Notes

Slide Show

Outline

1	Unit 2 – Electrons and Periodic Behavior
2	The Bohr Model of the Atom
3	Quantum Mechanical Model of the Atom
4	Schrodinger Wave Equation
5	Heisenberg Uncertainty Principle
6	Electron Energy Level (Shell)
7	An orbital is a region within an energy level where there is a probability of finding an electron. This is a probability diagram for the s orbital in the first energy level…
8	Energy Levels, Sublevels, Electrons
9	Sizes of s orbitals
10	s orbital shape
11	P orbital shape
12	d orbital shapes
13	Shape of f orbitals
14	Orbital filling table
15	Pauli Exclusion Principle
16	Electron Spin
17	Electron configuration of the elements of the first three series
18
19	Irregular conformations of Cr and Cu
20	Wave-Particle Duality
21	The Wave-like Electron
22	Electromagnetic radiation propagates through space as a wave moving at the speed of light.
23	Types of electromagnetic radiation:
24	The energy (E ) of electromagnetic radiation is directly proportional to the frequency (n) of the radiation.
25	Wavelength Table
26	Spectroscopic analysis of the visible spectrum…
27	Spectroscopic analysis of the hydrogen spectrum…
28	Electron transitions involve jumps of definite amounts of energy.
29	Mendeleev’s Periodic Table
30	Modern Russian Table
31	Stowe Periodic Table
32	A Spiral Periodic Table
33	“Mayan” Periodic Table
34	The Periodic Table
35	The Properties of a Group: the Alkali Metals
36	Properties of Metals
37	Examples of Metals
38	Properties of Nonmetals
39	Examples of Nonmetals
40	Properties of Metalloids
41	Silicon, Si – A Metalloid
42	Determination of Atomic Radius:
43	Table of Atomic Radii
44	Ionization Energy - the energy required to remove an electron from an atom
45	Table of 1^st Ionization Energies
46	Ionization of Magnesium
47	Electronegativity
48	Periodic Table of Electronegativities
49	Summation of Periodic Trends
50	Ionic Radii
51	Table of Ion Sizes