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26 Cards in this Set
- Front
- Back
Ionization energy
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the energy required to REMOVE one electron from an atom of an element; measured in kJ/mol
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Electronegativity
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how attracted an element is to electrons; the “desire” to gain electrons; a scale from 0.0 to 4.0
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Atomic Radius
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the radius (size) of an atom; measured in pm (picometers)
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Ionic Radius
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the radius of an ion; cations (lose electrons) decrease in radius; anions (gain electrons) increase in radius
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Chemical Reactivity
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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
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Metallic Character
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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”
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Nonmetallic character
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nonmetals are NOT malleable (shatter upon being hit with a hammer), NOT ductile, do NOT have luster (dull), and do NOT conduct electricity
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Metals
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elements that have all four properties/characteristics of a metal; located under/to the left of the staircase, except for Hydrogen (H)
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Metalloids
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elements that have two properties/characteristics of metals; located along the “staircase,” except for Al and At
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Nonmetals
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elements that have zero or one property/characteristic of a metal; brittle; located above/to the right of the staircase
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Alkali metals
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all elements located in Group 1 on the periodic table except hydrogen; contains the most reactive metals
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Alkaline Earth metals
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all elements located in Group 2 on the periodic table
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Halogens
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all elements located in Group 17 on the periodic table; most of the halogens have high electronegativities
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Noble Gases
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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
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Transition metals
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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
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Periodic
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cyclic; repeating pattern/cycle
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Periodic Law
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elements of the periodic table are periodic functions of their atomic number
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Periods
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horizontal rows on periodic table
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Octet
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full valence shell; 8 electrons, except for period 1 elements
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Solids
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have definite shape and definite volume; most elements are solids at STP
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Liquids
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take the shape of their container and have definite volume; only 2 elements exist as liquids at STP: Br, and Hg
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Gases
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have no definite shape and fill their container; at STP this includes H, N, O, F, Cl, & all of group 18 (the noble gases)
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Diatomic elements
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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
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Allotrope
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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)
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Groups |
vertical columns on periodic table |
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States of Matter |
any of the three phases in which an element can exist; solid (s), liquid (l), gas (g) |