The Periodic Table and Atomic Configurations Notes B. A. Rowland 53750/53760 History of the Periodic Table The current version of the Periodic Table was organized by Dmitri Mendeleev in 1869. He arranged his version of the Periodic Table by atomic ma
Lecture 5 Notes B. A. Rowland 53750 Atomic Configurations We can assign atomic electronic configurations via one of two methods. The first is by using the periodic table. If you recognize the s-, p-, d-, and f-blocks of the periodic table you can fig
Lecture 4 Notes B. A. Rowland 53750 Hydrogen Orbitals The solutions for the Schrdinger equation for the hydrogen atom are characterized by four quantum numbers. n is called the principle quantum number. You may think of this quantity exactly as we th
Lecture 2 Notes B. A. Rowland 53750 Blackbody Radiation The early 1900s were a good time for physicists. They thought they had it all figured out. Unfortunately, the problem of Blackbody Radiation was to prove difficult for the scientific paradigm of
Lecture 1 Notes B. A. Rowland 53750 I will outline a few highlights from the first lecture in these notes. These are written in conjunction with the slides presented in class. Light For years light was thought to be a wave. There are some terms you s
Lecture 1 Notes B. A. Rowland 53750 I will outline a few highlights from the first lecture in these notes. These are written in conjunction with the slides presented in class. Light For years light was thought to be a wave. There are some terms you s
Applications of the First Law B. A. Rowland 53750/53760 Types of Enthalpies You will need to be able to classify certain types of enthalpy reaction, and be able to give an example of each: Hrxn = The Enthalpy of Reaction: the enthalpy for any given c
The First Law of Thermodynamics B. A. Rowland 53750/53760 Types of Systems We can classify thermodynamic systems as one of three types. The first is the open system. In an open system, the system may exchange both matter and energy with the surroundi
Introduction to Thermodynamics B. A. Rowland 53750/53760 What is Energy? In this class, we will define energy as the ability to produce work (w) or heat (q). Energy is a conserved quantity, which means it can never be created or destroyed, just conve
Liquids, Solutions, and Solids B. A. Rowland 53750/53760 Comparing the States of Matter Let us take a molecular-level view of the three phases of matter (you can see this diagram on slide 3 of this lecture). Gas: Lots of space between gas particles a
Kinetic Molecular Theory B. A. Rowland 53750/53760 Kinetic Molecular Theory of Gases Kinetic Molecular Theory (KMT) was developed by Clausius, Maxwell, and Boltzmann in the 19 th century to provide a theoretical justification for the behavior of idea
Advanced Topics in Gas Laws B. A. Rowland 53750/53760 Gas Stoichiometry (Dry) The idea behind dry gas stoichiometry is to use the ideal gas law in conjunction with regular stoichiometric methods to calculate how much gas is produced (or consumed, or
Lecture 3 Notes B. A. Rowland 53750/53760 Coulombs Law Charged particles (protons [+] and electrons [-]) can exert a force between each other known as electrostatic forces. A knowledge of electrostatics is very helpful in chemistry, as one can explai
Introduction to Gas Laws B. A. Rowland 53750/53760 Phases of Matter There are three distinct phases of matter that we can observe on the Earth: solids, liquids, and gases. There are also two others: plasmas (ionized mattervery hot!) and Bose-Einstein
Spectroscopy B. A. Rowland 53750/53760 Overview of Molecular Spectroscopy Molecular spectroscopy is the use of electromagnetic radiation (EMR) to induce electrons to make quantum transitions. In the figure in my slides, I have presented the potential
Crystal Field Theory B. A. Rowland 53750/53760 Bonding with a Transition Metal Up until this point we have only been concerned with compounds formed from the maingroup elements. We have yet to describe bonding for compounds containing transition meta
Molecular Orbital Theory B. A. Rowland 53750/53760 Molecular Orbital Theory Molecular Orbital (MO) theory is a theory of bonding which is more consistent with quantum mechanics, as it allows us to delocalize the electrons (rather than keeping them lo
Hybridization of Atomic Orbitals B. A. Rowland 53750/53760 Hybridization Overview Experimental studies (basically, spectroscopy) shows that the four single bonds in the molecule methane (CH4) are exactly identical: they have the same length as well a
VSEPR and Molecular Geometries B. A. Rowland 53750/53760 VSEPR Model I We have thus far constructed 2-D representations of simple molecules. Unfortunately, this is not the correct picture We thus introduce the concept of the Valence Shell Electron Pa
Exceptions to the Octet Rule, Resonance, and the VSEPR Model B. A. Rowland 53750/53760 Exception 1: Octet Deficient Atoms Up to this point, we have only discussed one octet deficient atomhydrogen. Hydrogen only wants 2 electrons to fill its octet. Th
The Covalent Bond and Lewis Structures B. A. Rowland 53750/53760 The Covalent Bond A covalent bond is one that is formed through the sharing of a pair of electrons in a molecule. Just as in our discussion of ionic bonds, there will be two parameters
Intermolecular Forces B. A. Rowland 53750/53760 IMF I Intermolecular forces are those forces which act between the molecules in a given sample (as opposed to intramolecular forces, which are the forces which hold the atoms together in an individual m
The Ionic Bond B. A. Rowland 53750/53760 Electron Shielding Please see Lecture Notes for The Periodic Table and Atomic Configurations. Formulas for Ionic Compounds In order to discuss ionic bond strength, we will need to be able to assign charges to
Chemical Bonds in Chemistry B. A. Rowland 53750/53760 Chemical Bonds Chemical bonds can be classified as ionic, covalent, polar covalent (a cross between ionic and covalent), or metallic. The two characteristics of chemical bonds that we will be inte
