Transition metal

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(Created page with "<u>What Is a Transition Metal?</u> Transition metals are d-block elements between the second and third groups in the periodic table. Ex...")
 
 
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<u>What Is a Transition Metal?</u>  
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=== <u></u>'''What Is a Transition Metal?'''<u></u> ===
  
Transition metals are d-block [[Element|elements]]&nbsp;between the second and third groups in the&nbsp;[[Periodic table|periodic table]]. Examples of well-known transition metals include titanium, iron, nickel, and copper. They are unique from other elements due to their ability to form an incomplete d sub-shell in the form of&nbsp;at least one ion.<ref>1</ref>  
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Transition metals are d-block [[Element|elements]]&nbsp;between the second and third groups in the&nbsp;[[Periodic table|periodic table]]. Examples of well-known transition metals include [[titanium|titanium]], [[iron|iron]], [[nickel|nickel]], and [[copper|copper]]. They are unique from other [[Element|elements]] due to their ability to form an incomplete [[d sub-shell|d sub-shell]] in the form of&nbsp;at least one ion&nbsp;<ref>Gent D. and Ritchie R (2008), OCR Chemistry (A2), Heinmann</ref>.<br>  
  
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=== <u></u>Exceptions<u></u>  ===
  
<u>Exceptions</u>  
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Although [[scandium|scandium]] and [[zinc|zinc]] are found within the d-block of the [[Periodic table|periodic table]], they are not in fact usually classified as transition metals because they do not fully fulfil the necessary criteria. This is due to the fact that scandium can only form one ion with a charge of 3<sup>+</sup>, but with d orbitals that have no electrons occupying them; zinc on the other hand can only form an ion with a charge of 2<sup>+</sup>, but with electrons that fully occupy its d-orbitals&nbsp;<ref>Gent D. and Ritchie R (2008), OCR Chemistry (A2), Heinmann</ref>.<br>  
  
Although scandium and zinc are found within the d-block of the [[Periodic table|periodic table]], they are not in fact usually classified as transition metals because they do not fully fulfil the necessary criteria. This is due to the fact that scandium can only form one ion with a charge of 3+, but with d orbitals that have no electrons occupying them; zinc on the other hand can only form an ion with a charge of 2+, but with electrons that fully occupy its d-orbitals.<ref>2</ref>
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=== References  ===
  
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<u>References</u>
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<references />&nbsp;Gent D. and Ritchie R (2008), OCR Chemistry (A2), Heinmann &nbsp;<references />
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Latest revision as of 11:38, 20 October 2012

What Is a Transition Metal?

Transition metals are d-block elements between the second and third groups in the periodic table. Examples of well-known transition metals include titanium, iron, nickel, and copper. They are unique from other elements due to their ability to form an incomplete d sub-shell in the form of at least one ion [1].

Exceptions

Although scandium and zinc are found within the d-block of the periodic table, they are not in fact usually classified as transition metals because they do not fully fulfil the necessary criteria. This is due to the fact that scandium can only form one ion with a charge of 3+, but with d orbitals that have no electrons occupying them; zinc on the other hand can only form an ion with a charge of 2+, but with electrons that fully occupy its d-orbitals [2].

References

  1. Gent D. and Ritchie R (2008), OCR Chemistry (A2), Heinmann
  2. Gent D. and Ritchie R (2008), OCR Chemistry (A2), Heinmann
 
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