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26 Cards in this Set

  • Front
  • Back
Ionization energy
the energy required to REMOVE one electron from an atom of an element; measured in kJ/mol
Electronegativity
how attracted an element is to electrons; the “desire” to gain electrons; a scale from 0.0 to 4.0
Atomic Radius
the radius (size) of an atom; measured in pm (picometers)
Ionic Radius
the radius of an ion; cations (lose electrons) decrease in radius; anions (gain electrons) increase in radius
Chemical Reactivity
the tendency for an atom of a given element to gain or lose electrons when interacting with an atom of another element. Most reactive: metal = francium; nonmetal = fluorine
Metallic Character
metals are malleable (can be hammered into thin sheets and bent), ductile (can be drawn into wire), have luster (shine), and conduct electricity; metals tend to lose electrons; all metals have a “sea of mobile valence electrons”
Nonmetallic character
nonmetals are NOT malleable (shatter upon being hit with a hammer), NOT ductile, do NOT have luster (dull), and do NOT conduct electricity
Metals
elements that have all four properties/characteristics of a metal; located under/to the left of the staircase, except for Hydrogen (H)
Metalloids
elements that have two properties/characteristics of metals; located along the “staircase,” except for Al and At
Nonmetals
elements that have zero or one property/characteristic of a metal; brittle; located above/to the right of the staircase
Alkali metals
all elements located in Group 1 on the periodic table except hydrogen; contains the most reactive metals
Alkaline Earth metals
all elements located in Group 2 on the periodic table
Halogens
all elements located in Group 17 on the periodic table; most of the halogens have high electronegativities
Noble Gases
all elements located in Group 18 on the periodic table; inert (do not tend to react with atoms of other elements); have a full valence shell
Transition metals
the rows of elements in the middle of the periodic table from scandium (Sc) to mercury (Hg); reactivity is based on the elements with which they are combined
Periodic
cyclic; repeating pattern/cycle
Periodic Law
elements of the periodic table are periodic functions of their atomic number
Periods
horizontal rows on periodic table
Octet
full valence shell; 8 electrons, except for period 1 elements
Solids
have definite shape and definite volume; most elements are solids at STP
Liquids
take the shape of their container and have definite volume; only 2 elements exist as liquids at STP: Br, and Hg
Gases
have no definite shape and fill their container; at STP this includes H, N, O, F, Cl, & all of group 18 (the noble gases)
Diatomic elements
elements that can’t exist alone in nature; travel in pairs; contain 2 identical atoms (same element); “Siamese twins,” “7-up”; N2, O2, F2, Cl2, Br2, I2, At2, H2
Allotrope
1 of 2 or more different forms of an element (nonmetal) in the same phase, but with different formulas and physical/chemical properties Ex 1: oxygen: O2 (oxygen) vs. O3 (ozone)

Groups

vertical columns on periodic table

States of Matter

any of the three phases in which an element can exist; solid (s), liquid (l), gas (g)