Chemistry 300 – First Semester Topic Review
1- Introduction & Matter
 Lab equipment and skills
 Safety
 Observing, collecting data and making conclusions
 What is matter?
 Mass vs. weight
 Three states of matter
o Solid, liquid, and gas basics
 Pure substances vs. mixtures
o Homogeneous vs. heterogeneous
o Elements, compounds, and mixtures
 Compounds vs. Mixtures
o Chemical combination vs. physical combination
 Separating matter
 Physical and chemical properties and changes
 Law of Conservation of Mass
 Intensive and extensive properties of matter
 Evidence of chemical change
o Color, odor, production of gas or solid, temperature
o Exothermic vs. endothermic reactions
 Introduction to the elements (symbols, groups/periods,
basic properties of metals, nonmetals, and metalloids and
location on Periodic Table)
2 - Measurement & Methods
 Scientific Method
o Hypothesis, etc.
o Qualitative vs quantitative data
o Variables – independent, dependent and controlled
 Measurements
 Graphing techniques
 Scientific Notation
 SI Units (metric prefixes)
 Significant Figures – (multiplication/division rules only)
 Temperature scales (converting between Celsius and Kelvin)
 Mass, volume, and density
 Uncertainty in measurement
o Accuracy vs. precision
o Percent error (experimental value – accepted
value)/(accepted value) x 100
3 - Atomic Structure
 History of development of models (Democritus, Dalton,
Thomson, Rutherford, Bohr)
 Structure of the atom
 Symbol, mass, charge and location for proton, neutron, and
electron
 Atomic number, atomic mass, mass number
 Determining number of protons, neutrons, and electrons
for atoms and ions
 Isotopes and weighted average atomic mass
 Ions – cations and anions and symbols
4 - Atomic Theory
 Basics of electromagnetic waves (light)
o Relationship between color of light and its energy
o Dual nature of light (waves and particles)
 Atomic emission spectra
 Bohr model of the atom
o Concept of ground and excited states for electrons
 Quantum mechanical model
o Heisenberg’s Uncertainty Principle and Schrodinger
o Atomic Orbitals vs. Orbits
 Electron configurations, orbital diagrams and noble gas
configurations
 Hund’s Rule, Pauli Exclusion Principal and Aufbau
Principle
 Isoelectronic species and ion formation
 Lewis Dot Diagrams
Periodic Table
 Periodic Table development: Mendeleev and Moseley
 Periodic Table: groups (family names), blocks, series, etc.
 Metals vs. nonmetals vs. metalloids
o Similarities and differences of chemical and physical
properties within and between groups.
 Periodic Table Trends: atomic radius, ionization energy,
electronegativity
o Net nuclear charge, shielding and shells
 Concept of valence electrons, Lewis dot structures for atoms,
and unpaired electrons and the Octet Rule.
6 - Ionic Compounds
 Bonds
o Attractive forces (chemical bonds all based on
attraction of protons and electrons)
o Types of bonding determines types of compounds:
 Ionic vs. covalent bonds (what happens to
electrons?)
 Ionic compounds vs. molecules (which types of
elements are involved?)
o Bond forming (energy released) and breaking (energy
must be absorbed). Exothermic vs. endothermic
 Ionic Compounds
o Creation by transfer of electrons from metals to nonmetals forming cations and anions
o Crystal lattices are strong structures
o Ionic compound properties
 Formula writing and naming for ions, ionic compounds
and diatomic elements
o Likely charges (based on valence electrons & group).
o Stock system and Latin naming for transition metals.
o Polyatomic ions
o Cross-over rule
 Balancing chemical equations using coefficients
 5 types of reactions (synthesis, decomposition, combustion,
single replacement, double replacement)
 Writing out symbolic equations given words
 Predicting products of reactions
 Activity Series - for Single Replacement Reactions
7 - Dimensional Analysis and the Mole
 Methodology for converting between units and problem
solving
 Memorize SI unit prefixes and base units.
 “Railroad Track” approach – let the units show the way!
 Mole concept and conversions (mass, moles, molecules,
atoms). Avogadro’s number (6.022 x 1023)
 Molar mass (gram formula mass)
 Converting between:
grams  moles  molecules  atoms or ions
 Percent composition
8 - Stoichiometry
 Empirical and molecular formulas
 Stoichiometry (using mole ratios from balanced reactions)
o Calculate of quantities of reactants and products in
chemical reactions using molar relationships
 Limiting reactants
 Percent yield
Note: It will help you greatly if you have the following items solidly
implanted in your brain: the chemical symbols of the elements,
charges based on locations on the Periodic Table, how to name all
types of ions, polyatomic ion names and formulas (“Nick the
Camel…”, how to recognize and name and write formulas for
ionic compound, metric prefixes for unit conversions, Avogadro’s
number, how to recognize the 5 different types of reactions, the
periodic trends (for shielding, shells, net nuclear charge, atomic
radius, ionization energy, and electronegativity) and why they
occur, the diagonal spdf pattern for determining electron
configurations, any important equations/formulas (ex: density,
converting Celsius to Kelvin, etc.), how to recognize atomic
number and atomic mass on ANY Periodic Table… just a few
suggestions.