This worksheet will guide you through the process of naming and formulating binary ionic compounds. Understanding these fundamentals is crucial for success in chemistry. We'll cover key concepts, provide examples, and offer a complete answer key to help solidify your understanding.
What are Binary Ionic Compounds?
Binary ionic compounds are formed when a metal (cation) and a nonmetal (anion) react, transferring electrons to create a stable electrostatic attraction. The key characteristic is the presence of only two elements in the compound. The metal, having lost electrons, becomes positively charged, while the nonmetal, having gained electrons, becomes negatively charged. These opposite charges attract, forming the ionic bond.
Naming Binary Ionic Compounds
The naming convention for binary ionic compounds is straightforward:
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Name the cation (metal) first: Use the element's name. If the metal has multiple possible charges (transition metals), indicate the charge using Roman numerals in parentheses. For example, Iron(II) or Iron(III).
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Name the anion (nonmetal) second: Change the ending of the nonmetal's name to "-ide". For example, chlorine becomes chloride, oxygen becomes oxide, sulfur becomes sulfide.
Example: NaCl is named Sodium Chloride. FeCl₂ is named Iron(II) Chloride, and FeCl₃ is named Iron(III) Chloride.
Writing Formulas for Binary Ionic Compounds
Writing the formula requires balancing the charges of the cation and anion to achieve electrical neutrality. The total positive charge must equal the total negative charge. This often involves using subscripts to indicate the number of atoms of each element.
Steps:
- Write the symbols for the cation and anion.
- Determine the charge of each ion.
- Use the criss-cross method: The absolute value of the cation's charge becomes the subscript of the anion, and the absolute value of the anion's charge becomes the subscript of the cation.
- Simplify the subscripts (if necessary) to the lowest whole number ratio.
Example: Forming the formula for Magnesium Oxide (Mg²⁺ and O²⁻):
- Mg²⁺ + O²⁻ becomes Mg₂O₂ which simplifies to MgO.
Practice Worksheet: Naming and Formula Writing
Part 1: Name the following binary ionic compounds:
- KCl
- MgBr₂
- Al₂O₃
- FeO
- CuCl₂
- SnF₄
- Cr₂S₃
- Li₂S
Part 2: Write the formulas for the following binary ionic compounds:
- Calcium Chloride
- Sodium Oxide
- Aluminum Sulfide
- Iron(III) Oxide
- Copper(I) Bromide
- Lead(II) Iodide
- Zinc Nitride
- Titanium(IV) Chloride
Answer Key
Part 1:
- Potassium Chloride
- Magnesium Bromide
- Aluminum Oxide
- Iron(II) Oxide
- Copper(II) Chloride
- Tin(IV) Fluoride
- Chromium(III) Sulfide
- Lithium Sulfide
Part 2:
- CaCl₂
- Na₂O
- Al₂S₃
- Fe₂O₃
- CuBr
- PbI₂
- Zn₃N₂
- TiCl₄
This worksheet provides a strong foundation in understanding and working with binary ionic compounds. Remember to practice regularly to build your proficiency and confidence. For further practice, research polyatomic ions and their role in forming more complex ionic compounds. This will expand your understanding of chemical bonding and nomenclature.
