Question

consider the lewis dot structures of potassium and bromine atoms.
k ·br·
which lewis dot structure best represents the compound formed when potassium and bromine react?
k^- ·br·^+ k^+ ·br·^- k^+ ·br·^- k^- ·br·^+

Explanation:

Step1: Determine the ions formed

Potassium (K) has one valence electron. It loses this electron to form \(K^{+}\) ion. Bromine (Br) has seven valence electrons. It gains one electron to form \(Br^{-}\) ion.

Step2: Analyze the Lewis dot structure of the compound

In an ionic compound, the cation (\(K^{+}\)) and anion (\(Br^{-}\)) are shown with their respective charges. The Lewis dot structure of the compound formed (KBr) should have \([K]^{+}\) (since K loses an electron, no dots around it in the ion) and \([\cdot\ddot{Br}\cdot]^{-}\) (Br gains an electron to complete its octet).

Answer:

The second option \([K]^{+}[\cdot\ddot{Br}\cdot]^{-}\) (assuming the second structure in the given set of options has \(K^{+}\) and \(Br^{-}\) correctly represented as per the ion - charge and electron - transfer description above)