General Chemistry Final Exam Study Guide: Structure, Reactions, Thermochemistry, Bonding, and States of Matter

Unit 1: Atomic Structure

Characteristics of Matter

• Atomic structure includes subatomic particles: protons, neutrons, electrons, symbols, and charge.

• Atoms are the basic units of matter, each with a unique number of protons (atomic number).

Properties of Elements and Periodic Table

• Understand the differences between the properties of atoms, isotopes, and ions.

• Isotopes are atoms of the same element with different numbers of neutrons.

• Ions are atoms or molecules that have gained or lost electrons, resulting in a net charge.

• Use the periodic table to quickly identify atomic number and mass number.

• Predict properties and trends (e.g., atomic radius, ionization energy, electronegativity) using periodic table position.

Phenomena Interpretation

• Interpret physical and chemical phenomena using atomic and molecular structure.

Unit 2: Reactions and Stoichiometry

Naming Compounds and Writing Formulas

• Write the formula of an ionic compound from the name or vice versa.

• Identify the amount of each atom in a compound from its formula.

Stoichiometry and Chemical Equations

• Balance chemical equations to obey the law of conservation of mass.

• Use stoichiometry to relate quantities of reactants and products in chemical reactions.

• Apply the concepts of limiting reactant, percent yield, and theoretical yield.

• Use mole relationships and conversion factors (mole-mass, mole-volume, Avogadro's number).

• Interpret and use solubility rules and ICE tables (Initial, Change, Equilibrium) for reaction calculations.

Unit 3: Thermochemistry

Key Concepts

• Understand heat, temperature, enthalpy change, exothermic and endothermic reactions, calorimetry, and specific heat.

• Calculate the heat change for a reaction using calorimetry data.

Enthalpy and Heats of Formation

• Use Hess's Law to determine the enthalpy change for a reaction from the enthalpy changes of multiple steps.

• Calculate the enthalpy change for a reaction using standard enthalpies of formation:

$\Delta H_{rxn} = \sum n_p \Delta H_f^{\circ} (\text{products}) - \sum n_r \Delta H_f^{\circ} (\text{reactants})$

• Understand the difference between heat of formation and other enthalpy terms (such as heat of combustion).

• Write equations for formation reactions.

Unit 4: Bonding

Types of Bonding

• Identify the type of bonding (ionic, covalent, metallic) present in a compound.

Lewis Structures and Molecular Geometry

• Draw the Lewis structure for a compound given its formula.

• Determine electron pair and molecular geometry using VSEPR theory.

• Predict bond angles and molecular polarity.

Bonding Details

• Describe the hybridization of an atom and the number of sigma and pi bonds in a molecule.

• Explain differences in bond length and bond strength based on bond order.

• Calculate the energy change for a reaction using bond energies:

$\Delta H = \sum \text{(Bond energies of bonds broken)} - \sum \text{(Bond energies of bonds formed)}$

Unit 5: Gases, Liquids, and Solids

States of Matter and Intermolecular Forces

• Identify different types of solids based on their formulas and the types of interparticle forces present.

• Rationalize differences in boiling points, melting points, vapor pressure, and heat of vaporization based on intermolecular forces (e.g., London dispersion, dipole-dipole, hydrogen bonding).

• Relate state of matter to energy, temperature, and pressure changes.

Applications and Properties

• Answer questions about laboratory techniques (e.g., chromatography, distillation).

• Understand the properties of conductors, semiconductors, and insulators.

• Describe band gap, n-type, and p-type semiconductors.