To determine the charges of each ion in aluminum oxide, we should analyze the chemical formula and the typical charges of aluminum and oxygen in their ionic forms.
Step-by-Step Solution:
1. Identify the chemical formula of aluminum oxide:
Aluminum oxide is commonly represented by the formula [tex]\( Al_2O_3 \)[/tex].
2. Identify the typical ionic charges for aluminum and oxygen:
- Aluminum (Al): Aluminum typically loses three electrons to form a cation with a charge of [tex]\( +3 \)[/tex]. This results in the ion [tex]\( Al^{3+} \)[/tex].
- Oxygen (O): Oxygen typically gains two electrons to form an anion with a charge of [tex]\( -2 \)[/tex]. This results in the ion [tex]\( O^{2-} \)[/tex].
3. Balance the charges in the formula [tex]\( Al_2O_3 \)[/tex]:
- In aluminum oxide, there are 2 aluminum ions and 3 oxygen ions.
- The total positive charge contributed by aluminum ions is [tex]\( 2 \times +3 = +6 \)[/tex].
- The total negative charge contributed by oxygen ions is [tex]\( 3 \times -2 = -6 \)[/tex].
4. Ensure charge neutrality:
- For the compound to be neutral, the total positive charge must balance the total negative charge.
- In [tex]\( Al_2O_3 \)[/tex], the charges balance with [tex]\( +6 \)[/tex] from the aluminum ions and [tex]\( -6 \)[/tex] from the oxygen ions, resulting in a neutral compound.
By analyzing the chemical formula and the typical ionic charges of the elements involved, we can conclude that the charges of each ion in aluminum oxide are:
[tex]\[ \boxed{Al^{3+} \text{ and } O^{2-}} \][/tex]
Thus, the correct answer is:
[tex]\[ \boxed{\text{A. } Al^{3+} \text{ and } O^{2-}} \][/tex]
