• Collision Theory

    Rate Comparisons

    Integrated Rate Law

    Differential Rate Law

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    Equilibrium Expression

    ICE Tables

    Calculating K

    K vs Q

    Le Chatelier's Principle

  • Definitions

    Conjugate Acids & Base Pairs

    Autoionization of water

    pH Scale

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    Quantitative Electrochemistry

Ionic Compounds

Related Examples and Practice Problems

Additional Worked Out Examples/ Practice

  • Identifying classification types: Differentiation between elements, compounds or mixtures and homogeneous and heterogenous mixtures

  • Separation techniques: Selected and explaining limitation of appropriate separation

  • Relating Properties to Composition: Predicting classification based on descriptive properties

    and more …

Topic Summary & Highlights
and Help Videos

Core Concept

Ionic compounds are composed of a cation and anion. The cation is typically a metal, and the anion is usually a nonmetal or a polyatomic ion (a group of atoms with an overall charge). If the compound contains a metal it is a good sign that it can be considered an ionic compound. 

Types of Ionic Compounds

  • Type I: Ionic compounds where the metal forms only one type of cation.

  • Type II: Ionic compounds where the metal can form multiple types of cations (transition metals with variable charges).

  • Type III: Compounds containing polyatomic ions.

WRITING NAMES FOR IONIC COMPOUNDS

Type I Ionic Compounds:

  • The metal name is written first, followed by the nonmetal name with an “-ide” ending.

  • Example: NaCl is named sodium chloride.

  1. Type II Ionic Compounds:

    • These involve transition metals, which can have multiple charges.

    • Use Roman numerals in parentheses to indicate the metal's charge.

    • Example: FeCl₃ is named iron (III) chloride.

  2. Type III Ionic Compounds (with Polyatomic Ions):

    • Name the cation and then the polyatomic ion without changing its name.

    • If a polyatomic ion is anion, keep the “-ate” or “-ite” suffix.

    • Example: Ca(NO₃)₂ is named calcium nitrate.

 LABORATORY 

 DEMONSTRATIONS 

 ACTIVITIES 

 VIRTUAL SIMULATIONS 

WRITING FORMULAS FOR IONIC COMPOUNDS

  1. Write the symbols and charges for each cation and anion. (Cation is written first.)

  2. Crisscross ONLY THE NUMBER (not +/-) OF THE CHARGE to the other ion - written as a subscript. (You may need to use parentheses if the cation or anion contains more than 1 element or has a subscript already written.)

  3. Simplify the numbers that were crisscrossed (now written as subscripts). (If the subscript is reduced to “1” then it should not be written and parentheses are not needed.)

Example:

  • Sodium chloride (Type I): Na+\text{Na}^+Na+ and Cl−\text{Cl}^-Cl− combine to form NaCl.

  • Iron (III) oxide (Type II): Fe3+\text{Fe}^{3+}Fe3+ and O2−\text{O}^{2-}O2− combine to form Fe2O3\text{Fe}_2\text{O}_3Fe2​O3​.

  • Calcium nitrate (Type III): Ca2+\text{Ca}^{2+}Ca2+ and NO3−\text{NO}_3^-NO3−​ combine to form Ca(NO3)2\text{Ca}(\text{NO}_3)_2Ca(NO3​)2​.

Practice Tips

  • Memorize Common Ions: Focus on learning the common polyatomic ions, charges, and patterns.

  • Roman Numerals for Transition Metals: Practice associating transition metals with their possible charges.

  • Cross-Method for Formulas: To determine the correct formula, use the “criss-cross” method to balance charges between cations and anions.

Video Resources