Periodic Table Flashcards

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Periodic Table Flashcards
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Group or Family

• Column (up down)

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Period or Series

• Row (across)

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of valence electrons

• Elements in the same column have the same

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of principle energy levels

• Elements in the same row have the same

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the number of valence electrons

• Chemical properties are determined by

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one valence electron

• Elements in column 1 (IA) have

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two valence electrons

• Elements in column 2 (IIA) have

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Noble gases

• The name of the family in column 18 (VIIIA)

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Halogens

• The name of the family in column 17 (VIIA)

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H2, N2, O2, F2, Cl2, He, Ne, Ar, Kr, Xe, Rn

• Elements that are gases at room temperature

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Hg (metal) Br2 (nonmetal)

• Elements that are liquids at room temperature

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Chemical properties

• Elements in the same column have similar

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3 valence electrons

• Elements in column 13 (IIIA) have

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4 valence electrons

• Elements in column 14 (IVA) have

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Half the diameter of an atom, a measure of size

• Atomic radius

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Increases as you go down a column (more principle
energy levels) decreases across a row (greater
effective nuclear charge)

• Trends for atomic radius

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Alkali Metals

• Name of family for column 1

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Alkaline Earth Metals

• Name of family for column 2

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Amount of energy required to remove the most
loosely held valence electron from a gas phase
atom

• Ionization Energy

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X energy ? X e-

• Ionization

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Decreases as you go down a column, increases
across a row

• Trends for Ionization Energy

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LOSERS

• Metals are _______

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Positive ions

• Metals lose electrons to form

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Properties of metals

1. Malleable
2. Ductile
3. Good conductors of heat electricity
4. Lustrous
5. Low ionization energy
6. Low electronegativity

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Properties of nonmetals

1. Brittle
2. Dull
3. Poor conductors of heat electricity
4. High ionization energy
5. High electronegativity

Opposite of Metals
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winners

• Nonmetals are _______

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Negative ions

• Nonmetals gain electrons to form

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High ionization energies high electronegativies

• Nonmetals have

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low ionization energies low electronegativies

• Metals have

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Negative ions are

• Larger than the parent ion

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Positive ions are

• smaller than the parent ion

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Metalloids are located

• On the staircase

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Metals are located

• To the left of the staircase (except for H!)

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Nonmetals are located

• To the right of the staircase

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Elements in column 15 (VA) have

• 5 valence electrons

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Elements in column 16 (VIA) have

• 6 valence electrons

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Trends for metallic character

• Decreases across. Increases down.

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Most active metals?

• Cs Fr

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Metals are losers. Reactivity of metals is
judged by how easily metals

• Lose electrons

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Elements with strongest metallic properties are
located

• In the lower left corner of the periodic table.

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Periodic table is arranged by

• Atomic number

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Electronegativity

• Ability of an atom to attract electrons in a bond.

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Most Electronegative Element

• Fluorine

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Trends for electronegativity

• Increases across decreases down.

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How do we judge the reactivity of Nonmetals?

• Nonmetals are winners so we judge the reactivity
  of nonmetals by how easily they gain electons.

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Trends for nonmetallic character

• Increases across and decreases down.

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Elements in column 17 (VIIA) have

• 7 valence electrons

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Elements in column 18 (VIIIA) have

• 8 valence electrons

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Form brightly colored salts and solutions
(except Zn)

• Transition metal ions

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Properties of transition metals (B Group elements)

• Hard solids
• High MP
• Multiple oxidation states
• Ions have color

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Allotropes

• Different forms of the same element in the same
  phase.

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Allotropes

• Have different structures so they have different
  chemical physical properties.

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Allotropes of oxygen

• O2 and O3

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Allotropes of carbon

• Graphite, diamond, buckminsterfullerine (C60)

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Lewis Structures

• Use dots to represent valence electrons.

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Lewis Structures






S
Br
Na






Mg
Al

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Oxidation Number

• The charge on an atom when it has an octet in the
  valence level.

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Oxidation s
Group Oxidation
1 1
2 2
13 1, 3
14 2, 4
15 3, 5, -3
16 Mostly -2
17 -1
18 0
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General formula for a metal from Group 1 oxygen

• M2O

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General formula for a metal from Group 2 oxygen

• MO

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General formula for a metal from Group 1 a
halogen

• MX

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General formula for a metal from Group 2 a
halogen

• MX2