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Transition Metals

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Practice Transition Metals
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Transition Elements

stock model of car

racing model of same car

From the outside, the two cars above look the same (except for the flashy paint job on the racing model).  They are the same model of the car, but one is a stock edition for regular driving while the other one is built for high-speed racing.  We really can’t tell much from the external view.  To see the differences, we need to go under the hood, take the engines apart, and look at the braking and suspension systems in order to see how the two cars differ.

Many electron configurations of elements are simple and straighforward.  We can look at the outer shell and easily understand how that set of elements will react in terms of electron gain or loss.  However, there are sets of elements that are more complex in their behavior. One such group is called the transition elements .

Transition elements are the elements that are found in Groups 3-12 (old groups IIA-IIB) on the periodic table (salmon-colored block in the middle of the table). The term refers to the fact that the  $d$ sublevel , which is in the process of being filled, is in a lower principal energy level than the  $s$ sublevel filled before it. For example, the electron configuration of scandium, the first transition element, is $[Ar]3d^14s^2$ . Remember that the configuration is reversed from the fill order – the  $4s$ filled before the  $3d$ begins. Because they are all metals, the transition elements are often called the transition metals. As a group, they display typical metallic properties and are less reactive than the metals in Groups 1 and 2. Some of the more familiar ones are so unreactive that they can be found in nature in their free, or uncombined state. These include platinum, gold, and silver.  Because of this unique filling order, the transition elements are often referred to as “ $d$ -block” elements.

piece of silver

Compounds of many transition elements are distinctive for being widely and vividly colored. Electron transitions that occur within the  $d$ sublevel release energies that result in the emission of visible light of varied wavelengths.

Transition metal compounds dissolved in water exhibit a wide variety of bright colors. From left to right are shown solutions of cobalt(II) nitrate, potassium dichromate, potassium chromate, nickel(II) chloride, copper(II) sulfate, and potassium permanganate.

Summary

• The transition elements are found in groups IIIA-IIB (new groups 3-12)
• These elements are characterized by having unfilled  $d$ sublevels.
• In general, the next higher  $s$ sublevel is already filled or has one electron missing.
• Many transition element compounds are brightly colored due to the inner-level  $d$ electron transitions.

Practice

1. Why are the transition metals named “transition?”
2. How do the properties of transition metals and main-group metals overlap?
3. Which electrons are more likely to be removed from transition metals as they react?

Review

1. List five different transition elements, giving their name, chemical symbol, and atomic number.
2. What is unique about the transition elements in terms of electron configurations?
3. Why are these elements often referred to as “ $d$ -block” elements?
4. Which transition group elements can be found in their free state in nature?
5. Why do many transition element compounds have bright colors?