Which of the following is true about ionic compounds?

Ionic compounds are formed through the transfer of electrons, typically between metals and nonmetals. In this process, metals lose electrons to form positively charged ions (cations), while nonmetals gain those electrons to form negatively charged ions (anions). This transfer of electrons leads to strong electrostatic forces of attraction between the oppositely charged ions, which is a defining characteristic of ionic bonding.

The formation of ionic compounds involves a clear interaction between the different electronegativities of metals and nonmetals, which is why they are primarily formed between these types of elements. This principle is foundational in chemistry and highlights the nature of ionic compounds in contrast to covalent compounds, where atoms share electrons.

In contrast, options describing ionic compounds having low melting points, being gases, or sharing electrons do not align with their characteristics. Ionic compounds are typically solid at room temperature and exhibit high melting points due to the strong ionic bonds that hold the lattice structure together. Additionally, in ionic bonding, atoms do not share electrons; rather, the transfer of electrons is what defines the ionic nature of the compound.