General Chemistry I Final Exam Study Guide and Worksheet

General Chemistry I Final Exam Study Guide

Overview

This study guide covers essential topics and equations for a General Chemistry I final exam, including physical and chemical changes, atomic structure, chemical reactions, solutions, gases, thermochemistry, quantum mechanics, periodic properties, and chemical bonding. The worksheet provides practice problems to reinforce these concepts.

Chapter 1: Matter, Measurement & Problem Solving

Physical and Chemical Changes

• Physical Change: A change that does not alter the chemical composition of a substance (e.g., melting, boiling).

• Chemical Change: A change that results in the formation of new substances (e.g., combustion, oxidation).

• Example: Dissolving salt in water is a physical change; burning magnesium is a chemical change.

Chapter 2: Atoms & Elements

Subatomic Particles

• Protons: Positively charged particles in the nucleus.

• Neutrons: Neutral particles in the nucleus.

• Electrons: Negatively charged particles orbiting the nucleus.

• Atomic Mass: The weighted average mass of an element's atoms, considering isotopic abundance.

• Isotopes: Atoms of the same element with different numbers of neutrons.

• Example: Chlorine has isotopes Cl-35 and Cl-37.

Chapter 3: Molecules and Compounds

Empirical and Molecular Formulas

• Empirical Formula: The simplest whole-number ratio of atoms in a compound.

• Molecular Formula: The actual number of atoms of each element in a molecule.

• Example: Glucose has empirical formula CH2O and molecular formula C6H12O6.

Chapter 4: Chemical Reactions and Chemical Quantities

Stoichiometry

• Balancing Chemical Equations: Ensures the same number of atoms of each element on both sides of the equation.

• Limiting Reactant: The reactant that is completely consumed first, limiting the amount of product formed.

• Theoretical Yield: The maximum amount of product that can be formed from the limiting reactant.

• Percent Yield: $\text{Percent Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\%$

Chapter 5 & 14: Solutions and Aqueous Solutions

Concentration and Molarity

• Molarity (M): $M = \frac{\text{moles solute}}{\text{L of solution}}$

• Dilution Equation: $M_1V_1 = M_2V_2$

• Example: To dilute 1.0 M solution to 0.5 M, use twice the final volume.

Chapter 6: Gases

Gas Laws

• Ideal Gas Law: $PV = nRT$

• Combined Gas Law: $\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$

• Variables: P = pressure, V = volume, n = moles, R = gas constant, T = temperature (K).

• Example: Calculate the pressure of a gas sample at different temperatures and volumes.

Chapter 7: Thermochemistry

Energy and Heat

• First Law of Thermodynamics: $\Delta E = q + w$ (change in internal energy equals heat plus work)

• Heat Transfer: $q = m \times C_s \times \Delta T$ (mass × specific heat × temperature change)

• Example: Calculate heat absorbed by water when heated.

Chapter 8: The Quantum-Mechanical Model of the Atom

Light and Energy

• Speed of Light: $c = \lambda \nu$ (wavelength × frequency)

• Energy of a Photon: $E = h \nu$ (Planck's constant × frequency)

• Example: Calculate energy of light with a given wavelength.

Chapter 9: Periodic Properties of the Elements

Periodic Trends

• Atomic Radius: Decreases across a period, increases down a group.

• Ionization Energy: Increases across a period, decreases down a group.

• Electronegativity: Tendency of an atom to attract electrons in a bond.

Chapter 10 & 11: Chemical Bonding I & II

Lewis Structures and Molecular Geometry

• Lewis Structure: Diagram showing valence electrons and bonds in a molecule.

• Hybridization: Mixing of atomic orbitals to form new hybrid orbitals (e.g., sp, sp2, sp3).

• Molecular Geometry: Shape of a molecule determined by VSEPR theory (e.g., linear, trigonal planar, tetrahedral).

• Example: NO3- has trigonal planar geometry.

Important Equations to Remember

• $M = \frac{\text{moles solute}}{\text{L solution}}$

• $M_1V_1 = M_2V_2$

• $PV_1 = P_2V_2$

• $PV = nRT$

• $\Delta E = q + w$

• $q = m \times C_s \times \Delta T$

• $c = \lambda \nu$

• $E = h \nu$

• $c = 3.0 \times 10^8$ m/s

Practice Worksheet Problems

Sample Problems and Solutions

• Isotope Calculations: Calculate average atomic mass using isotopic abundances.

• Energy of Light: Use $E = \frac{hc}{\lambda}$ to find energy of photons.

• Empirical Formula: Determine simplest ratio from percent composition.

• Gas Law Applications: Calculate pressure, volume, or temperature changes using $PV = nRT$ and related equations.

• Thermochemistry: Calculate heat transfer and specific heat capacity.

• Lewis Structures: Draw structures, determine hybridization and geometry.

• Limiting Reactant and Percent Yield: Identify limiting reactant, calculate theoretical and percent yield.

• Boiling Point and Vapor Pressure: Compare compounds based on intermolecular forces.

• Average Speed of Gas Molecules: Predict based on molar mass.

Sample Table: Key Equations and Their Applications

Equation	Application
$M = \frac{\text{moles solute}}{\text{L solution}}$	Calculating solution concentration
$PV = nRT$	Relating pressure, volume, temperature, and moles of a gas
$q = m \times C_s \times \Delta T$	Calculating heat transfer
$E = h \nu$	Calculating energy of a photon
$M_1V_1 = M_2V_2$	Dilution of solutions

Additional info:

• Constants such as the speed of light ($c = 3.0 \times 10^8$ m/s) and Planck's constant ($h$) will be provided on the exam.

• Students should be familiar with all chapter core materials, including lab techniques and mathematical operations.