chem topic 2 (10th grade)
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45 Terms
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Periodic Table
Organizes elements by atomic number - showing periods and groups
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Periods
Horizontal rows - number of electron shells
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Groups
Vertical columns - number of electrons in outer shell
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Valence Electrons
Electrons in outermost energy level that determine reactivity
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Rule of Octet
Atoms bond to have 8 electrons in outer shell (except hydrogen)
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Metal Properties
Shiny - ductile - malleable - good conductors - react with water (corrosion)
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Non-Metal Properties
Dull - brittle - poor conductors - many are gases
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Metalloid Properties
Solid - can be shiny or dull - semi-conductors - ductile - malleable
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Atomic Radius (AR)
Distance from nucleus to outermost electron - size of atom
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AR Trend
Increases down a group - decreases across a period
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Ionization Energy (IE)
Energy needed to remove an electron from a gaseous atom
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IE Trend
Decreases down a group - increases across a period
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Electronegativity (EN)
Ability of an atom to attract electrons in a chemical bond
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EN Trend
Decreases down a group - increases across a period
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Electron Affinity (EA)
Energy change when an atom gains an electron
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EA Trend
Becomes more negative across a period - varies down a group
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Metallic Character
How easily an element loses electrons (metal-like behavior)
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Metallic Character Trend
Increases down a group - decreases across a period
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Alkali Metals
Group 1 - 1 valence electron - highly reactive - never free in nature
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Alkaline Earth Metals
Group 2 - 2 valence electrons - reactive - never free in nature
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Transition Metals
Groups 3–12 - dense - multiple oxidation states - good conductors
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Boron Family
Group 13 - 3 valence electrons - includes metalloid (B) and metals
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Carbon Family
Group 14 - 4 valence electrons - includes metals - metalloids - non-metals
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Nitrogen Family
Group 15 - 5 valence electrons - mostly share electrons
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Oxygen Family
Group 16 - 6 valence electrons - reactive - forms compounds easily
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Halogens
Group 17 - 7 valence electrons - most active non-metals - form salts with alkali metals
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Noble Gases
Group 18 - full outer shell (8 electrons except helium which has 2) - extremely unreactive (inert)
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Rare Earth Elements
Lanthanides and Actinides - mostly synthetic (trans-uranium)
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Electron Configurations
Arrangement of electrons in shells and subshells
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Example Li
1s² 2s¹
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Example Na
1s² 2s² 2p⁶ 3s¹
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Example K
1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹
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Subshell Order
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰
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Shells by Letters
K=1st - L=2nd - M=3rd - N=4th
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Reactivity
How easily an element bonds with others
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Group 1 Reactivity Trend
Increases down the group
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Group 7 Reactivity Trend
Decreases down the group
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Noble Gas Reactivity
Extremely unreactive
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Transition Metal Density
Denser than Group 1 elements
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Melting/Boiling Points Trend
Decrease down Group 1
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Effective Nuclear Charge (Zeff)
The attraction between protons in the nucleus and the valence electrons
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Zeff Trend Across a Period
Increases because more protons pull electrons stronger
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Zeff Trend Down a Group
Decreases because more shells reduce the pull on valence electrons
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Oxidation State
The charge an atom has after losing or gaining electrons
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Most Electronegative Element
Fluorine F has the strongest pull on electrons
Note 
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