Kinetics PPT on mastering chemistry

Set1: Ch14 Q31,35,36,39,45 (p.664-665)

Set2: Ch14 Q53,59,73,75,95,120 (p.666-667)

Half Life Lab

Kinetics Test

list the factors that influence the rate of a chemical reaction.

use experimental data to determine the rate law, determine the order of the reaction, and to define proper units for the constant.

compare and contrast zero, first, and second order reactions in terms of the plot needed to give a straight line, the relationship of the rate constant to the slope of the straight line, and the half-life of the reaction.

use experimental data to postulate a reaction mechanism.

interpret how changing the conditions of the reaction (i.e., temperature, pressure, concentration, and addition of a catalyst) affects both the rate and the rate constant of the reaction.

discuss the role of a catalyst in the rate and mechanism of a reaction; distinguish between a homogeneous and a heterogeneous catalyst.

interpret data from a first order reaction to determine its half-life.

use kinetics to make calculations regarding half-life.

solve problems involving activation energy and the Arrhenius equation.

create and analyze an energy vs reaction coordinate plot, using it with collision theory to explain the kinetics of a reaction.

write nuclear reactions using the of charge and mass number.

Understand the three major types of decay discussed.

explain the concept of carbon-dating.

compare and contrast fission and fusion

Read Ch. 15 and Ch 19 (sec 7-How Gibbs Free Energy relates to Equilibrium)

Read about Solubility Constant (Ksp)-Ch 17 Sec 4-7

Test on Chemical Equilibrium & Solubility Product Constant

• describe the meaning of physical and chemical equilibrium, and give real life examples of each.
• write the law of mass action for any system at equilibrium.
• Understand the meaning of equilibrium constant and reaction quotient (Q).
• interpret the position of equilibrium from the size of the equilibrium constant.
• use Le Chatelier’s principle to predict the direction a system in equilibrium will shift in order to re-establish equilibrium.
• understand that temperature, pressure, and concentration will shift the position of equilibrium.
• Understand that a catalyst will not have an effect of the equilibrium constant.
• write solubility product expressions for slightly soluble compounds.
• solve problems involving: (a) solubility product constants from solubility; (b) molar solubility from Ksp; (c) concentrations of substances necessary to produce a precipitate; (d) concentrations of ions involved in simultaneous equilibrium.

Ch 16 Sec 1-7

Readings from Tro-A/B pH box Ionic Equilibria Acids and Bases Mixture of Acids, Bases, & Polyprotic acids (fill in) When the Assumption fails Acid/Base Problems refresher

The RainBow Lab

Acid/Base Ionic Equilibria Assessment

• distinguish between the various modern theories of acids and bases.
• name and write formulas for normal salts, hydrogen salts, hydroxy salts, oxysalts, and acids.
• write balanced equations for hydration reactions involving acids, bases, and salts.
• use the concept of conjugate acid-base pairs to predict reaction products.
• define and give examples of amphoteric species.
• list the six strong acids.
• determine the pH of acid/base/salt solutions.

Ch 16 Sec 8-12 & Ch 17 Sec 1-4

Ch16 Sec 8-11 Notes: Strengths & Properties of Acids & Lewis Acid Strength Reference Buffer Notes Titration Graphs How to solve ANY kind of ionic equilibria problem

Set 1: Q96,97,99,102,105 (p.773)

Salt Hydrolysis (Ch 16 Sec8-11) Assessment

Titration and Buffer Assessment

• perform a titration and solve for the appropriate concentration.
• use the concept of conjugate acid-base pairs to predict reaction products.
• define and give examples of amphoteric species.
• determine the concentrations of all species in acid/base/salt solutions.
• determine the pH of acid/base/salt solutions.
• Recognize Lewis acid-base reactions.
• pick a suitable indicator for a titration.
• Given the concentration and amount of weak acids or bases and an appropriate titrant, calculate data to produce a titration curve.

Ch 7&8

Atomic Structure and Periodicity Assessment

• solve problems regarding the characteristics of electromagnetic radiation.
• explain the emission and absorption of photons by electrons moving between energy levels and calculate the wavelengths of the photons.
• make predictions regarding electron configurations.
• explain element physical and chemical properties using electronic structure.
• use electronic structure to predict and explain trends and exceptions of the above characteristics on the periodic table.
• define the following: central ion or atom
• ligand, cis and trans isomers (organic), % transmittance, Absorbance, Beer’s law, spectrometer.

Ch 9 and 10

Half Life Lab

Bonding Test

• determine types of bonding in compounds.
• use bonding to explain physical and chemical characteristics.
• calculate changes in enthalpy of reactions using bond energies.
• use lewis structures and the VSEPR Model to predict shapes and physical and chemical properties of covalent molecules.
• use hybridization to explain the geometric shapes of covalent molecules.
• identify the hybridization of molecules.

Intermolecular Forces Quiz

• identify important forces between particles of any element or compound.
• use interparticle forces to explain physical properties of elements or compounds.
• calculate changes in enthalpy during state changes using heats of formation and calorimetry.
• analyze phase diagrams for pertinent information.
• synthesize phase diagrams given information about a substance.

Ch 25

Alkane WS

Alkene/Alkyne WS

Organic Halide WS

Cyclic WS & Aromatic WS

Intro to Derivatives WS

Level 1 and Levels 2/3 WS

• name a variety of organic molecules.
• write simple reactions as listed above.
• predict structural isomers of organic molecules.