Answer:
When determining the charge each atom will make when it bonds with other atoms, we need to consider their position in the periodic table and their electron configuration.
Step-by-step explanation:
Here are the charges that each atom will make when it bonds with other atoms:
1. Calcium (Ca): Calcium belongs to group 2 of the periodic table, known as the alkaline earth metals. Alkaline earth metals tend to lose two electrons to achieve a stable configuration. Therefore, when calcium bonds with other atoms, it will typically have a charge of +2.
2. Phosphorus (P): Phosphorus belongs to group 15 of the periodic table. It has five valence electrons and tends to gain three electrons to achieve a stable configuration. Hence, when phosphorus bonds with other atoms, it will usually have a charge of -3.
3. Boron (B): Boron belongs to group 13 of the periodic table. It has three valence electrons and tends to lose three electrons to achieve a stable configuration. Thus, when boron bonds with other atoms, it will typically have a charge of +3.
It is important to note that these charges are general trends and can vary depending on the specific compound and the bonding situation. Also, there are cases where atoms can have different charges depending on the bonding partners and the specific arrangement of electrons. Therefore, it is essential to consider the specific context and chemical formula when determining the charges of atoms in compounds.