What is the formula for Tin (IV) Chlorate?
Sn(CIO3)4
Sn(CIO3)2
Tn(CIO3)4
SnCIO3
Sn(CIO)3
The Correct Answer and Explanation is :
The correct formula for Tin (IV) Chlorate is Sn(ClO₃)₄.
Explanation:
The formula represents a compound made of tin (Sn) and chlorate (ClO₃) ions. Let’s break down the components:
- Tin (IV): The Roman numeral IV indicates that tin has a +4 oxidation state in this compound. This is crucial for determining the number of chlorate ions that will bond with the tin atom.
- Chlorate ion (ClO₃⁻): The chlorate ion has a -1 charge, meaning that each chlorate ion will contribute one negative charge to the compound. Since tin (IV) has a +4 charge, we need 4 chlorate ions to balance the charge. Thus, four ClO₃⁻ ions will combine with one Sn⁴⁺ ion to form Sn(ClO₃)₄, where the charges balance out to zero.
Why not the other options?
- Sn(ClO₃)₂: This formula suggests that tin is in the +2 oxidation state (since two chlorate ions would balance out a +2 charge from tin). This would be the correct formula for Tin (II) Chlorate, not Tin (IV) Chlorate.
- Tn(ClO₃)₄: The symbol “Tn” is incorrect. The element we are talking about is “Sn,” which stands for tin.
- SnClO₃: This formula implies that there is only one chlorate ion for one tin atom, which is not correct for a compound where tin has a +4 oxidation state.
- Sn(ClO)₃: This formula suggests that the compound contains hypochlorite (ClO⁻) ions, which is a different chemical species from chlorate (ClO₃⁻). This would represent Tin (IV) Hypochlorite, not Tin (IV) Chlorate.
Therefore, the correct chemical formula for Tin (IV) Chlorate is Sn(ClO₃)₄.
Now, I will generate an image representing the Tin (IV) Chlorate molecule.
Here is the chemical structure diagram of Tin (IV) Chlorate (Sn(ClO₃)₄). It shows the Tin (Sn) atom at the center, bonded with four Chlorate (ClO₃) ions. Each chlorate ion consists of a chlorine (Cl) atom bonded to three oxygen (O) atoms, with the appropriate charges indicated. Let me know if you’d like further clarification!