Dr. K's Complete First Semester General Chemistry I Course

Definition of Chemistry, introduction to symbols for the elements and mnemonics for the common elements.  Flash card videos included in the resource folder to drill the symbols of the elements.

The Scientific Method explained.  Definitions of terms.  Example of Phlogiston.

Matter, mass, weight, mixtures, pure substances, elements and chemical compounds discussed.  Introduction to chemical formulas.

Difference between physical and chemical properties and changes discussed.  Intensive and extensive properties discussed.

Measurement defined.  Discussion of expressing numbers in ordinary and scientific notation.  Section One In-Class Problems are in the Resource folder for this lecture.

Metric and SI base units explained.  Prefixes used with the metric system are introduced.

Length, mass, volume and temperature measurements discussed. 

Errors made in measurements discussed.  Accuracy and precision defined.  How measurements determine the number of significant figures in the measurement.

Rules for identifying the number of significant figures in a measurement.  Exact numbers defined.  Rules for rounding calculations to the correct number of significant figures.

Introduction to using dimensional analysis for calculations.  Method for obtaining conversion factors discussed. 

Introduction of density as a physical property.  Use of compound units as conversion factors introduced.

Brief history of the atom.  Dalton's Atomic Theory, Laws of mass conservation, Definite Proportion and Multiple Proportion discussed. 

Brief historical discussion of the atom and the discovery of the sub-atomic particles: proton, neutron and the electron.

Discussion of subatomic particles, chemical elements defined, atomic and mass numbers introduced and their relation to the periodic table.  Atomic Notation and isotopes introduced.  In-Class problems for Section 2 given in the Resources folder.

Atomic Mass Unit (amu) defined.  Atomic weights of the elements discussed.  Use of isotopes in calculating average atomic weights.

Detailed discussion of chemical formulas, elements that exist as diatomic molecules, use of parentheses in chemical formulas.

Power point presentation of the periodic table.  Discussion includes identification of main group, transition and inner-transition elements, distinction of metals, non-metals and semi-metals.  Group names introduced.  Properties of metals, non-metals and semi-metals given.

Distinction between molecular and ionic compounds introduced.  Ions, cations and anions defined.  Formation of ionic compounds from ions discussed.  Method for identifying charge of main group element ions using the periodic table.

Naming of monatomic cations and anions.  Introduction to the use of Roman Numerals with the naming of transition metal cations.   Flash card videos for drilling monatomic ions are given in the Resources folder.

Memory aids for remembering the charges of transition metal ions.

Chemical formulas and charges given for polyatomic ions.  Rules for naming ions given.  Memory aids for remembering the formulas and charges of the polyatomic anions given.  Flash card videos for drilling polyatomic anions are given in the Resources folder.

Rules for naming ionic compounds explained.  Flash card videos for drilling ionic compound nomenclature are given in the Resources folder.

Rules for naming binary and ternary acids explained.  Flash card videos for drilling acid nomenclature are given in the Resources folder.

Rules for naming binary molecular compounds explained.  Greek numerical prefixes given.

Calculation of formula weight (molecular weight) of chemical compounds explained.  In-Class problems for this Section given in the Resources folder.

The mole concept explained and molar mass of chemical compounds introduced.  The use of molar mass as a conversion factor is explained.

Avogadro's Number introduced with respect to the mole concept.  The use of Avogadro's Number as a conversion factor is explained.

Relationship between moles of atoms in one mole of a chemical compound explained.

Mass percent of elements in a chemical compound are explained and calculated.

The empirical and molecular formulas of chemical compounds are determined from the mass percent of each element in the compound.

Introduction to solutions:  terms defined,

The solution concentration of molarity is introduced and discussed.  Use of molarity as a conversion factor explained.

Procedure given for the diluting of solutions.

Mass percent as a concentration unit discussed.  The units of parts per million (ppm) and parts per billion (ppb) also discussed.

Identifying the parts of a chemical equation.  Learning to balance chemical equations by inspection.  The In-Class problems for Section 4 are given in the Resources folder for this lecture.

Electrolytes and non-electrolytes defined.  Dissociation reaction introduced.

Procedure for writing and balancing molecular, ionic and net ionic equations is discussed.

Arrhenius and Bronsted-Lowry acids and bases are defined and their chemistry is discussed.  Ionization reactions are introduced.  Acid and base anhydrides are explained. 

The distinction between strong and weak acids and bases is discussed.

Metathesis reactions are defined and driving forces identified.  Solubility rules for ionic compounds introduced.  Writing and balancing molecular, ionic and net ionic equations for metathesis reactions explained.

Introduction to oxidation and reduction.  Oxidizing and reducing agents defined.

Oxidation numbers are defined and rules for assigning oxidation numbers to atoms in compounds or polyatomic ions are explained.  Multiple examples are given.

Procedure using the half-reaction method for balancing redox reactions in acid solution is explained.

Procedure using the half-reaction method for balancing redox reactions in basic solution is explained.

The three types of redox reactions involving metals (Single Replacement Reactions) is discussed.  The Activity Series is explained.

Mole-mole calculations are now applied to stoichiometric calculations in a balanced chemical equation.

Mass-mass stoichiometric calculations are discussed.  The embedded mole-mole conversions become known as the "Molar Highway."

The concept of limiting reactant is introduced.  Determining which reactant is the limiting reactant and which one is in excess is explained.

Theoretical yield, actual yield and percent yield for a given chemical reaction is explained.

Stoichiometric calculations used in Lectures 46 - 48 are applied to reactions carried out in aqueous solutions.

A lab technique used to determine the molarity of an acid or base is explained.

Combustion reaction is defined.  Lecture explains how combustion analysis can be used to determine the empirical or molecular formula of an un known compound.  (refer to Lecture 30)

Energy is defined and discussed.  The Law of Energy Conservation is introduced and discussed.  Energy units are defined.

Temperature and heat are defined.

Measurement of heat is described.  System and surroundings are defined.  Heat transfer between two objects is calculated.

The Heat of a chemical reaction is discussed.  State functions are defined.

Heat of reaction is explained.

Heat and work and examined.  Heat of reaction is defined.  Exothermic and endothermic reactions are described.

Specific requirements for thermochemical calculations are listed.

Heat of reaction calculations are explained using Hess's Law taking advantage of Enthalpy being a state function.

Standard Heat of Reaction for the formation of chemical compounds is explained and used in calculating the Heat of reaction.

Properties of waves are described and applied to the electromagnetic spectrum including visible light.

The distinction between continuous and quantized energy is discussed with their application to the electrons in atoms.

The four quantum numbers are introduced and discussed.  The Pauli Exclusion Principle is introduced.

In this lecture the shapes of the electron orbitals are described.

The procedure for assigning the electron configuration, including core notation, is explained.  Orbital Notation is also presented.  Hund's rule is introduced.

Valence electrons are defined and it is shown how the number of valence electrons can be determined from the electron configuration of the element and its location on the periodic table.

Some electron configuration exceptions are discussed and explained.

The concept of electron shielding of the atom's valence electrons is discussed and how it determines the effective nuclear charge of the element.

The sizes of atoms and ions are predicted based on effective nuclear charge and their position on the periodic table.

Energy requirements to remove electrons form atoms is discussed.  Trends for ionization energy are predicted from effective nuclear charge and the position of the elements on the periodic table.

Discussion of removal of more than one electron from an atom.  The ability to identify an unknown elements based of successive ionization energies is discussed.

The energy change involved with the addition of an electron to a neutral atom is discussed in view of orbital vacancies and effective nuclear charge.

Ionic bonds are defined.  Electron configurations for ions are discussed.  Octet rule is introduced.

Covalent bonds are defined.  Bond length is discussed. 

Electronegativity is introduced and used to determine bond polarity.  Electronegativity trends of the elements determined by atomic size and effective nuclear charge.  Memory trick given for electronegativity trends of the most common elements.

Rules for assigning Lewis dot structures are presented, dots representing the valence electrons of atoms.

The concept of formal charge of an atom in a compound is described.  The formula for calculating formal charge is given.  The Pauling Electroneutrality Principle is defined and applied to formal charge determinations.

The concept of resonance Lewis dot structures is explained.

Bond dissociation energy is discussed and used to approximate heat of reaction calculations.

Strength of ionic bonds expressed as lattice energy is discussed with predictions made using Coulomb's Law.

Hess's Law is used to calculate the lattice energy of an ionic compound in a procedure called the Born-Haber Cycle.  Hess's Law was covered in Lecture 61, not 62, as I incorrectly stated in this lecture.

The HONC mnemonic is given and the VSEPR Model is introduced which is used to predict the parent and molecular geometry (shape) of molecules and polyatomic ions.

The parent and molecular geometry for compounds which have 2 to 4 electron domains on the central atom are presented.

The parent and molecular geometry for compounds which have 5 and 6 electron domains on the central atom are presented.  At about the 7:36 mark of the lecture video, I incorrectly said carbon atom instead of chlorine atom.

The geometry of multi-centered atoms are explained in this lecture.

Polar and non-polar molecules are determined in this lecture by examining the bond polarity and geometry of the chemical compound.