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Periodic Table Metals Nonmetals Main Group Noble gases
Transition metals Lanthanides & Actinides
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Metals
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Nonmetals
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Main Group Elements
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Noble Gases
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Transition Metals
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Lanthanides and Actinides
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Ionic Charges of Main Group
1 II III IV V VI VII
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Main Group Ions Group I and II: cations that correspond to group number Na+, Mg2+, Sr2+ Group III: Al (Ga): Group number: Al3+ Group IV: no monatomic ions Group V, VI, VII: anions that are 8 – group number: N3-, S2-, Br–
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1 – Predict the charges on the ions formed from the following Main Group atoms
Mg Cl F N P K Ba
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1 – Predict the charges on the ions formed from the following Main Group atoms
Mg Cl F O P K Ba Mg2+ Cl– F– O2– P3– K+ Ba2+
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Periodic Table Law versus Theory Scientific Law Empirical observation
No known exceptions Often a relationship between properties
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Periodic Table Scientific Theory Periodic Table
Principles that explain observations associated w/ laws Testable and tested Periodic Table Mendeleev & Meyer Empirical observations Atomic Theory came much later
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Periodic Properties: Atomic Size
Atoms are not billiard balls. Radial Electron Density (Atomic Radius) Effective Nuclear Charge, Zeff Z = number of protons Zeff < Z Shielding or screening by inner shell electrons
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Atomic Radius Z+ Nuclear charge is screened by inner shell electrons
Zeff < Z Z+ n=1 n=2 n=3
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Atomic Radius “Same” shell electrons do not screen as well as inner shell electrons. Zeff as you fill a shell (move across row of periodic table) Na Mg Al Si P S Cl Ar Increasing Z (+1) Screening < 1 Zeff Zeff = Z – S
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Atomic Radius Atomic radius as you move across row
Atomic radius as you move down column Size decreases Size increases
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Problem 2 Arrange each of the following groups of atoms in order of increasing size: Cl, Mg, Si Ge, Pb, C
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Problem 2 Cl < Si < Mg C < Ge < Pb
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Ionic Size in an Isoelectronic Series
Isoelectronic Series: N3– O2– F– Ne Na+ Mg2+ Al3+ Size decreases Same electron configuration Increasing Z
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Periodic Properties: Ionization Energy
M + energy M+ + e– Ionization energy, In M+ + energy M2+ + e– I2 As Zeff , In Photoelectric effect: I1 = Eho
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Ionization Energy Ionization Energy Increases
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Problem 3 Arrange the following groups of atoms in order of increasing ionization energy. Cr, N, Rb, F Ar, In, P, Ba,
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Problem 3 Rb < Cr < N < F Ba < In < P < Ar
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Ionization Energies Atom I1 I2 I3 I4 I5 I6 I7 Na Mg Al Si P 496 4560
6912 9544 13,353 16,610 20,115 Mg 738 1450 7730 10,540 13,630 17,995 21,704 Al 578 1820 2750 11,600 14,800 18,400 23,300 Si 786 1580 3230 4360 16,100 19,800 23,800 P 1012 1900 2910 4960 6270 22,200 25,400
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Other Periodic Trends Physical properties Ion formation Reactivity
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Other Periodic Trends Alkali metals Form +1 ions
Very reactive with O2, water Gray, soft metals Always found in compound form
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Other Periodic Trends Alkaline earths Form +2 ions Less reactive
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Other Periodic Trends Halogens Form –1 ions, very negative
electron affinities Very reactive with metals to form MnXy
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Other Periodic Trends Noble Gases Monatomic Very unreactive (Xe, Kr)
Large I1
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