HONORS CHEMISTRY: FINAL EXAM STUDY GUIDE



HONORS CHEMISTRY: FINAL EXAM STUDY GUIDE

• The final exam will consist of 80 Multiple Choice questions and 2 open-end questions. The outline provided below describes the major topics and units that will be covered on the multiple choice section of the final exam:

UNIT6: “Gases and Gas Law Relationships ( ~ 10 questions)

- Gases vs. Liquids vs. Solids: Properties and Behavior

- Pressure and Volume: Boyle’s Law

- Temperature and Volume: Charles’ Law

- The Combined Gas Law

- Moles and The Ideal Gas Law Equation

- Avogadro’s Law, Dalton’s Law of Partial Pressure, Graham’s Law

UNIT 7: “Chemical Bonding and Molecular Geometry” ( ~ 20 questions)

- Ionic, Covalent and Metallic Bonding: Definitions, Models and Properties

- Using Dot Diagrams to draw Lewis bond structures

- Polar vs. Non-Polar Bonding and Electronegativity Difference

- Isomers and Resonance

- VSEPR Theory, Facts, and Examples

- ABE Formulas, Bond Length and Bond Angles, Molecule Shapes

- Bond Hybridization Basics

- Intermolecular Forces including Hydrogen Bonding

UNIT 8: “Thermodynamics and Kinetics” ( ~ 20 questions)

- Definitions of Energy, Enthalpy, Entropy

- Exothermic vs. Endothermic Changes

- Hess’s Law Calculations and Interpretation

- Entropy Analysis and Factors Affecting Entropy Change

- Gibbs Free Energy Calculations and Interpretation

- Rate-Influencing Factors and Collision Theory

- Determining Rate Order and Solving Rate Law Expressions

- Reaction Mechanisms

- Catalysts and Energy/Rate Graphical Analysis

UNIT 9: “Chemical Equilibrium and Acid-Base Chemistry” ( ~ 20 questions)

- Reversible Reactions, Chemical Equilibrium

- Equilibrium Constants and Expression + Problem Solving

- LeChatelier’s Principle and Factors affecting equilibrium

- Reaction Quotient: Q vs. K – Problem Solving and Analysis

- Common properties and uses of acids and bases

- Arrhenius, Bronsted-Lowry, and Lewis models +examples

- Conjugate acids and bases

- pH: Background, Facts, Examples, + Calculations

- Titrations: Equipment, Goal, Procedure, Problem Solving, Chemical Indicators

- Weak vs. Strong acids and bases, Equilibrium of Weak Acid Solutions (Ka)

- Acid Rain Connections + Acids and Bases in the Human Body

UNIT10: “Introduction to Organic Chemistry” ( ~10 questions)

- Hydrocarbon groups: Alkanes, Alkenes, and Alkynes

- Organic Chemistry Vocabulary: Isomers, Saturation, Aromatics, etc…

- Fundamental nomenclature rules for organic molecules

- Recognition of Functional Groups (Structures and Names)

- Organic Reaction Types

- Polymers and Polymerization

- Organic Molecules in Biochemistry

The best way to study for the final exam is to read through your notes and text, and work with your UNIT QUIZZES. The multiple choice questions on the final exam will definitely include questions that are very similar to the same questions used on unit quizzes. Use this study guide as a checklist, especially to address your individual weakness areas.

You will also receive a study guide to help you prepare for the 2 open-ended questions on the final exam. You will be provided with approximately 8 potential final exam open-ended questions. The nature and difficulty of these practice problems will be very similar to the real questions chosen for each exam. By completing these problems in advance you will be very prepared to face similar questions on the open-ended section of the final exam

Good Luck with your studying! Please see me with any concerns or questions you may have.

FINAL EXAM PREPARATION

• Your final exam will include 80 multiple choice questions and 2 open-ended questions. The 2 open-ended questions on the exam will be very similar to the questions included in the short list below. As a result, you can really help yourself in preparing for the final exam by working through these problems in advance of the test!

1. UNIT 7 – Chemical Bonding Basics:

“For the three compounds below, first identify which is ionic, which is polar covalent and which is non-polar covalent. Next, use definitions and knowledge bond types and forces to discuss how each pure substance would respond to being mixed with pure water.”

MgCl2 (S) C6H14 (l) NH3 (l)

2. UNIT 7 – Molecular Geometry / VSEPR:

“ When the element sulfur reacts with a high concentration of fluorine gas, an expanded octet molecule can form. Use your knowledge of the valence electrons of these two non-metals to draw a structural formula for the product molecule. Also, indicate the shape name and the bond angle separation and the bond hybridization for this product molecule”

S + F2 → ?

3. UNIT 7 – Intermolecular Forces:

“ Despite having very similar formulas and molar mass values, Ethane is a gas at room temperature but Ethanol is a liquid. Explain this fact in terms of the intermolecular forces and density”

Ethane: C2H6 vs. Ethanol: C2H5OH

4. UNIT 8 – Thermodynamics:

“Define enthalpy and entropy and then use the data and reaction with the Gibbs free energy equation to discuss whether or not the spontaneity of the decomposition reaction below would be affected by changes in reaction temperature”.

2 KClO3 (s) → 2 KCl (s) + 3 O2 (g)

ΔH = -77.6 kJ

5. UNIT 8 – Kinetics:

“Define activation energy and discuss how temperature changes can influence rates of reactions in terms of activation energy and collision theory. Also, create a sketch of an energy diagram curve for a 2-step reaction mechanism in which step 1 is an endothermic rate-determining step and step 2 is an exothermic step”

6. UNIT 9 – Chemical Equilibrium:

“Write an equilibrium (Kp) expression for the reversible reaction below. Then calculate the Kp value from the provided equilibrium pressure data. Finally, explain how this equilibrium system would respond or “shift” if the concentration of HCl was decreased by separating and pumping out the reactant gas”

2 HCl (g) ↔ 1 H2 (g) + 1 Cl2 (g)

Equilibrium Pressure Data: PHCl = 0.55 atm PH2 = 1.1 atm PCl2 = 1.1 atm

7. UNIT 9 – The pH Scale

“Write a brief essay on the pH scale. Be sure to clearly describe what the hydronium ion is and also be sure to communicate the role of the self-ionization of water molecules at 25 ˚C as the basis of the 0-14 pH scale. Also, calculate the pH of a 0.250 M solution of potassium hydroxide”

8. UNIT 9 – Acid-Base Reactions

“Explain the difference between weak and strong acids using definitions and examples. Also, if a 25.0 mL sample of 2.0 M HNO3 solution was titrated with 1.0 M NaOH solution how many milliliters of the base would be required to reach the equivalence point? Support with mathematical evidence and explain”

9. UNIT 10 – Organic Chemistry Question

“The chemical C3H8O has three structural isomers. Neatly draw the structural diagram for each isomer, identify functional groups, and also name each isomer”

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