Which of the following statements is true regarding sodium and chloride ions?

Sodium and chloride ions have opposite charges, with sodium typically losing one electron to become a positively charged ion (Na⁺), while chloride gains an electron to become a negatively charged ion (Cl⁻). The electrostatic attraction between these oppositely charged ions leads to the formation of an ionic bond, which is characterized by a strong interaction between the ions. This type of bonding results in the formation of sodium chloride (table salt), which is a classic example of ionic compounds.

Ionic bonds are typically formed between metals and nonmetals, where the metal ion donates electrons, and the nonmetal accepts them. In the case of sodium chloride, this transfer of electrons and the resulting ionic bond account for the high melting and boiling points of ionic compounds, as well as their crystalline structure in solid form.

In contrast, other given options do not accurately describe the nature of sodium and chloride ions. For instance, similar charges would not lead to an attraction between the ions, and covalent bonding would involve sharing of electrons rather than transfer. Additionally, sodium chloride does not exist as a gas at room temperature; it is a solid due to strong ionic interactions.