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Presentation transcript:

How would you organize these…?

Early Periodic Tables J.W. Dobereiner John Newlands Group elements in triads (sets of 3) Based on chemical/physical properties Didn’t work well with metals John Newlands Law of Octaves Properties of elements seem to change every 8th elements

Modern Periodic Table Dmitri Mendeleev Periodicity Periodic Law Groups elements by atomic mass Groups = vertical columns Periods = horizontal lines Predicted details for elements not yet discovered Periodicity Repeating patterns at set intervals Periodic Law pattern in chemical and physical properties of the elements when they are arranged by increasing atomic numbers

Modern Periodic Table Henry Moseley Designed periodic table used today Ordered elements by increasing atomic numbers

Reading the Periodic Table Element Atomic symbol Atomic number Atomic mass

Number of electrons in sublevels Periods Period shows the number of shells possible for those elements 2n2 = max # of electrons Period #/ Shell # Number of electrons in sublevels Max # of electrons In Shell n=1 2 n=2 8 n=3 18 n=4 32 n=5 50 n=6 72 n=7 98

Groups “A” Group- representative elements Special Names: Group # = Valence electron # Special Names: I A = Alkali Metals II A= Alkaline Earth Metals VII A= Halogens VIII A= Nobel Gases

Element Ion Charges -1; F-, Cl-, etc… +4/-4 Elements are most stable when they have a full set (8) of valence electrons A’s Group # = Ion charge Group I A = +1; H+, K+, etc.. Group IIIA = +3; B+3, Al+3, etc.. Group VIIA = Group VIA= -2; O-2, Se-2, etc… Group IVA= -1; F-, Cl-, etc… +4/-4