CHEM104 Lecture Chapter 3 Overview - Naming Ionic Compounds

Instructor: Dorothy Swain

Overview

• Introduction to naming ionic compounds, an essential topic in introductory chemistry.
• Focus on the systematic methods for naming ionic compounds, including binary ionic compounds and those with polyatomic ions.

Key Concepts

Binary Ionic Compounds

• Composed of two different elements: a metal and a non-metal.
• The metal cation is named first, followed by the non-metal anion.
• The non-metal anion's name is modified to end in "-ide."
  • Example: NaCl is named sodium chloride.

Transition Metals

• Transition metals can have multiple oxidation states.
• Use Roman numerals in parentheses to denote the charge of the metal cation.
  • Example: FeCl₂ is named iron (II) chloride.

Polyatomic Ions

• For compounds containing polyatomic ions, the name of the ion is used as is.
• Common polyatomic ions include:
  • Ammonium (NH₄⁺)
  • Nitrate (NO₃⁻)
  • Sulfate (SO₄²⁻)
• Example: NaNO₃ is named sodium nitrate.

Tips for Naming Ionic Compounds

• Always identify the cation and anion first.
• Check the periodic table for standard charges of elements.
• Use the list of common polyatomic ions to assist with naming.

Practice Problems

• The lecture may include practice problems for students to test their understanding of naming ionic compounds.
• Practice involves writing the names of given chemical formulas and vice versa.

Summary

• Understanding ionic compound naming is crucial for further studies in chemistry.
• Naming conventions allow chemists to communicate effectively about chemical compounds.

Additional Resources

• Provided resources may include a list of common ions, periodic table, and practice worksheets.

This lecture provides foundational knowledge essential for chemistry students, focusing on the principles and practices of naming ionic compounds effectively.