Periodic Table Flashcards

Group or Family Column (up & down)

Period or Series Row (across)

# of valence electrons Elements in the same column have the same …

# of principle energy levels Elements in the same row have the same …

the number of valence electrons Chemical properties are determined by

one valence electron Elements in column 1 (IA) have

two valence electrons Elements in column 2 (IIA) have

Noble gases The name of the family in column 18 (VIIIA)

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

H 2, N 2, O 2, F 2, Cl 2, He, Ne, Ar, Kr, Xe, & Rn Elements that are gases at room temperature

Hg (metal) & Br 2 (nonmetal) Elements that are liquids at room temperature

Diatomic Elements H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2

Chemical properties Elements in the same column have similar

3 valence electrons Elements in column 13 (IIIA) have

4 valence electrons Elements in column 14 (IVA) have

Half the diameter of an atom, a measure of size Atomic radius

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

Alkali Metals Name of family for column 1

Alkaline Earth Metals Name of family for column 2

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

Decreases as you go down a column, increases across a row Trends for Ionization Energy

Format of Ionization Equation Na(g) + energy  Na +1 (g) + 1e -

Ionization Energy Always Endothermic!

LOSERS Metals are “_______”

Positive ions that are smaller than the parent atom. Metals lose electrons to form …

Most active metals Most “metallic” character Metals with the lowest ionization energy

Most Active Metal Cs

Ionization energy & Potential Well

What property do we use to assess the character of metals? Ionization Energy The best metals are the best losers! They have the lowest I.E.!

Properties of metals 1)Malleable 2)Ductile 3)Good conductors of heat & electricity 4)Lustrous 5)Low ionization energy 6)Low electronegativity

Properties of nonmetals 1)Brittle 2)Dull 3)Poor conductors of heat & electricity 4)High ionization energy 5)High electronegativity

Metals tend to have … Only a few valence electrons: 1, 2, or 3

winners Nonmetals are “_______”

Negative ions that are larger than the parent atom. Nonmetals gain electrons to form …

What property do we use to assess the reactivity of NONmetals? Nonmetals are winners, so it makes sense to use a property that has to do with GAINING electrons.

Electron Affinity Amount of energy required to add an extra electron to a neutral atom in the gas phase.

Format for Electron Affinity Equation Na(g) + 1e - + energy  Na -1 (g)

Electron Affinity Can be endothermic or exothermic Is really tough to measure

Compare Ionization & Electron Affinity Equations Na(g) + energy  Na +1 (g) + 1e - Na(g) + 1e - + energy  Na -1 (g) Electrons on different sides Ions on different sides Ions have opposite charges

What property do we use to assess the nonmetallic character? Electronegativity This is a “calculated” value

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

Most Electronegative Element Fluorine

High ionization energies & high electronegativies Nonmetals have

low ionization energies & low electronegativies Metals have

Negative ions are Larger than the parent ion

Positive ions are smaller than the parent ion

Metalloids are located On the staircase

Metals are located To the left of the staircase (except for H!)

Nonmetals are located To the right of the staircase

Elements in column 15 (VA) have 5 valence electrons

Elements in column 16 (VIA) have 6 valence electrons

Trends for metallic character Decreases across. Increases down.

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

Elements with strongest metallic properties are located In the lower left corner of the periodic table.

Periodic table is arranged by Atomic number

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

Trends for nonmetallic character Increases across and decreases down.

Elements in column 17 (VIIA) have 7 valence electrons

Elements in column 18 (VIIIA) have 8 valence electrons

Form brightly colored salts and solutions (except Zn) Transition metal ions

Can have more than one positive oxidation state.

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

Allotropes Have different structures so they have different chemical & physical properties.

Allotropes of oxygen O 2 and O 3 Different formulas Different structures

Allotropes of carbon Graphite, diamond, & buckminsterfullerine (C 60 )

Lewis Diagrams of neutral atoms Use dots to represent valence electrons.

Lewis Structures of atoms Na Br Al Mg S

Lewis structures of ions Positive ions have no dots. Negative ions have 8 dots. All have [ ] and charge.

Lewis Diagrams of Cations [Na] +1, [Mg] +2, [Al] +3

Lewis Diagrams of Anions

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

Oxidation #’s GroupOxidation # , , , +5, -3 16Mostly