Final answer:
The question asks to sketch Lewis structures of carbonic acid, sodium chloride, calcium chloride, sodium hydroxide, and barium hydroxide. For compounds like NaCl, CaCl₂, and NaOH, the structures reflect the transfer of electrons leading to ionic bonds. For molecular compounds like carbonic acid, the structure shows covalent bonding and lone pairs of electrons.
Step-by-step explanation:
The student is inquiring about how to sketch the Lewis structures of several chemical compounds. To sketch these structures accurately, it is important to understand how atoms bond and how they share or transfer electrons.
- H₂CO₃ (carbonic acid): The central carbon atom forms two single bonds with two oxygen atoms and one double bond with another oxygen atom, which carries two lone pairs of electrons. Each hydrogen attaches to the single-bonded oxygen atoms.
- NaCl (sodium chloride): This ionic compound is formed by the transfer of one electron from sodium to chlorine, resulting in a sodium cation (Na+) and a chlorine anion (Cl-).
- CaCl₂ (calcium chloride): Calcium transfers two electrons, one to each chlorine atom, forming Ca2+ and two Cl− ions.
- NaOH (sodium hydroxide): Na+ forms an ionic bond with OH−, where the oxygen atom is covalently bonded to a hydrogen atom and carries a lone pair of electrons.
- Ba(OH)₂ (barium hydroxide): Barium donates two electrons, one to each hydroxide ion (OH−), resulting in Ba2+ and two hydroxide ions each with the oxygen bonded to hydrogen and carrying lone pairs of electrons.
Lewis structures are important for predicting the molecular geometry, reactivity, and other properties of compounds.