To determine the product formed from a reaction between calcium (Ca) and phosphorus (P), we need to consider the valency (or oxidation state) of each element.
1. Valency of Calcium (Ca):
Calcium is an element in Group 2 of the periodic table. Elements in this group typically have a +2 valency because they tend to lose two electrons to achieve a stable electron configuration. Therefore, the valency of calcium is +2.
2. Valency of Phosphorus (P):
Phosphorus is in Group 15 of the periodic table. Elements in this group typically gain three electrons to achieve a stable electron configuration, giving them a valency of -3. Hence, the valency of phosphorus is -3.
To form a neutral compound, the total positive charge must balance out the total negative charge.
3. Balancing the Charges:
- Calcium has a valency of +2.
- Phosphorus has a valency of -3.
We need to find the smallest whole number ratio of calcium to phosphorus that will balance the charges. This can be done by finding the least common multiple (LCM) of the absolute values of the valencies (2 and 3).
- The LCM of 2 and 3 is 6.
Therefore:
- To achieve a total positive charge of 6, we need 3 calcium atoms ([tex]\(3 \times +2 = +6\)[/tex]).
- To achieve a total negative charge of 6, we need 2 phosphorus atoms ([tex]\(2 \times -3 = -6\)[/tex]).
When these combine, the formula of the compound will be [tex]\(Ca_3P_2\)[/tex].
So, the correct answer is:
D. [tex]\( \text{Ca}_3\text{P}_2 \)[/tex]
