inorganic facts

    Cards (84)

    • sodium and magnesium oxides form an alkaline solution when they react with water because they contain O(2-) ions which react with the water to produce OH(-) ions
      the equation is O(2-) + H2O -> 2OH(-)
    • each period has the same general pattern for ionisation energy, an increase of 2, then 3, then 3
    • Mg(OH)2 is sparingly soluble
      Ba(OH)2 is the most soluble
    • Mg(OH)2 is used in medicine as an antacid because it is alkaline so neutralises stomach acid
    • Ca(OH)2 is used in agriculture to neutralise acidic soil because it is alkaline
    • MgSO4 is the most soluble
      BaSO4 is the least soluble
    • BaSO4 is used in medicine as barium meals to outline soft tissue in X-rays, it is toxic if it enters the bloodstream but because it is insoluble it cannot do so
    • test for sulfates:
      • acidify with nitric or hydrochloric acid
      • add barium chloride
      • positive = white precipitate
    • the equation for magnesium being used in the extraction of titanium is:
      TiCl4 + 2Mg -> 2MgCl2 + Ti
    • the equation for flue gas desulfurisation is:
      CaO + 2H2O + SO2 -> CaSO3 + 2H2O
      or
      CaCO3 + 2H2O + SO2 -> CaSO3 + 2H2O + CO2
    • of the halogens:
      fluorine is the most powerful oxidising agent
      iodine is the least powerful oxidising agent
    • of the halide ions:
      fluoride is the least powerful reducing agent
      iodide is the most powerful reducing agent
    • equation for sodium fluoride reacting with conc sulfuric acid:
      NaF + H2SO4 -> NaHSO4 + HF
    • equation for sodium chloride reacting with conc sulfuric acid:
      NaCl + H2SO4 -> NaHSO4 + HCl
    • equations for sodium bromide reacting with conc sulfuric acid:
      NaBr + H2SO4 -> NaHSO4 + HBr
      2H+ + 2Br- + H2SO4 -> SO2 + 2H2O + Br2
    • equation for sodium iodide reacting with conc sulfuric acid:
      NaI + H2SO4 -> NaHSO4 + HI
      8H+ + 8I- + H2SO4 -> 4H2O + H2S + 4I2
    • the test for halide ions is:
      • add dilute nitric acid HNO3 and silver nitrate AgNO3
      • results: Cl = white ppt, Br = cream ppt, I = yellow ppt
      • add dilute ammonia NH3
      • results: Cl ppt dissolves, Br and I ppts do not dissolve
      • add concentrated ammonia NH3
      • results: Cl and Br ppts dissolve, I ppt does not dissolve
    • the equations for chlorine reacting with cold water are:
      Cl2 + H2O <-> HClO + HCl
      Cl2 + H2O <-> ClO(-) + Cl(-) + 2H(+)
    • the equation for chlorine reacting with water in the presence of sunlight/UV light is:
      2Cl2 + 2H2O -> 4HCl + O2
    • the equation for sodium chlorate reacting with water is:
      NaClO + H2O -> Na(+) + OH(-) + HClO
    • the equation for chlorine reacting with sodium hydroxide is:
      Cl2 + 2NaOH -> NaClO + NaCl + H2O
    • equation for Na reacting with water:
      2Na + 2H2O -> 2NaOH + H2
    • equation for Mg reacting with water:
      Mg + 2H2O -> Mg(OH)2 + H2
    • equation for Mg reacting with steam:
      Mg + H2O -> MgO + H2
    • equation for production of sodium oxide:
      2Na + 1/2(O2) -> Na2O
    • equation for production of magnesium oxide:
      2Mg + O2 -> 2MgO
    • equation for production of aluminium oxide:
      4Al + 3O2 -> 2Al2O3
    • equation for production of silicon dioxide:
      Si + O2 -> SiO2
    • equation for production of phosphorus pentoxide:
      4P + 5O2 -> P4O10
    • equation for production of sulfur dioxide and sulfur trioxide:
      S + O2 -> SO2 + small amount of SO3
    • the order of melting points of period 3 oxides is:
      MgO > Al2O3 > SiO2 > Na2O > P4O10 > SO3 > SO2
    • equation for magnesium oxide reacting with water:
      MgO + H2O -> Mg(OH)2
    • equation for sodium oxide reacting with water:
      Na2O + H2O -> 2NaOH
    • equation for phosphorus pentoxide reacting with water:
      P4O10 + 6H2O -> 4H3PO4
    • equation for sulfur dioxide reacting with water:
      SO2 + H2O -> H2SO3
    • equation for sulfur trioxide reacting with water:
      SO3 + H2O -> H2SO4
    • when period 3 elements react with oxygen, you would observe:
      • Na = yellow-orange flame, white solid
      • Mg = white flame, white solid
      • Al = white flame, white powder
      • Si = white flame, white powder
      • P = white flame, white fumes
      • S = blue flame, fumes
    • examples of monodentate ligands are H2O, NH3 and Cl-
    • examples of bidentate ligands are H2NCH2CH2NH2 and C2O4(2-)
    • examples of multidentate ligands are EDTA(4-)