name the following ionic compounds.
strontium permanganate
iron (II) thiosulfate
manganese (II) phosphite
lithium hypochlorite
zirconium periodate
titanium (IV) dichromate
The correct answer and explanation is :
Naming the Given Ionic Compounds:
- Strontium Permanganate – Sr(MnO₄)₂
- Iron (II) Thiosulfate – FeS₂O₃
- Manganese (II) Phosphite – Mn₃(PO₃)₂
- Lithium Hypochlorite – LiClO
- Zirconium Periodate – Zr(IO₄)₄
- Titanium (IV) Dichromate – Ti(Cr₂O₇)₂
Explanation of Naming:
Ionic compounds consist of cations (positively charged ions) and anions (negatively charged ions). Naming them follows specific rules:
- Cation First, Anion Second:
- The metal (cation) is always named first.
- The anion follows and may require a specific name based on its polyatomic group.
- Using Roman Numerals for Transition Metals:
- Transition metals can have multiple oxidation states. Roman numerals indicate the charge of the metal in the name.
- Example: Iron (II) Thiosulfate (Fe²⁺) means iron has a +2 charge.
- Recognizing Polyatomic Ions:
- Some anions are polyatomic, meaning they consist of multiple atoms bonded together.
- Common ones include:
- Permanganate (MnO₄⁻)
- Thiosulfate (S₂O₃²⁻)
- Phosphite (PO₃³⁻)
- Hypochlorite (ClO⁻)
- Periodate (IO₄⁻)
- Dichromate (Cr₂O₇²⁻)
- Balancing Charges in Formulas:
- The total positive charge must balance the total negative charge to form a neutral compound.
- Example: Strontium Permanganate (Sr²⁺ and MnO₄⁻) → Needs two MnO₄⁻ ions to balance Sr²⁺ → Sr(MnO₄)₂.
Understanding these principles helps systematically name ionic compounds based on their chemical formula.