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      • Matter Lesson 2 Mixtures and Separation
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      • Gas Laws Lesson 2 Combined Gas Law
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      • Lesson 1 Atomic Theory
      • Lesson 2 Subatomic Particles
      • Lesson 3 Foundations of PT
      • Lesson 4 Types of Elements
      • Lesson 5 Electrons
      • Lesson 6 Atoms vs Ions
      • Lesson 7 Oxidation Numbers
      • Lesson 8 Electron Dot Diagrams
      • Lesson 9 Isotopes
      • Lesson 10 Periodic Trends
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      • Bonding Lesson 1 Basics
      • Bonding Lesson 2 Ionic Bonds
      • Bonding Lesson 2b Stock System
      • Bonding Lesson 3 Covalent Bonds
      • Bonding Lesson 3b Naming Covalent Bonds
      • Bonding Lesson 3c Multiple Bonds and Bond Strength
      • Bonding Lesson 4 Metallic Bonds
      • Bonding Lesson 5 Symmetry
      • Bonding Lesson 6 IMF
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      • Nuclear Lesson 2 Radioisotope Uses
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      • 10. Math & Moles >
        • Math Lesson 1 Mass
        • Math Lesson 2 Percent Composition
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        • Math Lesson 4 Molecular Formula from Empirical
        • Math Lesson 5 Mole Ratios
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        • Acids and Bases Lesson 1 Properties
        • Acids and Bases Lesson 2 Naming
        • Acids and Bases Lesson 3 Reactions
        • Acids and Bases Lesson 4 pH Scale
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        • Kinetics & Equilibrium Lesson 1 Collision Theory and Factors
        • Kinetics & Equilibrium Lesson 2 PE Diagrams
        • Kinetics & Equilibrium Lesson 3 Equilibrium
        • Kinetics & Equilibrium Lesson 4 LeChateliers Principle
        • Kinetics & Equilibrium Lesson 5 Entropy and Enthalpy
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        • RedOx Lesson 2 RedOx Reactions
        • RedOx Lesson 3 Half Reactions
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        • Organic Lesson 1 Intoduction
        • Organic Lesson 2 Hydrocarbons
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  • NYS Chemistry Curriculum

Lesson 2 Subatomic particles

Atom: the smallest particle of an element

Picture
Subatomic Particles
Atoms are made up of three particles:
particle                   charge              mass                    location
proton (p)                                       +                               1 amu (u)                               nucleus
neutron (n
)                           no charge               1 amu (u)                         nucleus
electron (e)                                      -                                 1/1836 amu (u)                   orbital   



amu: atomic mass unit - 1/12 the mass of a carbon atom

Nucleus: the dense positively charged central core of the atom

Orbital: a region in the atom where there is a high probability of locating an electron.





Atomic Number: number of protons in the nucleus (Bottom # on PT)
*identifies the element (like your SS#)


Mass number: total number of protons and neutrons in the nucleus (Top # on PT)

Nuclear Charge: (always +) equals atomic number (neutrons have no charge)

Isotopes: elements that have the same #p, but different #n (same element but different masses)

atomic mass: the average mass of all of the isotopes of an element

Net (overall) charge =  #p - #e
​All elements, as written, on the periodic table are neutral. This means that #p = #e


***If an atom does not have the same number of protons and electrons it is an ION and is positive (if it has more protons) or negative (if it has more electrons).
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