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Oxygen atoms love to have eight electrons around them to achieve a stable electron configuration, which is known as the octet rule. After drawing the single bonds, we need to add electrons around the oxygen atoms to complete their octets. Each oxygen atom already has two electrons from the single bond, so it needs six more. Add three lone pairs (each pair has two electrons) to each oxygen atom, completing their octets. This uses up 4 oxygen atoms × 6 electrons/oxygen atom = 24 electrons. Now, let’s check how many electrons we have used so far: 8 electrons (for single bonds) + 24 electrons (to complete oxygen octets) = 32 electrons. This matches the total number of valence electrons we calculated in Step 1, so we are on the right track!
