To determine the correct notation for magnesium chloride among the given options, we need to understand the chemical composition and standard notation for magnesium chloride.
1. Magnesium (Mg) is a Group 2 element in the periodic table, and it typically forms a [tex]$2^{+}$[/tex] ion ([tex]$Mg^{2+}$[/tex]).
2. Chlorine (Cl) is a Group 17 element in the periodic table, and it typically forms a [tex]$1^{-}$[/tex] ion ([tex]$Cl^{-}$[/tex]).
When magnesium and chlorine combine to form magnesium chloride:
- One magnesium ion ([tex]$Mg^{2+}$[/tex]) needs two chloride ions ([tex]$Cl^{-}$[/tex]) to neutralize its charge.
- This leads to the formula [tex]$MgCl_{2}$[/tex], which indicates that there are two chloride ions for every one magnesium ion.
Now, let's examine each option:
A. [tex]$MGCl _2$[/tex]
- The notation uses "MG" instead of "Mg". The correct element symbol for magnesium is "Mg", not "MG". So, this is incorrect.
B. [tex]$MgCl _2$[/tex]
- This notation correctly displays magnesium (Mg) and chlorine (Cl) with the appropriate subscript "2" indicating two chloride ions. This is the correct formula for magnesium chloride.
C. MgCl
- This notation does not account for the two chloride ions needed to balance the charge of one magnesium ion. It is incomplete and incorrect.
D. [tex]$Mg ^{+2} Cl ^{-1}$[/tex]
- This notation indicates the charges but does not represent the correct ratio of magnesium to chloride ions needed to form a neutral compound. It shows individual ions rather than the compound's formula.
After evaluating each option, the appropriate and final way to display the formula for magnesium chloride is:
B. [tex]$MgCl_{2}$[/tex]
Thus, the correct answer is option B.
