CH1 Lecture Notes
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The Atomic Theory
The Atomic Models
1803: John Dalton, atoms are tiny, indestructible partilces, with no internal structure
1897: J.J. Thomson: Discovers the electron and develops the plum-pudding model.
1904: Hantaro Nagaoka suggests atoms have nucleus
1911: Ernest Rutherford; Gold foil experiment leads to nuclear atom model
1913: Neils Bohr; electron moves in circular path around nucleus at fixed energy levels.
1923: Louis de Broglie; electrons have wave and particle properties.
1926: Erwin Schrodinger describes motion of electrons leading to electron cloud model
1932: James Chadwick confirms neutrons
The Atomic Structure
The Bohr Theory
Shells, subshells, and orbitals
Order of increasing energy
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d
Electronic structure and the periodic table
Writing electron configurations
See definition of protons. The Atomic number of an element is equal to the number of protons.
The majority of the atomic mass is located in the nucleus of the atom.
Constructed in vertical columns called groups or families and rows called periods.
Three distinct areas of the periodic table.
- Main group elements
- Transition group elements
- Inner transition group elements
- Classical - Main groups
- Amended - Main groups and transition groups labeled
- Modern - Arabic numerals 1 through 18
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