Atomic Theory
The Periodic Table
Anatomy of the Atom
Ions
Isotopes
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The smallest particle of any given element

The atom

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The 18 vertical columns on the Periodic Table

Groups

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The center of the atom

Nucleus

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Ions have a different number of this subatomic particle:

Electrons

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Isotopes have a different number of this subatomic particle: 

Neutrons

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H2O, CO2, NaCl are examples:

A molecule

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Periods are organized left to right by: 

Atomic Number 

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The positively charged subatomic particle

Proton

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A negatively charged Ion: 

Anion

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The number next to an Isotope represents: 

Atomic Mass 

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The modern Atomic Theory was first published by English Scientist: 

John Dalton

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Has properties of both Metals and Nonmetals such as Arsenic 

Metalloids

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Represented as atomic mass - atomic number

Neutrons

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Li+ is known as a Cation and has this type of charge: 

Positive

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The atomic mass of U-235

235

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Represented by their atomic number, each element has a different number of: 

Protons

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1869 Russian chemist, created the Periodic Table of Elements

Dimitri Mendeleev

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In an uncharged atom found in equal numbers to protons

Electrons

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Solve for all subatomic particles: Tc7+

Technetium; A#: 43 AM: 98 P+: 43 N0: 55 E-: 36

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Solve for all subatomic particles: O-18 

Oxygen; A#: 8 AM: 18 P+: 8 N0: 10 E-: 8

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Atoms combine in this type of numbered ratio: 

Whole-number 

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Scientists use the PTE to understand and predict: 

Element properties

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Two subatomic particles found in the nucleus

Protons and Neutrons

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A common Ionic element used in most batteries

Lithium 

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A common use for the Isotope C-14 in Geology

Carbon dating

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