ADVANCED CHEMISTRY SAT2 MATERIAL

PACKET #1: MATH & LAB SKILLS Dimensional Analysis

Questions:

How many miles are equivalent to 5025 inches?

How many ounces are equivalent to 0.234 kg?

How many yards are equivalent to 2016 mm?

PACKET #2: ENERGY & THERMODYNAMICS Gibb’s Free Energy Hess’s Law Heating/Cooling Curve over multiple segments Triple Phase Diagram

Gibb’s Free Energy

Questions

Hess’s Law:

Question:

Question:

Heating/Cooling Curve (multiple segments): How much heat energy is absorbed as 10.0g water is heated from -40.°C until it is

vaporized at its boiling point (specific heat capacity of water ice = 2.11 J/g°C)?

Triple Point Phase Diagram:

Remember that sublimation and deposition are represented on the Triple Phase Diagram and that the triple point is the point at which all three phases exist at equilibrium under specific conditions of temperature and pressure.

PACKET #3 – ATOMIC CONCEPTS Orbitals (sublevels)

PACKET #5: NOMENCLATURE

Latin Prefixes – higher oxidation state (-ic), lower oxidation state (-ous) Antimony (Sb) – stibium Coppor (Cu) – cuprum Gold (Au) – aurum Iron (Fe) – ferrum Mercury (Hg) – hydrargyrum or mercurous/ic Lead (Pb) – plumbum Potassium (K) – kallium Silver (Ag) – argentum Sodium (Na) – natrium Tin (Sn) - stannum Tungsten (W) - wolfrum

PACKET #6: MOLES & STOICHIOMETRY Limiting Reactant – for each of the following reaction do the following:

Balance the reaction Name the type of reaction Determine the limiting reactant/reactant in excess Determine the maximum amount of product underlined Determine the amount of reactant in excess used Determine the amount of reactant in excess remains

1.

2.

PACKET #7 – BONDING VSPER Model Hybrid Orbitals

PACKET #8 – GAS LAWS Ideal Gas Law Dalton’s Law of Partial Pressure

Ideal Gas Law:

PV = nRT (R = 0.0821 atm.L/mol.K)

Questions:

Dalton’s Law of Partial Pressure:

PACKET #9 – SOLUTIONS Molality Molarity by Dilution Colligative Properties

Questions:

Questions:

Colligative Properties:

(Kb = +0.513 °C/m and Kf = -1.86 °C/m)

Questions:

ACIDS, BASES, AND SALTS Conjugate Acid/Base Pairs Lewis Acids/Bases Hydrolysis of Salts

Identify the conjugate acid/base pairs in the reactions below: HOCl (aq) + H2O (l) OCl- (aq) + H3O+ (aq) NH3 (aq) + HSO4- (aq) NH4+ (aq) + SO42- (aq) Lewis Acid: Lewis Base:

Lewis acids and bases combine through coordinate covalent bonds with each other. HYDROLYSIS OF SALTS Strong Acids: Stong Bases: Strong acid + strong base water + _______________________ salt Strong acid + weak base water + _______________________ salt Weak acid + strong base water + ________________________ salt Weak acid + weak base water + ____________________________ salt

KINETICS AND EQUILIBRIUM Reaction Mechanisms Equilibrium Constant

REACTION MECHANISMS Rate Determining Step: Question: Given a potential mechanism below, answer the following questions. Step 1: NO2 + NO2 NO3 + NO (slow)

Step 2: NO3 + CO NO2 + CO2 (fast)

How will increasing the concentration of NO2 affect the rate of the reaction? Why?

How will increasing the concentration of CO affect the rate of the reaction? Why?

What is the net chemical equation for the reaction show above?

Identify an intermediate in the mechanism above. Justify your answer. EQUILIBRIUM CONSTANT Given the general reaction: mA + nB ↔ pC + qD where m, n, p, and q are numerical coefficients representing moles of A, B, C, and D. All equilibrium equations have a mass action expression in the form: Keq = [C]p [D]q [A]m [B]n

Significance of Keq: K < 1

K > 1 Ka—Acid Dissociation Constant Kb—Base Dissociation Constant Kw—Autoionization of Water Constant Ksp—Solubility Product Constant

REDOX/ELECTROCHEMISTRY Determining Cell Potential, E°cell

If the cell potential for a reaction is positive, the reaction will be ______________________________. If the cell potential for a reaction is negative, the reaction will be _____________________________. If the cell potential for a reaction is zero, the reaction will ____________________________________. What will be the sign of G° in the above scenarios? Question: Fe

3+(aq) + Cu(s) → Cu

2+(aq) + Fe

2+(aq)

Calculate E °cell for this reaction. Is the reaction spontaneous?

Question: Given the Voltaic cell below, answer the questions that follow. Each electrode is in a

nitrate solution with its own cation.

Identify the anode and cathode. Justify your decision. Indicate the direction of electron flow through the wire. Which electrode is the site of oxidation? Which electrode is the site of reduction? What is the oxidizing agent in the reaction above? What is the reducing agent in the reaction above? Which electrode decreases in size as the reaction progresses? Which electrode increases in size as the reaction progresses? What is the purpose of the salt bridge? Indicate the direction of ion flow through the cell. Write half reactions for each half cell. Write a balanced chemical equation for the Voltaic cell. Determine the standard cell potential, E°cell, for the reaction represented above.

ORGANIC CHEMISTRY Cyclic hydrocarbons

General Formula for Cyclic Hydrocarbons:

Aromatic hydrocarbons

General Formula for Aromatic Hydrocarbons:

NUCLEAR CHEMISTRY Parts of a nuclear reactor

Fuel rods:

Shielding:

Moderators:

Control rods:

Coolant: