Name each ionic compound. a. SnCl₄ b. PbI₂ c. Fe₂O₃ d. CuI₂ e. HgBr₂ f. CrCl₂

Verified step by step guidance

1. Identify the cation and the anion in the compound. In SnCl_4, Sn is the cation (tin) and Cl is the anion (chloride).
2. Determine the charge of the anion. Chloride (Cl) has a charge of -1.
3. Calculate the total negative charge from the anions. Since there are four chloride ions, the total negative charge is 4(-1) = -4.
4. Determine the charge of the cation. The total positive charge must balance the total negative charge. Therefore, the charge on Sn must be +4.
5. Name the compound by stating the name of the cation followed by the anion. Since tin can have multiple oxidation states, specify the charge of the tin cation using Roman numerals. The name of SnCl_4 is tin(IV) chloride.

Key Concepts

Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively charged cations and negatively charged anions. These oppositely charged ions attract each other, creating a stable compound. The properties of ionic compounds include high melting and boiling points, and they typically dissolve in water to form electrolytes.

Nomenclature of Ionic Compounds

The nomenclature of ionic compounds involves naming the cation first, followed by the anion. For cations derived from metals, the name remains the same as the element, while anions typically have their names modified to end in '-ide' for simple anions or use specific names for polyatomic ions. In the case of transition metals, the oxidation state is indicated using Roman numerals.

Tin (Sn) and its Oxidation States

Tin (Sn) can exhibit multiple oxidation states, commonly +2 and +4. In the compound SnCl4, tin is in the +4 oxidation state, as it forms four bonds with chloride ions (Cl-). Understanding the oxidation state is crucial for correctly naming the compound and recognizing its chemical behavior.