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Transition Metals – Acid and Bases

This article explores the definitions and examples of acids and bases, highlighting their behavior in chemical reactions. Acids are substances that donate protons (H+), while bases absorb them. Water, for example, can function as both an acid and a base, making it amphoteric. Additionally, we discuss the classification of transition metal oxides based on oxidation states: acidic oxides (e.g., CrO3, Mn2O7) at high oxidation states, amphoteric oxides (e.g., Cr2O3, Mn2O3), and basic oxides (e.g., FeO, CrO, MnO).

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Transition Metals – Acid and Bases

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  1. Transition Metals – Acid and Bases Acids and Bases Examples Equations

  2. Defining Acids and Bases • Base – any chemical that absorbs H+ (protons) is called an acid • Example: H2O + H+ H3O+ • Acid – any chemical that can donate H+ (protons) is called a base • Example: H2O OH- + H+ • Amphoteric – any chemical that can act as an acid or a base • Example: Water (see the above examples)

  3. Acidic, Amphoteric and Basic Oxides • Transition metal form acidic oxides when they have high oxidation numbers such as 6 or 7 • Examples: CrO3 and Mn2O7 • Amphoteric oxides have an oxidation state of 3 • Examples: Cr2O3 and Mn2O3 • Basic oxides have an oxidation state of 2 • Examples: FeO, CrO, and MnO

  4. Equations • How could the following chemicals act like an acid, a base or both? • CrO3 • Mn2O3 • FeO

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