In the Lewis structure of LiCl, lithium (Li) loses one electron to achieve a stable octet configuration, becoming a positively charged lithium ion (Li+). Chlorine (Cl) gains this electron to complete its outer shell, forming a negatively charged chloride ion (Cl-). The electrostatic attraction between these oppositely charged ions results in the formation of LiCl, an ionic compound with a linear molecular structure. The Lewis structure depicts the transfer of electrons, highlighting the ionic bond between Li and Cl, emphasizing the significance of achieving stable electron configurations in chemical bonding.
