the periodic table chapter 5 notes. mendeleev ● designed first periodic table (1869) ● arranged...
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The Periodic Table
Chapter 5 Notes
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Mendeleev●Designed first periodic table (1869)
●Arranged mostly by increasing atomic
mass
●Elements in the same column have similar
properties
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Moseley
●Arranged by increasing atomic number
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Periodic Law
●Elements’ physical and chemical
properties show a periodic [“repeating”]
pattern when arranged by atomic number
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●COLUMN = Group or FamilyoSimilar properties based on the same number
of valence electrons
oNumbered 1-18 or with Roman numerals
●ROW = Period
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Valence electrons
●Electrons in the outermost shell
●Octet Rule = all atoms want 8 valence
electrons to achieve stabilityoExceptions: H, He
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Families of the Periodic Table
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Alkali Metals●Soft
●Most reactive metals
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Noble Gases
●very UNreactive
●“inert”
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Halogens
●Most reactive nonmetals
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Metals
●luster/shiny, good conductors of heat &
electricity, malleable, ductile
●LEFT SIDE of periodic table
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Nonmetals
●not shiny, poor conductors, not malleable
or ductile, brittle
●RIGHT SIDE of periodic table
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Metalloids●“semi-metals”
●some properties of metals, some of
nonmetals
●touch ZIG-ZAG LINE
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Periodic Trends
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Atomic Radius●Distance from the nucleus to the outer
electrons
●Decreases across a row
●Increases down a column
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Explanation of Atomic Radius
increasing down a column
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Explanation of
Atomic Radius
increasing
down
a column
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Explanation of Atomic Radius
decreasing across a row
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Explanation of Atomic Radius
decreasing across a row
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Electronegativity●Ability of an atom to attract electrons to
itselfoIncreases across a row
oDecreases down a column
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Ionization Energy●Energy needed to remove an electron
●Increases across a row
●Decreases down a column
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Electron Affinity●How much an atom wants to gain an
electronoDecreases down a column
oIncreases across a row
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Think about Corners
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Practice- Circle your answer
choiceLarger atomic radius?
1) Mg or Sr
2) Mg or S
Larger electronegativity?
3) P or Sb
4) Ge or Br
Larger ionization energy?
5) Ca or Se
6) Ca or Ra
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Ion Size
●Cation – atom loses electronoAtom gets smaller
●Anion – atom gains electronoAtom gets bigger
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Exampl
e
of Ion
Size