To determine which statement correctly describes the phosphate ion, [tex]\( PO _4^{3-} \)[/tex], let's analyze each statement step by step:
1. "It is composed of one phosphorus atom and four oxygen atoms covalently bonded together, and there is a -3 charge distributed over the entire ion."
- The phosphate ion consists of one phosphorus atom and four oxygen atoms.
- The bonding between the phosphorus atom and the oxygen atoms in a phosphate ion is covalent.
- The entire ion carries an overall charge of -3, which is distributed over the whole ion rather than localized on a single atom.
2. "It is composed of one phosphorus atom and four oxygen atoms covalently bonded together, and there is a -3 charge on the phosphorus atom."
- While the composition and type of bonds described here are correct, the charge distribution is not accurate. The -3 charge is not localized on the phosphorus atom but is distributed over the entire ion.
3. "It is composed of one phosphorus atom and four oxygen atoms ionically bonded together, and there is a -3 charge distributed over the entire ion."
- This statement is incorrect because the bonds within a phosphate ion are covalent, not ionic.
4. "It is composed of one phosphorus atom and four oxygen atoms ionically bonded together, and there is a -3 charge on the phosphorus atom."
- This statement is also incorrect due to the nature of the bonding. The bonds within a phosphate ion are covalent, not ionic, and the charge is not localized on the phosphorus atom.
Based on this analysis, the correct statement is:
- It is composed of one phosphorus atom and four oxygen atoms covalently bonded together, and there is a -3 charge distributed over the entire ion.
Hence, the correct statement that describes the phosphate ion, [tex]\( PO_4^{3-} \)[/tex], is:
- "It is composed of one phosphorus atom and four oxygen atoms covalently bonded together, and there is a -3 charge distributed over the entire ion."
This corresponds to the first statement in the list.
