What is the formula for Manganese (II) Phosphide?
The Correct Answer and Explanation is :
The formula for Manganese (II) Phosphide is Mn₃P₂.
Explanation:
Manganese (II) Phosphide consists of two elements: Manganese (Mn) and Phosphorus (P). The key to understanding its formula lies in determining the oxidation states of these elements and how they combine to form a neutral compound.
- Oxidation States:
- Manganese (Mn) can have various oxidation states, but in this case, it is in the +2 oxidation state, as indicated by the “(II)” in the compound’s name. The +2 oxidation state means each manganese ion has lost two electrons.
- Phosphorus (P), when it forms phosphides, generally has an oxidation state of -3. This means each phosphorus ion has gained three electrons to form a stable ion.
- Combining Manganese and Phosphorus:
- To balance the charges and form a neutral compound, the total positive charge from manganese must equal the total negative charge from phosphorus.
- Manganese in the +2 oxidation state (Mn²⁺) and phosphorus in the -3 oxidation state (P³⁻) need to combine in a ratio that neutralizes the charges. The simplest way to balance the charges is to have three Mn²⁺ ions (totaling +6) and two P³⁻ ions (totaling -6). This results in a neutral compound.
- Formula:
- The number of manganese ions needed is 3, and the number of phosphorus ions needed is 2. Thus, the formula for Manganese (II) Phosphide is Mn₃P₂.
This type of compound is part of a group known as metal phosphides, which are often used in various industrial and technological applications, such as semiconductors, magnets, and in the synthesis of other materials.