To determine the appropriate and final way to display the formula for magnesium chloride, let's analyze each option step by step.
First, we need to understand the formation of magnesium chloride:
- Magnesium (Mg) is a group 2 element that typically forms a +2 ion (Mg²⁺).
- Chlorine (Cl) is a group 17 element that typically forms a -1 ion (Cl⁻).
- To create a neutral compound, we need two chloride ions to balance the charge of one magnesium ion, resulting in the chemical formula MgCl₂.
Now let's evaluate each option given in the question:
A. [tex]\( Mg ^{+2} Cl ^{-1} \)[/tex]
- This notation indicates the charges on the ions, but it is not the conventional way to write the formula of a compound. Therefore, it is not the final and appropriate representation.
B. [tex]\( \text{MGCl}_2 \)[/tex]
- This notation has incorrect capitalization. Chemical symbols for elements must be written with the first letter capitalized and, if applicable, the second letter in lower case (Mg for magnesium, Cl for chlorine). This option uses MG instead of Mg and thus, is incorrect.
C. [tex]\( \text{MgCl} \)[/tex]
- This notation suggests a 1:1 ratio between magnesium and chlorine, but magnesium chloride actually consists of one magnesium ion and two chloride ions to maintain charge neutrality. Therefore, this formula is incorrect.
D. [tex]\( \text{MgCl}_2 \)[/tex]
- This notation correctly displays the chemical formula for magnesium chloride, indicating one magnesium ion (Mg²⁺) and two chloride ions (Cl⁻) in the compound. It is the appropriate and final way to represent magnesium chloride.
Therefore, the appropriate and final way to display the formula for magnesium chloride is:
D. [tex]\( \text{MgCl}_2 \)[/tex]
