Final answer:
In the high school chemistry question, Lewis structures are drawn for LiF, Cl₂, NO⁺, and NO⁻, with each exhibiting a unique arrangement and none matching another. LiF has an ionic structure, Cl₂ shows a single covalent bond, while NO⁺ and NO⁻ are shown with double bonds and differing charges.
Step-by-step explanation:
The question:
"Write Lewis structures for the following compounds. Match compounds with the same Lewis structure. All must be correct to get credit.
a. LiF
b. Cl₂
c. NO⁺
d. NO⁻"
involves the creation of Lewis structures for ionic and covalent compounds and ions. Each of these species can be represented using dots for electrons and lines for bonds between atoms.
a. LiF would have the lithium atom with no dots since it's losing one electron to become Li⁺, and the fluorine atom with seven dots around it, indicating the additional electron it gains to become F⁻.
b. Cl₂ is a diatomic molecule, so it will be represented by two chlorine atoms, each having seven dots, sharing a pair of electrons to form a single bond.
c. NO⁺, or nitric oxide cation, would have the nitrogen and oxygen atoms sharing two pairs of electrons (a double bond), with nitrogen having a positive charge due to the removal of one electron.
d. NO⁻, or nitric oxide anion, would have a similar structure to NO⁺ but with an additional lone pair of electrons on the nitrogen, and with nitrogen carrying a negative charge due to the addition of one electron.
Upon reviewing the structures, it can be seen that none of the compounds listed in the question have the same Lewis structure. Each has a unique arrangement of electrons and bonding.
For accuracy and to provide a mentioned correct option in the final answer, it is essential to use the information provided correctly and to ensure that the structures drawn represent the true electronic configuration of each compound or ion.