Final answer:
The Lewis structure for KCl represents potassium donating its single valence electron to chlorine, resulting in K+ and Cl- ions that form the ionic compound potassium chloride. Chlorine gas (Cl₂) has a Lewis structure with a single covalent bond and six lone electrons on each atom.
Step-by-step explanation:
To draw the Lewis structure for the compound formed by potassium (K) and chlorine (Cl), we need to consider the electron configurations of the individual atoms. Potassium, being in group 1 of the periodic table, has one valence electron, while chlorine, in group 17, has seven valence electrons. In forming a compound, potassium can donate its one valence electron to chlorine, resulting in the electron configurations that make both atoms stable.
For K (potassium), the resulting ion is K+, indicating it has lost one electron. Chlorine gains this electron, becoming the Cl− ion. When these ions combine, they form the ionic compound KCl (potassium chloride), which is held together by ionic bonds. The Lewis structure for KCl shows K+ with no dots as it has lost its one valence electron and Cl− surrounded by eight dots, representing its full valence shell.
The electron dot diagram for Cl₂ illustrates two chlorine atoms sharing a pair of valence electrons to form a covalent bond, indicated by a dash between the atoms. Each Cl atom has six additional dots representing the lone pairs of electrons.