Chemical Name Calculator
Find names and formulas of ionic compounds without memorizing all the terminology
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Naming Explanation
Ionic Compound Naming
For binary ionic compounds, the cation (metal) name comes first, followed by the anion (nonmetal) name with an “-ide” suffix.
🔍 Ionic Compounds Guide
What are Ionic Compounds?
Ionic compounds are formed when metals transfer electrons to nonmetals, creating positively charged cations and negatively charged anions that attract each other.
Naming Rules
• Binary Ionic Compounds: Metal + Nonmetal with “-ide” ending
• Transition Metals: Use Roman numerals to indicate charge
• Polyatomic Ions: Use specific names for ion groups
Common Polyatomic Ions
• NH₄⁺: Ammonium
• NO₃⁻: Nitrate
• SO₄²⁻: Sulfate
• CO₃²⁻: Carbonate
• PO₄³⁻: Phosphate
Understanding Chemical Nomenclature
Chemical nomenclature is the system used for naming chemical compounds. The International Union of Pure and Applied Chemistry (IUPAC) establishes the rules for naming compounds to ensure consistency across the scientific community.
Types of Chemical Compounds
Chemical compounds can be broadly classified into several categories:
- Ionic Compounds: Formed between metals and nonmetals through electron transfer
- Covalent Compounds: Formed between nonmetals through electron sharing
- Organic Compounds: Contain carbon and hydrogen, often with other elements
- Acids and Bases: Have specific naming conventions based on their properties
Importance of Proper Naming
Correct chemical naming is crucial for:
- Scientific communication and reproducibility
- Safety in handling chemicals
- Regulatory compliance
- Educational purposes
Complete Guide to Ionic Compound Naming
Binary Ionic Compounds
Binary ionic compounds contain exactly two different elements. The naming follows this pattern:
Examples:
- NaCl: Sodium Chloride
- MgO: Magnesium Oxide
- CaCl₂: Calcium Chloride
Transition Metal Compounds
Transition metals can form multiple ions with different charges. We use Roman numerals to specify the charge:
Examples:
- FeO: Iron(II) Oxide
- Fe₂O₃: Iron(III) Oxide
- CuCl: Copper(I) Chloride
- CuCl₂: Copper(II) Chloride
Compounds with Polyatomic Ions
When compounds contain polyatomic ions, use the specific name of the ion:
- NaNO₃: Sodium Nitrate
- CaCO₃: Calcium Carbonate
- NH₄Cl: Ammonium Chloride
Chemical Formula Writing Rules
| Rule | Description | Example |
|---|---|---|
| Cation First | Always write the cation (positive ion) first | NaCl, not ClNa |
| Charge Balance | The total positive charge must equal the total negative charge | Ca²⁺ + 2Cl⁻ = CaCl₂ |
| Subscript Simplification | Reduce subscripts to lowest whole numbers when possible | Ca₂O₂ becomes CaO |
| Polyatomic Ions | Keep polyatomic ions together in parentheses when needed | Fe₂(SO₄)₃ |
Common Mistakes to Avoid
- Don’t capitalize element symbols incorrectly (Na, not NA)
- Don’t forget to balance charges in ionic compounds
- Don’t use prefixes for ionic compounds (use for covalent only)
- Don’t confuse metal and nonmetal positions in formulas
Practice Tips
To master chemical naming and formula writing:
- Memorize common ions and their charges
- Practice with flashcards for common compounds
- Use online tools like this calculator to check your work
- Start with simple binary compounds before moving to more complex ones