{"id":30,"date":"2023-04-01T12:25:31","date_gmt":"2023-04-01T12:25:31","guid":{"rendered":"http:\/\/localhost\/solvefor2\/?p=30"},"modified":"2023-04-01T12:29:46","modified_gmt":"2023-04-01T12:29:46","slug":"chemical-formulae-and-equations-summary-notes","status":"publish","type":"post","link":"https:\/\/edu.co.tz\/notes\/chemical-formulae-and-equations-summary-notes\/","title":{"rendered":"CHEMICAL FORMULAE AND EQUATIONS SUMMARY NOTES"},"content":{"rendered":"

CHEMICAL FORMULAE AND EQUATIONS
\n<\/strong><\/span><\/p>\n

\n\u00a0<\/p>\n

The formulae of compounds are written from the name of ions of atoms and the charge on the ions of atoms combined together.
\n<\/span><\/p>\n

There are two ways of writing the formulae of compounds:
\n<\/span><\/p>\n

    \n
  1. \n
    Prefix method
    \n<\/strong><\/span><\/div>\n

    Prefixes are used to indicate the number of atoms present in a compound.
    \n<\/span><\/p>\n<\/li>\n<\/ol>\n

      \n
    • Mono- = 1
      \n<\/span><\/li>\n
    • Di- = 2
      \n<\/span><\/li>\n
    • Tri- = 3
      \n<\/span><\/li>\n
    • \n
      Tetra- = 4
      \n<\/span><\/div>\n

      Examples
      \n<\/span><\/p>\n

      Carbon monoxide (CO)
      \n<\/span><\/p>\n

      Carbon dioxide (CO2<\/sub>)
      \n<\/span><\/p>\n

      Sulphur dioxide (SO2<\/sub>)
      \n<\/span><\/p>\n

      Sulphur trioxide (SO3<\/sub>)
      \n<\/span><\/p>\n

      Dinitrogen monoxide (
      \n<\/span><\/p>\n

      Dinitrogen pent oxide (
      \n<\/span><\/p>\n

      \n\u00a0<\/p>\n

      \n\u00a0<\/p>\n

      \n\u00a0<\/p>\n

      \n\u00a0<\/p>\n

      \n\u00a0<\/p>\n

      \n\u00a0<\/p>\n

      \n\u00a0<\/p>\n

      \n\u00a0<\/p>\n

      \n\u00a0<\/p>\n

      \n\u00a0<\/p>\n<\/li>\n<\/ul>\n

        \n
      1. \n
        Valency method
        \n<\/strong><\/span><\/div>\n

        This is when valences of atoms, ions or radicals (compound ions) are used to determine the proportions of atoms in a compound.
        \n<\/span><\/p>\n

        \n\u00a0<\/p>\n

        Negative ions (anions)
        \n<\/span><\/p>\n

        \n\u00a0<\/p>\n<\/li>\n<\/ol>\n

        \n\n\n\n\n<\/colgroup>\n\n\n\n\n\n\n\n\n\n\n
        \n

        Name of ion<\/strong><\/span><\/p>\n<\/td>\n

        		\n

        formulae<\/strong><\/span><\/p>\n<\/td>\n

        		\n

        Valency<\/strong><\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        Fluoride<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Chloride<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Sulphide<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        oxide<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Nitride<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Phosphide<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        iodide<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        bromide<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n

        \n\u00a0<\/p>\n

        Positive ions (cations)
        \n<\/span><\/p>\n

        \n\u00a0<\/p>\n

        \n\n\n\n\n<\/colgroup>\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n
        \n

        Name of ion<\/strong><\/span><\/p>\n<\/td>\n

        		\n

        formulae<\/strong><\/span><\/p>\n<\/td>\n

        		\n

        valency<\/strong><\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        silver<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\n

        1<\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        Sodium<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Potassium<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Copper I<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Copper II<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Zinc<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Calcium<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Magnesium<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Lead II<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Lead IV<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Iron II<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Iron III<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Barium<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Aluminium<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Cobalt II<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n
        \n

        Gold III<\/span><\/p>\n<\/td>\n

        		\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n

        \n\u00a0<\/p>\n

        Polyatomic ions\/compound ions\/radicals
        \n<\/strong><\/span><\/p>\n

        \n\u00a0<\/p>\n

        \n\n\n\n\n<\/colgroup>\n\n\n\n\n\n\n\n\n\n\n\n\n\n
        \n

        Name of ion<\/strong><\/span><\/p>\n<\/td>\n

        		\n

        Formulae<\/strong><\/span><\/p>\n<\/td>\n

        		\n

        valency<\/strong><\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        hydroxide<\/span><\/p>\n<\/td>\n

        		\n

        OH–<\/sup><\/span><\/p>\n<\/td>\n

        		\n

        1<\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        nitrate<\/span><\/p>\n<\/td>\n

        		\n

        NO3<\/sub>–<\/sup><\/span><\/p>\n<\/td>\n

        		\n

        1<\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        nitrite<\/span><\/p>\n<\/td>\n

        		\n

        NO2<\/sub>–<\/sup><\/span><\/p>\n<\/td>\n

        		\n

        1<\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        Sulphate <\/span><\/p>\n<\/td>\n

        		\n

        SO4<\/sub>2-<\/sup><\/span><\/p>\n<\/td>\n

        		\n

        2<\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        sulphite<\/span><\/p>\n<\/td>\n

        		\n

        SO3<\/sub>2-<\/sup><\/span><\/p>\n<\/td>\n

        		\n

        2<\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        carbonate<\/span><\/p>\n<\/td>\n

        		\n

        CO3<\/sub>2-<\/sup><\/span><\/p>\n<\/td>\n

        		\n

        2<\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        phosphate<\/span><\/p>\n<\/td>\n

        		\n

        PO4<\/sub>3-<\/sup><\/span><\/p>\n<\/td>\n

        		\n

        3<\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        Hydrogen carbonate<\/span><\/p>\n<\/td>\n

        		\n

        HCO3<\/sub>–<\/sup><\/span><\/p>\n<\/td>\n

        		\n

        1<\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        Phosphit5e<\/span><\/p>\n<\/td>\n

        		\n

        PO3<\/sub>3-<\/sup><\/span><\/p>\n<\/td>\n

        		\n

        3<\/span><\/p>\n<\/td>\n<\/tr>\n

        \n

        ammonium<\/span><\/p>\n<\/td>\n

        		\n

        NH4<\/sub>+<\/sup><\/span><\/p>\n<\/td>\n

        		\n

        1<\/span><\/p>\n<\/td>\n<\/tr>\n

        \u00a0<\/td>\n\u00a0<\/td>\n\u00a0<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n

        \n\u00a0<\/p>\n

        Examples
        \n<\/span><\/p>\n

        Write the formula of the following compounds
        \n<\/span><\/p>\n

          \n
        1. Sodium hydroxide
          \n<\/span><\/li>\n
        2. Calcium oxide
          \n<\/span><\/li>\n
        3. Aluminium oxide
          \n<\/span><\/li>\n
        4. Magnesium nitrate
          \n<\/span><\/li>\n
        5. Potassium phosphate
          \n<\/span><\/li>\n
        6. Ammonium carbonate
          \n<\/span><\/li>\n
        7. Copper II chloride
          \n<\/span><\/li>\n<\/ol>\n

          \n\u00a0<\/p>\n

          Exercise
          \n<\/span><\/p>\n

          Write the formula of the following compounds
          \n<\/span><\/p>\n

            \n
          1. Manganese IV oxide
            \n<\/span><\/li>\n
          2. Calcium phosphate
            \n<\/span><\/li>\n
          3. Copper II sulphate
            \n<\/span><\/li>\n
          4. Magnesium sulphite
            \n<\/span><\/li>\n
          5. Lead II nitrate
            \n<\/span><\/li>\n
          6. Sodium phosphate
            \n<\/span><\/li>\n
          7. Iron III phosphate
            \n<\/span><\/li>\n
          8. Magnesium hydrogen carbonate
            \n<\/span><\/li>\n
          9. aluminium sulphate
            \n<\/span><\/li>\n
          10. zinc hydroxide
            \n<\/span><\/li>\n
          11. ammonium sulphate
            \n<\/span><\/li>\n
          12. lithium oxide
            \n<\/span><\/li>\n<\/ol>\n

            \n\u00a0<\/p>\n

            EQUATIONS
            \n<\/strong><\/span><\/p>\n

            There are two parts to an equation, which are reactants and products. The two are separated by an arrow. Reactants are found on the left hand side and products on the right hand side
            \n<\/span><\/p>\n

            There are two ways to write equations of chemical reactions.
            \n<\/span><\/p>\n

              \n
            1. \n
              Word equations
              \n<\/span><\/div>\n

              A word equation is written in words
              \n<\/span><\/p>\n

              Examples
              \n<\/span><\/p>\n

                \n
              1. Sodium chloride + magnesium nitrate \u2192 sodium nitrate + magnesium chloride
                \n<\/span><\/li>\n
              2. Calcium phosphate + aluminium sulphate \u2192
                \n<\/span><\/li>\n
              3. Potassium fluoride + sodium carbonate \u2192
                \n<\/span><\/li>\n
              4. Lead ii chloride + potassium iodide \u2192
                \n<\/span><\/li>\n
              5. Ammonium hydroxide + copper II sulphate \u2192
                \n<\/span><\/li>\n
              6. \n
                Zinc chloride + sodium hydroxide \u2192
                \n<\/span><\/div>\n

                \n\u00a0<\/p>\n<\/li>\n<\/ol>\n<\/li>\n

              7. \n
                Symbolic equations
                \n<\/span><\/div>\n

                These are equations where symbols or formulas of compounds are used.
                \n<\/span><\/p>\n

                Examples
                \n<\/span><\/p>\n

                Rewrite the following word equations as symbolic equations.
                \n<\/span><\/p>\n

                \n\u00a0<\/p>\n

                \n\u00a0<\/p>\n

                \n\u00a0<\/p>\n

                \n\u00a0<\/p>\n

                \n\u00a0<\/p>\n

                \n\u00a0<\/p>\n

                \n\u00a0<\/p>\n

                \n\u00a0<\/p>\n

                \n\u00a0<\/p>\n

                \n\u00a0<\/p>\n

                BALANCING OF EQUATIONS
                \n<\/span><\/p>\n

                Rules for balancing equations
                \n<\/span><\/p>\n

                  \n
                1. Count the atoms on each side of the equation
                  \n<\/span><\/li>\n
                2. If the number of each type of an atom on either side of the equation is not the same, we have to balance the equation.
                  \n<\/span><\/li>\n
                3. In balancing of equations put big numbers at the back of the formula which contains atoms that do not balance.
                  \n<\/span><\/li>\n
                4. \n
                  Carry on until the atoms on each side of the equation are the same
                  \n<\/span><\/div>\n

                  NB: Only symbolic equations could be balanced.
                  \n<\/span><\/p>\n

                  \n\u00a0<\/p>\n

                  \n\u00a0<\/p>\n

                  Common acids
                  \n<\/strong><\/span><\/p>\n

                  Hydrochloric acid HCl
                  \n<\/span><\/p>\n

                  Sulphuric acid H2<\/sub>SO4<\/sub>
                  \n\t\t\t\t\t\t<\/span><\/p>\n

                  Nitric acid HNO3<\/sub>
                  \n\t\t\t\t\t\t<\/span><\/p>\n

                  Carbonic acid H2<\/sub>CO3<\/sub>
                  \n\t\t\t\t\t\t<\/span><\/p>\n

                  Phosphoric acid H3<\/sub>PO4
                  \n<\/sub><\/span><\/p>\n

                  \n\u00a0<\/p>\n

                  \n\u00a0<\/p>\n

                  \n\u00a0<\/p>\n

                  \n\u00a0<\/p>\n

                  Common di-atomic molecules
                  \n<\/strong><\/span><\/p>\n

                  \n\u00a0<\/p>\n<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n

                    \n
                  • Hydrogen H2<\/sub>
                    \n\t\t\t<\/span><\/li>\n
                  • Oxygen O2<\/sub>
                    \n\t\t\t<\/span><\/li>\n
                  • Nitrogen N2<\/sub>
                    \n\t\t\t<\/span><\/li>\n
                  • Chlorine Cl2<\/sub>
                    \n\t\t\t<\/span><\/li>\n
                  • Fluorine F2<\/sub>
                    \n\t\t\t<\/span><\/li>\n
                  • Bromine Br2<\/sub>
                    \n\t\t\t<\/span><\/li>\n
                  • \n
                    Iodine I2<\/sub>
                    \n\t\t\t\t<\/span><\/div>\n

                    \n\u00a0<\/p>\n

                    \n\u00a0<\/p>\n

                    Examples
                    \n<\/span><\/p>\n

                    Balance the following equations
                    \n<\/span><\/p>\n<\/li>\n<\/ul>\n

                      \n
                    1. \n\t\t<\/li>\n<\/ol>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      Ionic equations
                      \n<\/strong><\/span><\/p>\n

                      These are equations which show the ions which take part in a chemical reaction.
                      \n<\/span><\/p>\n

                      Ions which do not take part in a chemical reaction are called SPECTATOR IONS.
                      \n<\/strong><\/span><\/p>\n

                      \n\u00a0<\/p>\n

                      \n\n\n\n<\/colgroup>\n\n\n\n\n\n\n
                      \n

                      STATE symbol<\/strong><\/span><\/p>\n<\/td>\n

                      		\n

                      Physical states (state symbol) meaning<\/strong><\/span><\/p>\n<\/td>\n<\/tr>\n

                      \n

                      g<\/span><\/p>\n<\/td>\n

                      		\n

                      Gaseous substance<\/span><\/p>\n<\/td>\n<\/tr>\n

                      \n

                      l<\/span><\/p>\n<\/td>\n

                      		\n

                      Liquid<\/span><\/p>\n<\/td>\n<\/tr>\n

                      \n

                      s<\/span><\/p>\n<\/td>\n

                      		\n

                      Solid (insoluble substance) precipitates<\/span><\/p>\n<\/td>\n<\/tr>\n

                      \n

                      aq<\/span><\/p>\n<\/td>\n

                      		\n

                      Aqueous (substance that are soluble in water\/dissolved in water)<\/span><\/p>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n

                      \n\u00a0<\/p>\n

                      \n\u00a0<\/p>\n

                      SOLUBILTY RULES
                      \n<\/strong><\/span><\/p>\n

                        \n
                      1. All acids are soluble
                        \n<\/span><\/li>\n
                      2. All nitrates are soluble
                        \n<\/span><\/li>\n
                      3. All sulphates are soluble EXCEPT BaSO4<\/sub>, CaSO4<\/sub>, PbSO4<\/sub>
                        \n\t\t\t<\/span><\/li>\n
                      4. All chlorides, Iodides, Bromides are soluble except for silver, lead and mercury.
                        \n<\/span><\/li>\n
                      5. All carbonates are INSOLUBLE except those formed by group 1 elements and ammonium carbonate, (NH4<\/sub>)2<\/sub>CO3<\/sub>.
                        \n<\/span><\/li>\n
                      6. \n
                        All hydroxides and oxides are insoluble except those formed by group 1 elements and ammonium.
                        \n<\/span><\/div>\n

                        \n\u00a0<\/p>\n

                        NB: All ammonium compounds are soluble
                        \n<\/span><\/p>\n

                        All compounds formed by group 1 are soluble
                        \n<\/span><\/p>\n

                        \n\u00a0<\/p>\n

                        HOW TO WRITE AN IONIC EQUATION
                        \n<\/strong><\/span><\/p>\n

                        \n\u00a0<\/p>\n

                          \n
                        1. Write a balanced chemical equation
                          \n\t\t\t\t\t\t\t<\/strong><\/span><\/span><\/li>\n
                        2. Put state symbol into the equation
                          \n\t\t\t\t\t\t\t<\/strong><\/span><\/span><\/li>\n
                        3. Break down\/separate the aqueous substances into ions. PLEASE DO NOT BREAK DOWN, SOLIDS, LIQUIDS AND GASES.
                          \n\t\t\t\t\t\t\t<\/span><\/strong><\/span><\/li>\n
                        4. Cancel out those ions which appear on both sides of the equation (spectator ions)
                          \n\t\t\t\t\t\t\t<\/span><\/strong><\/span><\/li>\n
                        5. \n
                          What remains is the net ionic equation
                          \n\t\t\t\t\t\t\t\t<\/strong><\/span><\/span><\/div>\n

                          \n\u00a0<\/p>\n

                          Examples <\/span><\/p>\n<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"

                          CHEMICAL FORMULAE AND EQUATIONS \u00a0 The formulae of compounds are written from the name of ions of atoms and the<\/p>\n","protected":false},"author":1,"featured_media":305,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[4,1],"tags":[],"class_list":["post-30","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-chemistry","category-uncategorized"],"yoast_head":"\nCHEMICAL FORMULAE AND EQUATIONS SUMMARY NOTES - MAKTABA EDUCATION CENTER<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/edu.co.tz\/notes\/chemical-formulae-and-equations-summary-notes\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"CHEMICAL FORMULAE AND EQUATIONS SUMMARY NOTES - 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