Let's analyze the given half of the balanced chemical equation:
[tex]\[ 3 \text{Mg(OH)}_2 + 2 \text{H}_3 \text{PO}_4 \][/tex]
First, we'll count the number of each type of atom on the reactant side:
For [tex]\(3 \text{Mg(OH)}_2\)[/tex]:
- Magnesium (Mg): [tex]\(3 \text{Mg(OH)}_2 = 3 \text{Mg}\)[/tex]
- Oxygen (O): Each [tex]\(\text{Mg(OH)}_2\)[/tex] has 2 O atoms, so [tex]\(3 \times 2 = 6 \text{O}\)[/tex]
- Hydrogen (H): Each [tex]\(\text{Mg(OH)}_2\)[/tex] has 2 H atoms, so [tex]\(3 \times 2 = 6 \text{H}\)[/tex]
For [tex]\(2 \text{H}_3 \text{PO}_4\)[/tex]:
- Hydrogen (H): Each [tex]\(\text{H}_3 \text{PO}_4\)[/tex] has 3 H atoms, so [tex]\(2 \times 3 = 6 \text{H}\)[/tex]
- Phosphorus (P): Each [tex]\(\text{H}_3 \text{PO}_4\)[/tex] has 1 P atom, so [tex]\(2 \times 1 = 2 \text{P}\)[/tex]
- Oxygen (O): Each [tex]\(\text{H}_3 \text{PO}_4\)[/tex] has 4 O atoms, so [tex]\(2 \times 4 = 8 \text{O}\)[/tex]
Now, we sum the atoms from both reactants:
- Magnesium (Mg): [tex]\(3 \text{Mg}\)[/tex]
- Phosphorus (P): [tex]\(2 \text{P}\)[/tex]
- Oxygen (O): [tex]\(6 + 8 = 14 \text{O}\)[/tex]
- Hydrogen (H): [tex]\(6 + 6 = 12 \text{H}\)[/tex]
So, the complete balanced chemical equation must contain:
- 3 atoms of Magnesium (Mg)
- 2 atoms of Phosphorus (P)
- 14 atoms of Oxygen (O)
- 12 atoms of Hydrogen (H)
Therefore, the numbers of each atom in the other half of the equation are:
[tex]\[ 3 \text{Mg}, 2 \text{P}, 14 \text{O}, 12 \text{H} \][/tex]
The correct option is:
[tex]\[ 3 \text{Mg}, 2 \text{P}, 14 \text{O}, 12 \text{H} \][/tex]
