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Metals and Nonmetals A. Metals 1. Characteristics Do not want electrons Low ionization energy

Metals and Nonmetals A. Metals 1. Characteristics Do not want electrons Low ionization energy Low electron affinities Conduct heat and electricity Form positive ions (lose all valence e -) 2. Reactivity Generally increases as you move towards Fr

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Metals and Nonmetals A. Metals 1. Characteristics Do not want electrons Low ionization energy

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  1. Metals and Nonmetals A. Metals 1. Characteristics Do not want electrons Low ionization energy Low electron affinities Conduct heat and electricity Form positive ions (lose all valence e-) 2. Reactivity Generally increases as you move towards Fr Group makes a bigger difference than period (Na is more reactive than Ca) React with nonmetals to make SOLID compounds 2 Na(s) + Cl2(g) 2 NaCl(s) Malleable and ductile Have luster Exist as solids

  2. 3. Metal Carbonates (MCO3) When heated, carbonate ion decomposes to create CO2 Metal oxide is left MCO3 MO + CO2 MgCO3  Li2CO3  4. Metal oxides When mixed in water, metal oxides create hydroxides (BASIC) CaO(s) + H2O  Ca(OH)2(aq) MgO + CO2(g) Li2O + CO2(g)

  3. B. Trends for Active Metals • 1. Alkali Metals (Group 1) • Never pure in nature • All lose one electron when reacting • A. With water • All form hydroxides and hydrogen gas (very exothermic) • 2 Na(s) + H2O  2 Na+(aq) + OH-(aq) + H2(g) • B. With hydrogen • All form hydrides • 2 Li + H2  2 LiH(s) • C. With oxygen (air) • Na K Rb Cs form peroxides • 2 Na(s) + O2(g)  Na2O2(s) • K Rb Cs can form superoxides • K + O2(g)  KO2 • Both peroxides and superoxides decay quickly to return oxygen to a -2 oxidation state. • D. Flame test • Li (crimson red) O2-2 O2-1 Na(yellow) • K (violet)

  4. 2. Alkaline Earth Metals (Group 2) Less reactive than alkali, but still not pure in nature A. With water Mg and below react with water to make hydroxides Ca + 2 H2O  Ca+2 + 2 OH- + H2(g) (Be does not react with H2O) B. With oxygen Mg and Ca form normal oxides 2 Mg + O2 2 MgO(s) Ba forms a peroxide Ba + O2 BaO2(s) C. Flame test Ca (brick red) Sr (crimson red) Ba (green-yellow)

  5. C. Nonmetals 1. Characteristics Want electrons to fill their sublevel High electron affinities (very negative) High ionization energies Poor conductors of heat and electricity Exist as liquids, gases and molecular solids at room temperature 2. Reactivity Generally increase as you move towards F Group makes a bigger difference than period 3. Nonmetal oxides GASES that react with water to form acids Acid anhydride – Nonmetal oxide that reacts with water to form an acid NO2 + H2O  HNO3 (H+ + NO3-) CO2 + H2O  H2CO3(aq) SO2 + H2O  H2SO3 SO3 + H2O  H2SO4 No luster Brittle

  6. D. Nonmetal Group Trends Pure nonmetals can often exist as allotropes Allotropes – Pure element with different molecular structures and different characteristics Examples Carbon Phosphorus Oxygen Sulfur Hydrogen Diatomic gas at room temp Ionization energy is HIGHER than alkali metals, due to a lack of shielding Alkali metals lose electrons in bonding, When hydrogen combines with alkali metals, it is REDUCED to become an H-1 ion (unstable) With nonmetals, it loses and electron, like a metal Graphite Diamond P4 (white) Px (red) Dioxygen (O2) Ozone (O3) Yellow (S8) Plastic (Sx)

  7. Oxygen Peroxides are unstable Will decay to create both O2 and O-2 H2O2 H2O + O2 Nitrogen In pure form is triple bonded Highly unreactive Halogens (Group 17) All diatomic in pure form F2 and Cl2 = gases Br2 = Liquid I2 = solid (sublimes at room temperature)

  8. 4. Noble Gases MONOATOMIC gases at room temperature They consist of one atom alone Noble gases have filled s and p sublevels (full octet) (He is full with only 2 electrons – full s) Some noble gases (Kr, Xe, Ar) have been forced to react with fluorine, because of its strong ability to attract e- 5. Transition Elements Elements with unfilled d-sublevels (Groups 3 – 11) Multiple oxidation states React by using electrons from several energy levels (valence + core) Make colored solutions

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