To determine the systematic name of the compound [tex]\( \text{Mg} \left( \text{NO}_3 \right)_2 \)[/tex], follow these steps:
1. Identify the cation: The compound consists of magnesium ([tex]\(\text{Mg}\)[/tex]) as the cation. Magnesium is a metal from Group 2 of the periodic table and typically forms a [tex]\(+2\)[/tex] charge.
2. Identify the anion: The compound also contains the nitrate ([tex]\(\text{NO}_3\)[/tex]) ion. The nitrate ion is a polyatomic ion with a [tex]\(−1\)[/tex] charge.
3. Determine the ratio of ions: Since magnesium has a [tex]\(+2\)[/tex] charge and the nitrate ion has a [tex]\(−1\)[/tex] charge, you need two nitrate ions to balance the positive charge of one magnesium ion. Thus, the formula of the compound is [tex]\( \text{Mg} \left( \text{NO}_3 \right)_2 \)[/tex].
4. Write the systematic name: To name the compound, combine the name of the cation followed by the name of the anion. The cation is named "Magnesium," and the anion is named "Nitrate."
Putting it all together, the systematic name of [tex]\( \text{Mg} \left( \text{NO}_3 \right)_2 \)[/tex] is Magnesium Nitrate.
