E.g.3 carbonate ion CO2- Step 1:deduce the skeletal structure of the carbonate ion by recognizing that C is less electronegative than O: Step 2:The outer-shell electron configurations of C and O are 2s22p2 and 2s22p4,respectively,and the ion itself has two negative charges.Thus,the total number of electrons is 4+(3X6)+2 24. Step 3:draw a single covalent bond between C and each O and comply with the octet rule for the O atoms::. Step 4:Although the octet rule is satisfied for the O atoms,it is not for the C atom. Therefore,move a lone pair from one of the O atoms to form another bond with C.The octet rule is also satisfied for the C atom: Step 2: The outer-shell electron configurations of C and O are 2s22p2 and 2s22p4 , respectively, and the ion itself has two negative charges. Thus, the total number of electrons is 4+(3×6)+2 = 24. Step 4: Although the octet rule is satisfied for the O atoms, it is not for the C atom. Therefore, move a lone pair from one of the O atoms to form another bond with C. The octet rule is also satisfied for the C atom: E.g. 3 carbonate ion CO3 2- Step 1: deduce the skeletal structure of the carbonate ion by recognizing that C is less electronegative than O: Step 3: draw a single covalent bond between C and each O and comply with the octet rule for the O atoms: