Periodic Table Test Flashcards
Lavoisier
Separated periodic tables into metals and nonmetals
Dobereiner
Created triads (groups of 3 elements that were similar)
Newlands
Developed Law of octaves. Recognized repeating pattern of 8
Meyer
Arranged elements by valence
Mendeleev
Arranged elements by atomic mass. Predicted properties of undiscovered elements
Moseley
Rearranged table based on atomic numbers
Seaborg
Pulled out lanthanides (actinide series)
Periods
Horizontal rows (1-7)
Tells the energy level of the highest energy electrons.
Families/Groups
Vertical columns.
Arranged base on similarities in reactivity.
Main groups (1A-8A) correspond to valence electrons (exc He)
Metals
Located left of zig zag line. Have luster, are malleable, are conductors and ductile. Predominantly solids at room temp.
Metallic oxides react with water to form bases.
Nonmetals
Right of zig zag line. Predominantly gases.
Usually brittle.
Insulators.
Nonmetallic oxides react with water to form acids.
Metalloids
Touch zig zag line (excp Al)
Has properties of metals and nonmetals. Semi conductors.
Alkali Metals
Group 1A.
Extremely reactive, explosive in water.
Not found alone in nature. Soft
Alkaline Earth Metals
Group 2a
Same as Alkali, but to lesser extent
Halogens
Group 7a
Very reactive nonmetals
Diatomic (two atoms combine with each other)
Diatomic
Two atoms combine with each other
Noble Gases
Group 8a
Inert (do not react)
Transitional metals
Groups 1b-8b
Properties differ from each other
Many form-colored solutions
Used to include lanthanide/ actinoid series (which is predominantly radioactive)
Atomic Radius
Size of the atom (from the nucleus, outwards)
Atomic Radii
Size increases going down family b/c of the addition of extra energy levels.
Size decreases a period due to increase in nuclear charge and “pulling in” electrons due to greater attractive force
Ionization Energy (Def)
Energy to remove an electron from a gaseous atom
Ionization Energy
Decreases going down a family b/c increased size of atom, which lowers the attractive force and “shields” inner electrons
Increases going across period due to increased nuclear charge, which increases attractive force
Nuclear Charge
Increases going across a period
Formation of Ions
Atoms gain/lose electrons to get to a noble gas configuration
Formation of Ions (Metals)
Metals lose electrons to form positive ions. If a metalloid is on the left, it acts as a metal.
Formation of Ions (Nonmetals)
Nonmetals gain electrons to form negative ions. If a metalloid is on the right, it acts as a nonmetal.
Ion Atomic Radius
Positive ions are smaller than original atoms.
Negative ions are larger than the original atom.
Electronegativity (Def)
Attraction for electrons within a bond
Electronegativity Trend
(Same as ionization energy)
Decreases going down family
increases going across a period
Electron Affinity (Def)
Attraction for an electron (not within a bond)
Electronegativity
(Same as ionization energy)
Decreases going down family
Increases going across a period
Melting Point
Decreases down metal groups
Increases down nonmetal groups
Increases across a period until group 4a (14), then decreases
Density
Increases going down a family
Reactivity
Increases going down a family for metals
Decreases going down a family for nonmetals
