Show electron configuration of various atoms using the spdf configuration and the noble gas configuration. Define core electrons and valence electron definitions. Use examples of various atoms along with their group number and period number when designating their election configuration. Discuss the hybridization of carbon to contain 4 bonds. Discuss the formation of anions and cations and which orbital electrons are lost and gained during their formation. Introduce diamagnetic and paramagnetic atoms and explain why they occur
Determine why electrons are assigned to specific orbitals, s, p, d, f. Discuss attraction and repulsion forces found between nuclear protons and electrons. View and discuss an electron cloud diagram for lithium which shows the penetration of electrons from higher energy levels into lower ones, and discuss the radial probability curve for fining the electron in orbit. Discuss the different methods of presenting the electron configuration of an atom. Introduce the spdf notation, the orbital box notation and the noble gas configuration notation.
Discuss why compound formulas are based on the distribution of electrons within the atom, how the electrons are arranged. State and discuss the Pauli exclusion principle along with a generalization of the principle. Review quantum numbers and what they demonstrate. Discuss attraction and repulsion of electrons by protons and other electrons in the atom. Use diagrams to indicate why electrons can exist and sub shells
View and discuss a video which which explained and demonstrates the 4 major quantum numbers, what each one represents, and how they can be used to identify the electron orbitals of an atom. Discuss the Pauli exclusion Principle.
Answer and discuss 6 questions from the textbook which involve determination of orbitals and electron numbers located within different sub shells . Solve wavelength and energy questions.
Discuss the quantum numbers used to describe the orbits for atoms. List and explain the principal quantum number and what it describes, the angular momentum quantum number and its description, and the magnetic quantum number. Describe sub shells and orbitals for each, along with maximum electron numbers for each orbital.
Ue diagrams to demonstrate orbital shapes. Discuss each orbital viewed and the electron cloud seen in the s orbitals. Discuss the distances from the nucleus and the boundary surface. Describe the shapes formed by the orbitals and the number of electrons maximum within each orbital.
Discuss how and why the Bohr's model of the atom can be descried accurately for the hydrogen atom,, for energy and location. Introduce the Heisenberg principle and why chemists accept the notion of knowing only the location when energy is the key to understanding the atom. Introduce quantum numbers as a description of the atom
Discuss Bohr's equation for Energy of an electron as E=-Rhc/n^2. Solve for the energy in a hydrogen electron. Discuss Bohr's observations, levels of energy, and the excited atom. Introduce the wave-particle duality theory and the photoelectric effect. Introduce wavelength=h/mv. Discuss why only with subatomic particles, protons, neutrons, and electrons, will a wavelength be determined
Discuss the atomic model as proposed by Neils Bohr.. Concentrate on the electronic structure of an atom and the emission spectrum seen by an excited atom. Introduce his theory of the planetary model. View the emission spectrum for hydrogen. Elicit how stability of the system due to the electron occupied by specific energy levels. Discuss the Bohr equation, E=- Rhc/n^2 and specify what each represents.
