Give the formulas and charges of the following ions: (a) Sulfite ion (b) Phosphate ion (c) Zirconium(IV) ion (d) Chromate ion (e) Acetate ion (f) Thiosulfate ion

Verified step by step guidance

1. Identify the chemical formula and charge for each ion based on common knowledge of polyatomic ions and transition metals.
2. For the sulfite ion, recognize that it is a polyatomic ion with the formula \( \text{SO}_3^{2-} \).
3. For the phosphate ion, note that it is a polyatomic ion with the formula \( \text{PO}_4^{3-} \).
4. For the zirconium(IV) ion, understand that the Roman numeral IV indicates a +4 charge, so the formula is \( \text{Zr}^{4+} \).
5. For the chromate ion, remember it is a polyatomic ion with the formula \( \text{CrO}_4^{2-} \).

Key Concepts

Ionic Compounds and Charges

Ionic compounds are formed from the electrostatic attraction between positively charged cations and negatively charged anions. The charge of an ion is determined by the loss or gain of electrons, with cations having a positive charge due to electron loss and anions having a negative charge due to electron gain. Understanding the common charges of elements and polyatomic ions is essential for writing correct formulas.

Polyatomic Ions

Polyatomic ions are ions that consist of two or more atoms bonded together, carrying a net charge. Examples include the sulfite ion (SO3^2-) and phosphate ion (PO4^3-). Recognizing the structure and charge of these ions is crucial for accurately identifying and writing their formulas, as they often appear in various chemical reactions and compounds.

Transition Metal Ions

Transition metals can form multiple oxidation states, which means they can have different charges depending on the compound they are in. For instance, zirconium can exist as a zirconium(IV) ion (Zr^4+) in certain compounds. Understanding how to denote these oxidation states is important for correctly identifying and writing the formulas of transition metal ions.