Final answer:
The Lewis structures for H₂S, CO, N₂, and O₃ show the distribution of valence electrons among the atoms, representing single, double, or triple bonds as well as lone pairs of electrons.
Step-by-step explanation:
Writing Lewis structures for molecules and ions is a way to represent the arrangement of valence electrons around atoms. Here are the Lewis structures for the requested substances:
- H₂S: The sulfur atom has six valence electrons and hydrogen has one valence electron each. Sulfur is at the center with two single bonds connecting to hydrogen atoms, leaving four non-bonding electrons on the sulfur to complete its octet.
- CO: Carbon monoxide has a triple bond between the carbon and oxygen atoms with a lone pair of electrons on the oxygen atom. Carbon has six electrons around it, accounting for the triple bond and a lone pair, whereas oxygen has eight, including the triple bond and two lone pairs.
- N₂: Nitrogen gas consists of two nitrogen atoms sharing a triple bond, with each nitrogen also having one lone pair of electrons to complete its octet.
- O₃ (ozone): Ozone is a bent molecule with an oxygen atom in the center forming a double bond with one oxygen on the end and a single bond with the other end oxygen atom, which has a negative charge. The central oxygen atom also has a lone pair of electrons.