Final answer:
The correct electron dot structure for KCl is b)⋅:K:⋅↑⋅:Cl:⋅↓, where potassium loses its one valence electron to chlorine, forming K+ and Cl- with a full octet.
Step-by-step explanation:
To choose the correct electron dot structure for KCl, we must understand the electron configurations of potassium (K) and chlorine (Cl) and how they combine to form an ionic compound. Potassium, being in group 1 of the periodic table, has 1 valence electron which it wants to lose to achieve a noble gas configuration. Chlorine, in group 17, has 7 valence electrons and needs 1 more to achieve a noble gas configuration.
K will lose its 1 valence electron and become a K+ cation. Cl will gain this electron to become a Cl- anion. So, the correct electron dot structure will show K with no electrons around it, and Cl with a complete octet along with the extra electron from K.
The answer is b)⋅:K:⋅↑⋅:Cl:⋅↓. This represents potassium with an empty valence shell, suggesting the loss of its electron, and chlorine with an octet of electrons, indicating it has gained an additional electron.