Transition Metals (Type II Metals)

Introduction to Transition Metals

Transition metals are elements found in the central block of the periodic table (Groups 3B to 2B). They are characterized by their ability to form multiple positive charges (cations) due to variable electron arrangements in their d orbitals.

• Transition metals often have more than one possible charge (oxidation state).

• These varying charges arise from the loss of electrons from both the outermost s and d orbitals.

• Advanced explanations for these charges involve electron configurations and will be discussed in later chapters.

Periodic Table Organization: Transition Metals

The periodic table highlights the location of transition metals, which occupy the center block (Groups 3B to 2B, periods 4-7). Some key transition metals include:

• Scandium (Sc)

• Yttrium (Y)

• Lanthanum (La)

• Actinium (Ac)

• Zinc (Zn)

• Silver (Ag)

• Cadmium (Cd)

These elements are shown in the provided periodic table, with their group and period positions indicated.

Common Charges of Transition Metals

Unlike main group metals, transition metals can form ions with different charges. The most common charges are:

• +2 (e.g., Fe2+, Cu2+)

• +3 (e.g., Fe3+, Cr3+)

• Some transition metals, such as Ag, commonly form only one charge (Ag+).

Example: Predicting the major charge of an ion in Period 10, Group 3B (hypothetical): The answer is +3.

Practice Problems and Solutions

Practice problems help reinforce understanding of transition metal charges and electron configurations.

• Practice 1: What is the likely charge of the element with atomic number 47?

  • Atomic number 47 corresponds to Silver (Ag).

  • Ag commonly forms a +1 ion.

  • Answer: +1

• Practice 2: How many electrons would the cadmium ion possess?

  • Cadmium (Cd) has atomic number 48.

  • The most common ion is Cd2+.

  • Number of electrons in Cd2+:

  • Answer: 46 electrons

Table: Selected Transition Metals and Their Common Charges

Key Concepts and Definitions

• Transition Metal: An element whose atom has an incomplete d sub-shell, or which can give rise to cations with an incomplete d sub-shell.

• Oxidation State (Charge): The charge an atom would have if all bonds to atoms of different elements were 100% ionic.

• Cation: A positively charged ion formed by the loss of electrons.

Summary

• Transition metals are central to inorganic chemistry due to their variable charges.

• Understanding their common charges is essential for predicting chemical behavior and writing formulas.

• Practice problems reinforce the identification of charges and electron counts for transition metal ions.