To determine the correct chemical formula of magnesium bromide, let's start by analyzing the elements involved and their respective valencies.
Magnesium (Mg) is an element in Group 2 of the periodic table, which means it has a valency of +2, as it tends to lose two electrons to form a stable ionic state.
Bromine (Br) is an element in Group 17 of the periodic table, which means it has a valency of -1, as it tends to gain one electron to achieve a stable ionic state like the noble gases.
To create a neutral compound, the total positive charge must balance the total negative charge. Here is the step-by-step process:
1. Determine the charges on the ions:
- Magnesium has a +2 charge: [tex]\(Mg^{2+}\)[/tex]
- Bromine has a -1 charge: [tex]\(Br^{-}\)[/tex]
2. Balance the charges:
- Since magnesium has a +2 charge and bromine has a -1 charge, you need two bromine ions to balance out the +2 charge of magnesium. This gives us [tex]\(MgBr_2\)[/tex].
Therefore, the correct chemical formula is:
[tex]$MgBr_2$[/tex]
Now, compare this with the given options:
A. [tex]$MgBr _2$[/tex]
B. MgBr
C. [tex]$Mg _2 Br _2$[/tex]
D. [tex]$Mg _2 Br$[/tex]
The correct answer is:
A. [tex]$MgBr _2$[/tex]
