Chapter Two - Chemistry Timeline
400 B.C. Demokritos and Leucippos
use the term "atomos"
2000 years of alchemy
Georg Bauer: systematic metallurgy
Paracelsus: medicinal application of
Robert Boyle:The Skeptical Chemist
(Apply in order listed)
1. All group 1A metal ions and ammonium ion are soluble.
2. All nitrates, perchlorates, and acetates are soluble.
3. Silver ion, lead(II), and mercury(I) are insoluble.
4. Chlorides, bromides, and iodides are soluble.
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Chapter 8 Notes - Bonding: General Concepts
8.1 Types of Chemical Bonds
A. Ionic Bonding
1. Electrons are transferred
2. Metals react with nonmetals
3. Ions paired have lower energy (greater stability) than separated ions
B. Coulomb's Law
E = energy in jo
Chapter 7 Notes - Atomic Structure and Periodicity
7.1 Electromagnetic Radiation
Types of EM Radiation (wavelengths in meters)
to 7x 10
Chapter 2 Notes - Atoms, Molecules and Ions
2.1 The Early History
Refer to the Chemistry History Timeline for this chapter
2.2 Fundamental Chemical Laws
A. Law of Conservation of Mass
1. "Mass is neither created nor destroyed"
2. Translation: In ordinary
Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry
4.1 Water, the Common Solvent
A. Structure of water
1. Oxygen's electronegativity is high
(3.5) and hydrogen's is low (2.1)
2. Water is a bent molecule
3. Water is a polar molecule
Chapter 1 Notes - Chemical Foundations
1.1 Chemistry: An Overview
A. Reaction of hydrogen and oxygen
1. Two molecules of hydrogen react with one molecule of oxygen to form
two molecules of water
2H2 + O2 2H2O
2. Decomposition of water 2H2O
2H2 + O2
Chapter 3 Notes - Stoichiometry
3.1 Atomic Masses
A. C-12, the Relative Standard
1. C-12 is assigned a mass of exactly 12 atomic mass units (amu)
2. Masses of all elements are determined in comparison to the carbon 12 atom (12C) the most common isotope of