Skip to main content
Chemistry LibreTexts

3.6: Transition Metal Ions

  • Page ID
  • \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

    \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)

    \( \newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\)

    ( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\)

    \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)

    \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\)

    \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)

    \( \newcommand{\Span}{\mathrm{span}}\)

    \( \newcommand{\id}{\mathrm{id}}\)

    \( \newcommand{\Span}{\mathrm{span}}\)

    \( \newcommand{\kernel}{\mathrm{null}\,}\)

    \( \newcommand{\range}{\mathrm{range}\,}\)

    \( \newcommand{\RealPart}{\mathrm{Re}}\)

    \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)

    \( \newcommand{\Argument}{\mathrm{Arg}}\)

    \( \newcommand{\norm}[1]{\| #1 \|}\)

    \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)

    \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\AA}{\unicode[.8,0]{x212B}}\)

    \( \newcommand{\vectorA}[1]{\vec{#1}}      % arrow\)

    \( \newcommand{\vectorAt}[1]{\vec{\text{#1}}}      % arrow\)

    \( \newcommand{\vectorB}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

    \( \newcommand{\vectorC}[1]{\textbf{#1}} \)

    \( \newcommand{\vectorD}[1]{\overrightarrow{#1}} \)

    \( \newcommand{\vectorDt}[1]{\overrightarrow{\text{#1}}} \)

    \( \newcommand{\vectE}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{\mathbf {#1}}}} \)

    \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

    \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)

     Platinum eagle coin
    Figure \(\PageIndex{1}\) (Credit: Courtesy of the ​​​​​​​US Mint; Source: Commons Wikimedia, Platinium eagle 101(opens in new window) []; License: Public Domain)

    What kind of coin is this?

    Most of us are familiar with the common coins: penny, nickel, dime, quarter. In some areas (such as Las Vegas), you might see large amounts of silver dollars (these get a little heavy in your pocket). But most of us have probably never seen a platinum eagle—an eagle-depicting coin that is held primarily by collectors. If you were to take a one-ounce platinum eagle into a store to buy one hundred dollars worth of items, the store owner will most likely not believe you when you claim that the coin is worth one hundred dollars. It would also be awkward and annoying if you lost one of these coins out of your pocket. Platinum is just one of several transition metals that is worth a lot of money (gold is another one).

    The group 1 and 2 elements form cations through a simple process that involves the loss of one or more outer shell electrons. These electrons come from the \(s\) orbital and are removed very readily.

    Transition Metal Ions

    Most transition metals differ from the metals of Groups 1, 2, and 13 in that they are capable of forming more than one cation with different ionic charges. As an example, iron commonly forms two different ions. It can sometimes lose two electrons to form the \(\ce{Fe^{2+}}\) ion, while at other times it loses three electrons to form the \(\ce{Fe^{3+}}\) ion. Tin and lead, though members of the \(p\) block rather than the \(d\) block, also are capable of forming multiple ions.

    CK12 Screenshot 7-5-1.png
    Figure \(\PageIndex{2}\): (Credit: Cepheus, modified by CK-12 Foundation; Source: Commons Wikimedia, Periodic Table(opens in new window) []; License: Public Domain)

    Ionic formation for transition metals is complicated by the fact that these elements have unfilled inner \(d\) shells. Although the next higher \(s\) orbitals are actually at a lower energy level than the \(d\) level, these \(s\) electrons are the ones that are removed during ionization.

    The table below lists the names and formulas of some of the common transition metal ions:

    Common Transition Metal Ions
    Table \(\PageIndex{1}\): Common Transition Metal Ions
    \(1+\) \(2+\) \(3+\) \(4+\)
    copper (I), \(\ce{Cu^+}\) cadmium, \(\ce{Cd^{2+}}\) chromium (III), \(\ce{Cr^{3+}}\) lead (IV), \(\ce{Pb^{4+}}\)
    gold (I), \(\ce{Au^+}\) chromium (II), \(\ce{Cr^{2+}}\) cobalt (III), \(\ce{Co^{3+}}\) tin (IV), \(\ce{Sn^{4+}}\)
    mercury (I), \(\ce{Hg_2^{2+}}\) cobalt (II), \(\ce{Co^{2+}}\) gold (III), \(\ce{Au^{3+}}\)  
    silver, \(\ce{Ag^+}\) copper (II), \(\ce{Cu^{2+}}\) iron (III), \(\ce{Fe^{3+}}\)  
      iron (II), \(\ce{Fe^{2+}}\)    
      lead (II), \(\ce{Pb^{2+}}\)    
      manganese (II), \(\ce{Mn^{2+}}\)    
      mercury (II), \(\ce{Hg^{2+}}\)    
      nickel (II), \(\ce{Ni^{2+}}\)    
      platinum (II), \(\ce{Pt^{2+}}\)    
      tin (II), \(\ce{Sn^{2+}}\)    
      zinc, \(\ce{Zn^{2+}}\)    

    Uses for Transition Metals

    Because there are so many metals in this group, there are a wide variety of uses. Many of the metals are used in electronics, while others (such as gold and silver) are used in monetary systems. Iron is a versatile structural material. Cobalt, nickel, platinum, and other metals are employed as catalysts in a number of chemical reactions. Zinc is a significant component of batteries.


    • Transition metals have unfilled inner \(d\) electron shells.
    • Ions form primarily through loss of \(s\) electrons.
    • Many transition metals can form more than one ion.
    • Transition metals have a wide variety of applications.


    1. What is unique about the electron configurations of transition metals?
    2. Which electrons of transition metal elements are most likely to be lost during ion formation?
    3. How many ions can iron form?
    4. Which transition metal forms only one ion?
    5. List several uses for transition metals.

    3.6: Transition Metal Ions is shared under a CC BY-NC license and was authored, remixed, and/or curated by LibreTexts.