ࡱ> ` bjbj .8<  ###8$$4X$L A2$$$$$$sh 3v$$s$ $n  $$ ![/A# 0A@ A $# #  Unit 4: The Periodic Table and Periodicity The Elements Element names come from a variety of sources. elements known to the ancients Au, Ag, S, Sn, C place names Fr, Po, Ge, Ga, In, Eu, Am, Cf, Sc famous people Es, Fm, Md, No, Gd, Rf, Bh foreign languages W, Fe, Au, Ag, Pb, Sn, K mythology-related names Th, Pm, Ce, Ta, Ti, Pd, Ir names related to element properties Xe Background on the Periodic Table Dmitri Mendeleev: given credit for Periodic Table (~1870) -- organized Table by increasing atomic mass -- left spaces and predicted properties of undiscovered elements Henry Moseley: put elements in order of increasing atomic number Describing the Periodic Table periodic law: the properties of elements repeat every so often period: horizontal row; (7) group (family): vertical column; (18) Regions of the Table metals: left side of Table; form cations properties: good conductors of heat and electricity, lustrous, malleable, ductile nonmetals: right side of Table; form anions properties: good insulators. gases or brittle solids metalloids (semimetals): stair between metals and nonmetals properties: in-between those of metals and nonmetals semiconductors Si and Ge ( computer chips alkali metals: group 1 (except H); 1+ charge; very reactive alkaline earth metals: group 2; 2+ charge; less reactive than alkalis halogens: group 17; 1 charge; very reactive noble gases: group 18; no charge; unreactive lanthanides: elements 5771 actinides: elements 89103 coinage metals: group 11 transition elements: groups 312; variable charges main block (representative) elements: groups 1, 2, 1318 Same number of valence e = similar properties Li 1s2 2s1 Na 1s2 2s2 2p6 3s1 In any group, the element BELOW has one more occupied energy level than does the element ABOVE.  Li Na The period that an element is in is the same as the energy level that its valence electrons are in. Li ( 2nd E.L. / 2nd period Na ( 3rd E.L. / 3rd period Periodicity ( there are trends in properties of elements -- left-right AND up-down trends atomic radius: the size of a neutral atom increases as we go add a new energy level each time  decreases as we go coulombic attraction: attraction between (+) and ()  Depends on amount of charge distance between charges      As we go , more coulombic attraction, no new  energy level, more pull, smaller size shielding effect: kernel e shield valence e from attractive force of the nucleus  -- caused by kernel and valence e repelling each other As we go , shielding effect increases.  ionic radius: the size of an ion cations anions Ca atom Ca2+ ion Cl atom Cl1 ion 20 p+ 20 p+ 17 p+ 17 p+  20 e 18 e 17 e 18 e cations are smaller anions are larger ionization energy: the energy required to remove an e from an atom  M + 1st I.E. ( M1+ + e  removes 1st e M1+ + 2nd I.E. ( M2+ + e M2+ + 3rd I.E. ( M3+ + e Each successive ionization requires more energy than the previous one.  As we go , 1st I.E. decreases As we go , increases electronegativity: the tendency for a bonded atom to attract e to itself Linus Pauling quantified the electronegativity scale.  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