2<\/sub>O, the subscript 2 indicates 2 atoms of hydrogen. In the formula of water, oxygen O is written without a subscript and it indicates 1 atoms of oxygen.<\/li>\n<\/ol>\nTable: Chemical formulae of some compounds<\/strong><\/p>\n\n\n\nCompound<\/strong><\/td>\nChemical formula<\/strong><\/td>\nMeaning of chemical formula<\/strong><\/td>\n<\/tr>\n\nElements present<\/strong><\/td>\nRatio of the number of atoms of elements<\/strong><\/td>\n<\/tr>\n\nWater<\/td>\n | H2<\/sub>O<\/td>\nHydrogen, oxygen<\/td>\n | H:O = 2:1<\/td>\n<\/tr>\n | \nAmmonia<\/td>\n | NH3<\/sub><\/td>\nNitrogen, hydrogen<\/td>\n | N:H = 1:3<\/td>\n<\/tr>\n | \nSulphuric acid<\/td>\n | H2<\/sub>SO4<\/sub><\/td>\nHydrogen, sulphur, oxygen<\/td>\n | H:S:O = 2:1:4<\/td>\n<\/tr>\n | \nZinc hydroxide<\/td>\n | Zn(OH)2<\/sub><\/td>\nZinc, oxygen, hydrogen<\/td>\n | Zn:O:H = 1:2:2<\/td>\n<\/tr>\n | \nMagnesium nitrate<\/td>\n | Mg(NO3<\/sub>)2<\/sub><\/td>\nMagnesium, nitrogen, oxygen<\/td>\n | Mg;N;O = 1:2:6<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\nRules for writing a chemical formula<\/b><\/strong><\/h2>\n\n- We first write the symbols of the elements which form the compound<\/li>\n
- Below the symbol of each element, we write down its valency.<\/li>\n
- Finally, we cross-over the valencies of the combining atoms. That is, with first atom we write the valency of second atom (as a subscript); and with the second atom we write the valency of first atom (as subscript).<\/li>\n<\/ol>\n
Example 1:<\/b><\/strong> \n \nExample 2:<\/b><\/strong> \n \nExample 3:<\/b><\/strong> \n \nExample 4:<\/b><\/strong> \n \nExample 5:<\/b><\/strong> \n<\/p>\nWriting the formula of a compound<\/b><\/strong><\/h2>\nStep-1 : <\/b><\/strong> \nWrite the symbols of formulae of the ions of the compound side by side with positive ion on the left hand side and negative ion on right hand side. \nStep-2 : <\/b><\/strong> \nEnclose the polyatomic ion in a bracket. \nStep-3 : <\/b><\/strong> \nWrite the valency of each ion below its symbol \nStep-4 : <\/b><\/strong> \nReduce the valency numerals to a simple ratio by dividing with a common factor, if any. \nStep-5 : <\/b><\/strong> \nCross the valencies. Do not write the charges positive or negative of the ions. \nExample:\u00a0<\/b><\/strong>Formula of barium nitrate. \nStep-1<\/b><\/strong> :<\/b><\/strong> Writing the formula of the ions : \nBa2+<\/sup>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 NO3<\/sub>\u2013<\/sup> \nStep-2 :<\/b><\/strong>\u00a0 \u00a0Ba2+<\/sup>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 (NO3<\/sub>)\u2013<\/sup> \nStep-3 :<\/b><\/strong>\u00a0 \u00a0Ba2+<\/sup>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 (NO3<\/sub>)\u2013<\/sup> \n2 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a01 \nStep-4 : <\/b><\/strong>Not applicable, because ratio is already simple \nStep-5 : <\/b><\/strong> \n \nThus, the formula of barium nitrate is Ba(NO3<\/sub>)2<\/sub><\/p>\nSignificance of the formula of a substance <\/b><\/strong><\/h2>\n\n- Formula represents the name of the substance.<\/li>\n
- Formula represents one molecule of the substance.<\/li>\n
- Formula also represents one mole of molecules of the substance. That is, formula also represents 6.022 \u00d7 1023<\/sup> molecules of the substance.<\/li>\n
- Formula gives the name of all the elements present in the molecule.<\/li>\n
- Formula gives the number of atoms of each element present in one molecule.<\/li>\n
- Formula represents a definite mass of the substance.<\/li>\n<\/ol>\n
Chemical formulae of ionic compounds<\/h2>\n\n- Ionic compounds consist of cations and anions.
\n(a) Cations are positively-charged ions. \n(b) Anions are negatively-charged ions.<\/li>\n - To construct chemical formulae of ionic compounds, we need to know the formulae of cations and anions.<\/li>\n
- Below tables \u00a0show the formulae of some common cations and anions.
\nTable: Formulae of some common cations.<\/p>\n\n\n\nCharge of cation<\/strong><\/td>\nCation (positive ion)<\/strong><\/td>\nFormula of cation<\/strong><\/td>\n<\/tr>\n\n+ 1<\/td>\n | Sodium ion<\/td>\n | Na+<\/sup><\/td>\n<\/tr>\n\nPotassium ion<\/td>\n | K+<\/sup><\/td>\n<\/tr>\n\nSilver ion<\/td>\n | Ag+<\/sup><\/td>\n<\/tr>\n\nHydrogen ion<\/td>\n | H+<\/sup><\/td>\n<\/tr>\n\nAmmonium ion<\/td>\n | NH4<\/sub>+<\/sup><\/td>\n<\/tr>\n\nCopper(I) ion<\/td>\n | Cu2+<\/sup><\/td>\n<\/tr>\n\n+2<\/td>\n | Calcium ion<\/td>\n | Ca2+<\/sup><\/td>\n<\/tr>\n\nMagnesium ion<\/td>\n | Mg2+<\/sup><\/td>\n<\/tr>\n\nZinc ion<\/td>\n | Zn2+<\/sup><\/td>\n<\/tr>\n\nBarium ion<\/td>\n | Ba2+<\/sup><\/td>\n<\/tr>\n\nIron(II) ion<\/td>\n | Fe2+<\/sup><\/td>\n<\/tr>\n\nCopper(II) ion<\/td>\n | Cu2+<\/sup><\/td>\n<\/tr>\n\nTin(II) ion<\/td>\n | Sn2+<\/sup><\/td>\n<\/tr>\n\nLead(II) ion<\/td>\n | Pb2+<\/sup><\/td>\n<\/tr>\n\n+3<\/td>\n | Iron(III) ion<\/td>\n | Fe3+<\/sup><\/td>\n<\/tr>\n\nAluminium ion<\/td>\n | Al3+<\/sup><\/td>\n<\/tr>\n\nChromium(III) ion<\/td>\n | Cr3+<\/sup><\/td>\n<\/tr>\n\n+4<\/td>\n | Tin(IV) ion<\/td>\n | Sn4+<\/sup><\/td>\n<\/tr>\n\nLead(IV) ion<\/td>\n | Pb4+<\/sup><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n\n\n\nCharge of anion<\/strong><\/td>\nAnion<\/strong> \n (negative ion)<\/strong><\/td>\nFormula of anion<\/strong><\/td>\n<\/tr>\n\n-1<\/td>\n | Fluoride ion<\/td>\n | F–<\/sup><\/td>\n<\/tr>\n\nChloride ion<\/td>\n | cl–<\/sup><\/td>\n<\/tr>\n\nBromide ion<\/td>\n | Br–<\/sup><\/td>\n<\/tr>\n\nIodide ion<\/td>\n | I–<\/sup><\/td>\n<\/tr>\n\nHydroxide ion<\/td>\n | OH–<\/sup><\/td>\n<\/tr>\n\nNitrate ion<\/td>\n | NO3<\/sub>–<\/sup><\/td>\n<\/tr>\n\nNitrite ion<\/td>\n | NO2<\/sub>–<\/sup><\/td>\n<\/tr>\n\n | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | |