Chemistry: The Big Picture What impact does chemistry have on our everyday lives? How does the structure of individual atoms determine their behavior in all types of matter? What mathematical relationships can be used to predict the interaction of matter? How do environmental conditions affect the interactions of matter?

Final Exam BIG Topics What do you know? What do you need to know? Atomic Structure (structure/isotopes) & Nuclear Chemistry Electrons in Atoms (electron configurations/equations) Periodic Table/Periodic Trends Chemical Bonding (Ionic/Molecular/Metallic) Lewis Structures/Electron Geometry/Molecular Geometry Organic Chemistry Types of Reactions, Net Ionic Equations, Reaction Stoichiometry, Limiting Reagent States of Matter, Gas Laws Water & Aqueous Systems (Solutions/Colligative Properties) Thermochemistry Reaction Rates & Chemical Equilibrium Acids & Bases

Big Problems Items Nuclear Reactions Electron configurations Math of an electron Organic Chemistry Chemical Reactions Net Ionic Equation Stoichiometry/Limiting Reagent Chemical Equilibrium (Keq or Ksp) Acid or Base Dissociation (Ka or Kb) Freezing Pt Depression or Boiling Pt Elevation Hess Law Titration Thermochemistry Gas Laws

Chemical Formulas Topics: Balanced chemical reactions, net ionic equations, oxidation reduction Can you determine the molar mass of these substances? Can you draw a VSEPR model of a water molecule? Water Sodium nitrate Copper (II) carbonate Iron (III) bromide Hydrochloric acid Carbonic acid Sodium hydroxide Can you identify the substances as an acid, base, salt, ionic or molecular? Can you combine the components and write balanced chemical reactions?

Chemical Names MgSO4 HBr NaOH NH3 CuS

Net Ionic Equations A student reacts aqueous barium nitrate and aqueous sodium sulfate in a test tube. Balance the occurring chemical reaction. Write the net ionic equation. Identify the spectator ions.

Composition Stoichiometry Activity Complete A-F with the correct conversion factor. A B F C D E

Composition Stoichiometry What is the number of moles in 432 g Ba(NO3)2 ? How many atoms are in 3.25 grams of calcium carbonate?

Stoichiometric Calculations The figure below summarizes the steps for a typical stoichiometric problem.

Reaction Stoichiometry Diagraming the process for the following types of problems Mole-mole (Always used to solve Rxn Stoic problems) Mass-mole Mole-Mass Mass-Mass Mass-Volume Volume-Mole

Reaction Stoichiometry Iron( III) oxide is formed when iron combines with oxygen in the air. How many grams of Fe O are formed when 16.7 g of Fe reacts completely with oxygen? ___Fe (s) + ___O2 (g)  ___Fe2O3 (s)

_____N2 + _____H2  _____NH3 Limiting Reactant How many grams of NH3 can be produced from the reaction of 96 g of N2 and 32.1 g of H2? _____N2 + _____H2  _____NH3

Molecular formula Determine the molecular formula of a compound with the empirical formula of C2H4O and molar mass of 88g.

Using the data shown in the diagram, determine the value for P2. 75 kPa 660 kPa 130 kPa 21 kPa 150 kPa

Gas Laws How many moles of N2 are in a flask with a volume of 250 mL at a pressure of 3 atm and a temperature of 300.0 K?

Colligative properties Calculate the freezing point of 50.0 g of water if 5 grams of NaCl is added to the water.

Thermochemistry If heat is released by a chemical system, an equal amount of heat will be ____. a. absorbed by the surroundings c. released by the surroundings b. absorbed by the universe d. released by the universe

Thermochemistry How much heat (in kJ) is released or absorbed when 0.265 mol of sodium bicarbonate is decomposed according to the reaction below? 2NaHCO3(s)  Na2CO3(s) + H2O(g)+ CO2(g) H =129 kJ

Thermochemistry Calculate H for the reaction of sulfur dioxide with oxygen. 2SO2 (g) + O2 (g)  2SO3 (g) ( H SO2 (g) = –296.8 kJ/mol;  H SO3 (g) = –395.7 kJ/mol)

Thermochemistry: Hess’s Law PbCl2(s) + Cl2(g) → PbCl4(l) ΔH = ? Pb(s) + 2Cl2(g) → PbCl4(l) ΔH = -329.2 kJ   Pb(s) + Cl2­(g) → PbCl2(s) ΔH = -359.4 kJ

Factors Affecting Equilibrium: Le Châtelier’s Principle Le Châtelier’s Principle (Henri Le Chatelier (1850-1936)) Stresses that upset the equilibrium of a chemical system include changes in the concentration of reactants or products changes in temperature changes in pressure Le Châtelier’s principle: If a stress is applied to a system in dynamic equilibrium, the system changes in a way that relieves the stress.

Equilibrium Constants Liquids & Solids are somewhat isolated. They are not included in the Keq equation. They are treated as a “1” value. Equilibrium Constants The equilibrium constant (Keq) is the ratio of product concentrations to reactant concentrations at equilibrium. aA + bB cC + dD From the general equation, each concentration is raised to a power equal to the number of moles of that substance in the balanced chemical equation. Keq = [C]c x [D]d [A]a x [B]b

Equilibrium Constants Write equilibrium constant expressions for the following reactions: Cl2(g) + I2(g)  2 ICl(g) 2HBr(g)  H2(g)+Br2(g)

Chemical Equilibrium Which of these equations represents a reaction in which entropy decreases? 2MgO(s) → 2Mg(s) + O2(g) 2O3(g) → 3O2(g) 2H2O(l) → 2H2(g) + O2(g) C(s) + 2H2(g)→ CH4(g) 2NI3(s) → 3I2(g) + N2(g)

Acids & Bases Classify each solution as acidic, basic, or neutral by its pH value.   [H+] = 7.5 x 10-12 M pH= _______ [H+] = 1.0 x 10-7 M pH= _______ pH = 12.0 pH= _______ pOH = 10.8 pH= _______ [OH-] = 2.8 x 10-5 M pH= _______ pH = 2.3 pH= _______

Acids & Bases Arrhenius acid Brønsted-Lowry acid Lewis acid Arrhenius base Brønsted-Lowry base This describes a substance that is a hydrogen-ion acceptor. This describes a substance that yields hydroxide ions in aqueous solution. This describes a substance that can accept a pair of electrons to form a covalent bond.

Strong Acid Dissociation Show how nitric acid will ionize or dissociation in water.

Ka dissociation A 0.10M solution of hydrocyanic acid, HCN, has an equilibrium hydrogen ion concentration of 6.3 × 10–6M. What is the Ka of hydrocyanic acid?

Potential diagrams What does this picture represent?