what is the correct way to represent the ionic compound sodium fluoride? na + f - *na *f: → → reset next

Explanation:

Step1: Determine ion charges

Sodium (Na) loses 1 electron to form $Na^+$ with a +1 charge. Fluorine (F) gains 1 electron to form $F^-$ with a - 1 charge.

Step2: Write the ionic - compound formula

The formula for an ionic compound is written by combining the ions in a ratio that results in a neutral compound. Since the charges of $Na^+$ and $F^-$ are equal in magnitude but opposite in sign, the formula for sodium fluoride is $NaF$. In the Lewis - structure representation, the sodium atom donates its valence electron to the fluorine atom. The sodium ion is represented as $Na^+$ and the fluoride ion as $[F:]^-$ with 8 valence electrons (a full octet). So the complete representation from the Lewis - structure perspective is $Na^+[F:]^-$.

Answer:

$NaF$ and $Na^+[F:]^-$