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Atomic Theory and Subatomic Particles:
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Different atomic models and their creators: John Dalton (Solid Sphere), J.J. Thomson (Plum Pudding, discovered electrons), Ernest Rutherford (Nuclear Model), Niels Bohr (Planetary Model), and Erwin Schrodinger (Quantum Model)1.
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Atomic Number equals the number of protons and electrons2.
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Atomic Mass equals the number of protons plus neutrons2.
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Calculating Neutrons: Atomic Mass - Atomic Number2.
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Isotopes are atoms of the same element with different numbers of neutrons2.
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Finding Protons and Electrons (ZAPEN) in ions: adjust the number of electrons based on the charge (add for non-metals, subtract for metals)2....
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Periodic Table:
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Key figures in the development of the periodic table: Johann Wolfgang Dobereiner, Alexander Reina Newlands, Dmitri Ivanovich Mendeleev, and Henry Moseley3....
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Periodic Law: atomic number is more important than atomic mass4.
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The periodic table contains 118 elements4.
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Columns are called groups, and rows are called periods4.
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Classification of elements: Metals, Metalloids, and Non-Metals4....
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Metalloids: Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, and Polonium5.
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Blocks: s & p (representative elements), d (transition metals), and f (inner transition metals: lanthanides and actinides)5....
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Groups: Alkali Metals (1A), Alkaline Earth Metals (2A), Transition Metals (1B-8B), Boron Group (3A), Carbon Group (4A), Nitrogen Group (5A), Oxygen Group (6A), Halogens (7A), Noble Gases (8A)6....
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Alkali Metals are the most reactive metals6.
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Halogens are highly reactive non-metals, with Fluorine being the most reactive7.
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Noble Gases are the most stable group7.
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Trends:
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Atomic Size: Decreases from left to right, Increases from top to bottom7.
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Electron Affinity, Electronegativity, Ionization Energy: Increases from left to right, Decreases from top to bottom8.
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Electron Configuration:
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Electron Configuration of elements and noble gas form8....
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S-shell (2 electrons), P-shell (6 electrons), D-shell (10 electrons), F-shell (14 electrons)8.
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Determining the period and group for representative elements based on electron configuration9.
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Ions:
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Valence Electrons: number of electrons in the outermost shell10.
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Octet Rule: atoms are stable with 8 valence electrons10.
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Anions: formed when an atom gains electrons, resulting in a negative charge10....
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Cations: formed when an atom loses electrons, resulting in a positive charge10.
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Determining valence charge based on group number11.
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Lewis Dot Structure:
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Representing valence electrons with dots around the element symbol11....
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Chemical Bonding:
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Forces of attraction that hold atoms together through electron transfer or sharing12.
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Ionic Bonding: metal + non-metal, characterized by the transfer of electrons12....
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Covalent Bonding: non-metal + non-metal, characterized by the sharing of electrons14.
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Metallic Bonding: metal + metal15.
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Drawing Lewis Dot Structures for ionic and covalent compounds, using arrows for electron transfer in ionic bonds and lines for shared electrons in covalent bonds13....
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