Let's analyze each statement regarding the phosphate ion, [tex]\(PO_4^{3-}\)[/tex]:
1. Option 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."
This statement correctly identifies the composition of the phosphate ion: one phosphorus atom bonded to four oxygen atoms via covalent bonds. Additionally, the -3 charge is indeed distributed over the entire ion, meaning the charge is not localized on any specific atom.
2. Option 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."
This implies that the entire -3 charge is localized solely on the phosphorus atom, which is not accurate. The -3 charge is, in fact, distributed over the entire ion, not just on the phosphorus atom.
3. Option 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 is incorrect because the bonds within the phosphate ion are covalent bonds, not ionic bonds. Ionic bonds generally occur between metals and non-metals, whereas covalent bonds happen between non-metal atoms, such as phosphorus and oxygen.
4. Option 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 is incorrect for two reasons: the atoms in the phosphate ion are covalently bonded, not ionically bonded, and the -3 charge is not localized on the phosphorus atom alone, but rather distributed over the entire ion.
Therefore, 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."
