Chromates *larger the charge less soluable* |
Dissolving Properties Solids vs. Gases |
Solids: some dissolve eaiser @ higher temps
Gases: Dissolve easier @ lower temps |
| Ionic Equations |
|
| Spectator Reactions |
| ions that don't contribute anything to the reaction |
| Aqeous Solution |
| a homogeneous mixture of 2+ substances |
| Electrolyte |
a substance that dissolves into water to yield a solution that conducts electricity * presence of ions allows it to conduct electricity* |
| Nonelectrolye |
| A substance that dissolves in water to yield a soltion that dosen't conduct electricity |
| Dissociation |
| When an ionic compound breaks into its ions |
| Ionization |
| When a covalent molecular compound forms into it's ions |
| Dissolving |
| When a molecular compound stays intact |
| Strong Electrolyte |
| An electrolyte that dissociates comletely |
| Strong Bases |
Metals in groups 1&2 LiOH, NaOH, KOH, RbOH, CaOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 |
| Acids |
| a proton (H+) donor |
| Bases |
| a proton (H+) acceptor |
| Monoprotic Acids |
| strong acids wher each mlecule has 1 proton to donate |
| Diprotic Acids |
Each acid milecule has 2 protons that it can donate *only strong during first ionization* |
| Polyprotic Acids |
|
| Neutralization Reaction |
A reaction between an acid and a base that produces water and salt *anion from the acid & cation from the base* |
| Oxidation-Reduction Reaction/Redox Reactions |
| chemical rection in which high energy electons are transferred from 1 reactant to a lower energy reactant |
| OIL RIG |
OIL: Oxidation is the loss of electrons
RIG: Reduction is the gain of electrons *when you gain an electron the oxidation # decreases* |
| Assigning Oxidation #s |
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 |
Type of Redox Reaction
Displacement Reaction |
metals are switched out Zn + CuCl2 --> ZnCl + Cu |
Type of Redox Reaction
Combination Reaction |
two ions come together N2 + 3H2 --> 2NH3 |
Type of Redox Reaction
Decomposition |
Start with a compound and break down into ions 2NaH --> Na = H2 |
Type of Redox Reaction
Disproportion Reaction |
when a substance is reduced and oxidized at the same time 2H2O2 --> 2H2O2 + O2 |
Type of Redox Reaction
Combustion Reaction |
when something burns in the presence of oxygen and creates carbon dioxide and water CH4 + 2O2 --> CO2 + 2H2O (C1)(V1) = (C2)(V2) |
| Molarity |
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) |
| Titration of an acid w/ a base |
| base of the known concentration is added to an acid of unknown concentration |
| Dilution |
| the process of preparing a less concentrated solution from a more concentrated one |
| Energy |
| The capacity to do work or transfer heat |
| Kinetic Energy |
| energy that results from motion |
| Potential Energy |
| energy possessed by an object by virtue of its position |
| Thermal Energy |
| a form of kinetic energy when energy associated w/ the random motion of atoms & molecules |
| How does thermal energy measured? |
| measures changes by monitoring temp changes |
| Chemical Energy |
| energy stored w/in the structure units (molecules/polyatomic ions) of chemical substances |
| Electrostatic Energy |
| potential energy that results from the interaction of charged particles |
| law of conservation of energy |
| when energy of one form disappears, the same amount of energy must appear in another form(s) |
| System |
| the specific part of the universe that is of interest Where the chemical reaction takes place |
| Surroundings |
| rest of the universe outside of the systems |
| Exothermic Process |
| process that gives off energy ex) handwarmers, burning a log |
| Endothermic Process |
| process that absobrs thermal energy as heat ex) cold packs |
| What is the SI unit of energy and what does it measure? |
| Joules & amount of kinetic energy |
| Thermodynamics |
| study of the effects of work, heat, and energy (E) of a system |
| Open System |
| chain exchange mass & energy w/ its surroundings |
| Closed System |
| allows the transfer of energy nut not mass |
| isolated system |
| does not exchange either mass or energy w/ its surroundings |
| First Law of Thermodynamics |
| mass & energy can't be created or destroyed |
| Internal Energy |
| the system = delta U Delta U = Uf - Ui total must be 0 one +, one - |
| Heat |
| when a system releases of absorbs heat it's internal energy (delta U) changes |
| q = ? |
| q = heat |
| w = ? |
| w = work |
| U decreases when... |
| releasing heat = q<0 doing work ON the surrounding work ON the surrounding = w<0 |
| U increases when... |
| heat is absorbed by the system q>0 work done on the system w>0 |
| Enthalpy |
| H = U+PV internal E of system + (pressure x vol of system) |
| Change in Enthalpy |
| delta H = delta U + delta(PV) |
| Enthalpy (delta H) |
| the different between the enthapies of the products & the enthapies of the reactants |
| Thermochemical Equations |
| chemical equations that show the enthalpy changes & the mass relationships |
| Guidelines of thermochemical equations |
| 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 |
| Calorimetry Specific Heat (s) of a substance |
| the amount of heat required to change 1g of the substance by 1 degree C |
| Calorimetry Heat Capacity |
| heat required to raise the temp of an object by 1 degree C |
| Exothermic reactions what do they do to the specific heat equation? |
| Make it negative |
| Hess's Law |
| 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 |
