The hypochlorite ion, ClO^-, is the active ingredient in bleach. The perchlorate ion, ClO₄^-, is a main component of rocket propellants. Draw Lewis structures for both ions. (c) What is the oxidation number of Cl in the hypochlorite ion? (d) What is the oxidation number of Cl in the perchlorate ion, assuming the Cl—O bonds are all single bonds?

Verified step by step guidance

1. To draw the Lewis structure for the hypochlorite ion (ClO-), start by counting the total number of valence electrons. Chlorine has 7 valence electrons, oxygen has 6, and the negative charge adds 1 more electron, totaling 14 valence electrons.
2. Arrange the atoms with chlorine as the central atom and oxygen bonded to it. Distribute the 14 valence electrons to satisfy the octet rule, starting with the oxygen atom, then the chlorine atom, and finally placing any remaining electrons as lone pairs on the chlorine.
3. For the perchlorate ion (ClO4-), count the total valence electrons: chlorine has 7, each oxygen has 6, and the negative charge adds 1 more, totaling 32 valence electrons. Place chlorine in the center and arrange the four oxygen atoms around it.
4. Distribute the 32 valence electrons among the atoms, starting with the oxygen atoms to satisfy their octets, then place any remaining electrons on the chlorine atom. Consider using double bonds if necessary to satisfy the octet rule for all atoms.
5. To determine the oxidation number of Cl in the hypochlorite ion, assign oxidation states based on the assumption that oxygen is -2. For the perchlorate ion, assume each Cl—O bond is a single bond and assign oxidation states accordingly, keeping in mind the overall charge of the ions.