General Chemistry II: Syllabus, Success Strategies, and Properties of Solutions (Ch. 13.1)

Course Introduction and Syllabus Overview

Course Structure and Communication

• Course: CHEM 1220 – General Chemistry 2 (Spring 2025)

• Instructor: Prof. Zadrozny (contact via Carmen email preferred; include [CHEM1220] in subject line)

• Office Hours: Fridays 10am–12pm, Learning Resource Center (Celeste 170)

• Important Contacts: General, exam, lab, and SLDS emails provided for specific inquiries

Assignments and Grading

• Quizzes: Mandatory, including an Academic Misconduct Quiz (must score 100%)

• Recitations: Weekly, with group activities and a short graded quiz (10 total, 1 drop allowed)

• Homework: Two per week (short and long), open until the end of the semester, no late penalties

• Exams: Four midterms (Ch. 13–21) and a cumulative final; exams are 60% of the total grade

• Laboratory: 20% of the total grade

Assignment Group	% of Grade
Mandatory Quizzes	5%
Recitation	10%
Online Homework	10%
Exam 1	10%
Exam 2	10%
Exam 3	10%
Exam 4	10%
Final Exam	15%
Laboratory	20%

Keys to Success

• Read assigned sections before class

• Attend and participate in lectures and recitations

• Practice problems from the textbook and MasteringChemistry

• Seek help early (office hours, TAs, study groups)

• Keep a dedicated notebook for problem-solving and review

• "Genius is 1% inspiration, 99% perspiration" – consistent effort is crucial

Course Content and Learning Objectives

Major Topics Covered

• Ch. 13: Properties of Solutions

• Ch. 14: Chemical Kinetics

• Ch. 15: Chemical Equilibrium

• Ch. 16: Acid-Base Equilibria

• Ch. 17: Additional Aspects of Aqueous Equilibria

• Ch. 19: Chemical Thermodynamics

• Ch. 20: Electrochemistry

• Ch. 21: Nuclear Chemistry

Learning Objectives

• Understand basic facts, principles, theories, and methods of modern science

• Recognize science as an evolving body of knowledge

• Describe the interdependence of science and technology

• Recognize social and philosophical implications of scientific discoveries

Review and Foundational Concepts

Essential Topics to Review

• Predicting molecular structure (Ch. 8, 9)

• Calculating formula weights (Ch. 1, 2)

• Balancing chemical reactions (Ch. 3, 4)

• Enthalpy and Hess’s Law (Ch. 5)

• Intermolecular interactions (Ch. 11)

• Mathematical skills: quadratic equation and algebraic manipulation

Hess’s Law and Enthalpy Calculations

Hess’s Law states that the total enthalpy change for a reaction is the sum of the enthalpy changes for each step, regardless of the pathway.

• Example: Combustion of methane

$\text{CH}_4(g) + 2\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{H}_2O(l)$ $\Delta H = -890\ \text{kJ}$

If you reverse a reaction, change the sign of $\Delta H$.

Intermolecular Forces in Solutions

Intermolecular forces determine the physical properties of substances and their behavior in solution.

Type of Force	Occurs Between	Relative Strength
Dispersion (London)	All molecules, especially nonpolar	Weakest
Dipole-dipole	Polar molecules	Intermediate
Hydrogen bonding	Polar molecules with O-H, N-H, or F-H	Strong
Ion-dipole	Ions and polar molecules	Strongest

Chapter 13.1: Properties of Solutions

What are Solutions?

• Solution: A homogeneous mixture of two or more substances

• Solute: The minority component (dissolved)

• Solvent: The majority component (does the dissolving)

• Examples: Solid solution (14K gold), liquid solution (whiskey), gaseous solution (air)

Solution Formation as a Spontaneous Process

• Spontaneous process: Occurs without external input; "just goes" under a given set of conditions

• Spontaneous processes favor an increase in entropy (disorder, higher degrees of freedom)

Enthalpy ($\Delta H$) Considerations for Solution Formation

• To separate molecules, energy must be added: $\Delta H > 0$ (endothermic)

• Bringing molecules together releases energy: $\Delta H < 0$ (exothermic)

Enthalpy of Solution Formation

• The enthalpy change for solution formation is the sum of three steps:

$\Delta H_{\text{solution}} = \Delta H_{\text{solvent}} + \Delta H_{\text{solute}} + \Delta H_{\text{mix}}$

• Endothermic process: $\Delta H_{\text{solution}} > 0$, absorbs heat

• Exothermic process: $\Delta H_{\text{solution}} < 0$, releases heat

• For ionic solids dissolving in water, $\Delta H_{\text{mix}}$ is often the largest negative term

Practice Example

• For the dissolution of LiCl in water, $\Delta H_{\text{solution}} = -37$ kJ/mol. The largest negative term is $\Delta H_{\text{mix}}$ (mixing of ions and water molecules).

Practice Problem: Hydrogen Bonding

• Which solvent exhibits hydrogen bonding? Ethanolamine (contains O-H and N-H groups)

Summary Table: Intermolecular Forces

Force	Occurs In	Relative Strength
Dispersion	All molecules	Weak
Dipole-dipole	Polar molecules	Moderate
Hydrogen bonding	Polar molecules with O-H, N-H, F-H	Strong
Ion-dipole	Ions in polar solvents	Very strong

Additional info:

• Students are encouraged to use AI tools to generate practice problems and to keep a problem-solving notebook for effective review.

• Developing a good relationship with instructors and TAs is important for future recommendation letters.