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61 Cards in this Set
- Front
- Back
Main-Group Elements
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Elements whose valence electrons fill an s or p orbital sublevel (Groups 1, 2, 13-18)
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Elements found in the earth's atmosphere
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oxygen, nitrogen, and hydrogen
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Ores
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how metals are found naturally in the earth's crust (metal + oxygen)
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Metallurgy
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process of obtaining a metal from its core. It always involves the reduction of ions to the elemental metal (oxidation number of zero)
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Physical characteristics of hydrogen
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colorless, odorless, gas
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Boiling point of hydrogen
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low
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Melting Point of Hydrogen
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low
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Flammability of hydrogen
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high (Hindenburg)
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Ways to produce hydrogen gas
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reaction of methane with water at high temps (and metal catalyst), and eletrolysis of water
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Industrial uses of hydrogen
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production of ammonia via Haber process and to saturate liquid vegetable oils
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Compounds formed with Hydrogen
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ionic hydrides (Group 1/2), Covalent Hydrides (nonmentals), metallic hydrides (transition metals)
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Possible way to store hydrogen as a fuel
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metallic hydrides
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Source of Lithium
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Silicate Minerals such as spodumene (LiAl(Si2O6))
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Method of Preparation of Lithium
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Electrolysis of molten LiCl
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Source of Sodium
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NaCl
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Method of Preparation of Sodium
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Electrolysis of molten NaCl
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Source of Potassium
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KCl
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Method of Preparation of Potassium
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Electrolysis of molten KCl
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Two Group 1 elements in the human body
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Potassium and Sodium
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Source of Rubidium
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Impurity in lepidolite, Li2(F,OH)2Al2(SiO3)3
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Method of Preparation of Rubidium
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Reduction of RbOH with Mg and H2
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Source of Cesium
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Pollucite (Cs4Al4Si9O26·H2O) and an impurity in lepidolite (Li2(F,OH)2Al2(SiO3)3)
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Method of Preparation of Cesium
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Reduction of CsOH with Mg an H2
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2M + X2 →
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2MX; Alkali Metals; X2 = Any halogen molecule
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4Li + O2 →
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2Li2O; Excess oxygen; Alkali Metals
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2Na + O2 →
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Na2O2; Alkali Metals
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M + O2 →
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MO2; M = K, Rb, or Cs; Alkali Metals
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2M + S →
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M2S; Alkali Metals
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6Li + N2 →
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2Li3N; Li only; Alkali Metals
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12M + P4 →
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4M3P; Alkali Metals
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2M + H2 →
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2MH; Alkali Metals
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2M + 2H2O →
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2MOH + H2; Alkali Metals
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2M + 2H+ →
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2M+ + H2; Alkali Metals; Violent reaction!
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Group 2 ions essential for human life
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Calcium (bones) and Magnesium (Metabolism, Muscle)
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Hard Water
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Prescence of Ca2+ and Mg2+ ions in water, which interferes with actions of detergents and form precipitates with soap ; pass through limestone
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Group 2 Trend in Ionization Energy
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Decreasing vertically
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Grou two trend in radius
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Increasing vertically
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Energy of metallurgy redox reaction
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Decreasing vertically
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Source of Beryllium
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Beryl (Be3Al2Si6O18)
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Method of Preparation of Beryllium
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Electrolysis of molten BeCl2
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Source of Magnesium
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magnesite (MgCO3), Dolomite (MgCO3·CaCO3), Carnallite (MgCl2·KCl· 6H2O)
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Preparation of Magnesium
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Electrolysis of molten MgCl2
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Kidney stones from this element
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Calcium
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Source of Calcium
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Various minerals containing CaCO3 (like marble and limestone)
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Preparation of Calcium
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Electrolysis of molten CaCl2
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Source of Strontium
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Celestite (SrSO4), Strontianite (SrCO3)
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Preparation of Strontium
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Electrolysis of molten SrCl2
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Source of Barium
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Baryte (BaSO4), Witherite (BaCO3)
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Preparation of Barium
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Electrolysis of motlen BaCl2
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Source of Radium
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Pitchblende (1 g of Ra/7 tons of ore)
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Preparation of Radium
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Electrolysis of molten RaCl2
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Elements from Pitchblende
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Radium, Uranium
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M + X2 →
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MX; Group 2A Elements; X2 = Any halogen molecule
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2M + O2 →
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2MO; Group 2A Elements; Ba gives BaO2 as well
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M + S →
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MS; Group 2A Elements
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2M + N2 →
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M3N2; Group 2A Elements; High temperatures
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6M + P4 →
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2M3P2; Group 2A Elements; High Temperatures
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M + H2 →
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MH2; Group 2A Elements; M = Ca, Sr, or Ba; High temperatures; Mg at high pressure
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2M + 2H2O →
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M(OH)2 + H2; Group 2A Elements; M = Ca, Sr, or Ba
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M + 2H+ →
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M2+ + H2; Group 2A Elements
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Be + 2OH- + 2H2O →
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Be(OH)42- + H2; Group 2A Elements
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