Question

missed this? watch iwe: writing formulas for ionic compounds; read section 5.5. you can c

part a

write a formula for the compound that forms between mg and cl.

○ mgcl
○ mgcl₂
○ mg₂cl
○ mg₂cl₂

Explanation:

Step1: Determine ion charges

Magnesium (Mg) typically forms a \( \text{Mg}^{2+} \) ion (loses 2 electrons). Chlorine (Cl) typically forms a \( \text{Cl}^- \) ion (gains 1 electron).

Step2: Balance charges

To form a neutral compound, the total positive charge must equal the total negative charge. Let the number of \( \text{Mg}^{2+} \) ions be \( x \) and \( \text{Cl}^- \) ions be \( y \). Then \( 2x = y \) (since \( +2x + (-1)y = 0 \)). The simplest ratio is \( x = 1 \), \( y = 2 \), so the formula is \( \text{MgCl}_2 \).

Answer:

B. \( \text{MgCl}_2 \)