Transition element: Difference between revisions
Jump to navigation
Jump to search
imported>Paul Wormer |
imported>Paul Wormer No edit summary |
||
| Line 1: | Line 1: | ||
'''(Under construction)''' | '''(Under construction)''' | ||
A '''transition element''' is a [[chemical element]] element whose [[atomic electron configuration]] of the ground (lowest energy) state has an incompletely filled ''d'' sub-shell. The electron configuration contains (''nd'')<sup>''k''</sup>, with 1 ≤ ''k'' ≤ 9, and where ''n'' is a [[principal quantum number]]. The | A '''transition element''' is a [[chemical element]] element whose [[atomic electron configuration]] of the ground (lowest energy) state has an incompletely filled ''d'' sub-shell. The electron configuration contains (''nd'')<sup>''k''</sup>, with 1 ≤ ''k'' ≤ 9, and where ''n'' is a [[principal quantum number]]. The incomplete electronic ''d'' subshell gives rise to some characteristic magnetic properties and brightly colored solutions of transition metal complexes. | ||
Also the atoms [[copper]] (Cu), [[silver]] (Ag), and [[gold]] (Au) that have a filled ''d'' sub-shell, but after ionization have an incomplete ''d'' sub-shell, are usually seen as transition elements. | Also the atoms [[copper]] (Cu), [[silver]] (Ag), and [[gold]] (Au) that have in their lowest energy state a filled ''d'' sub-shell, but after ionization have an incomplete ''d'' sub-shell, are usually seen as transition elements. As seen in the table of electron configurations below, they have the configurations of outer electrons: (''nd'')<sup>10</sup>(''n''+1)''s''<sup>1</sup>, with ''n'' = 3, 4, and 5 for copper, silver, and gold, respectively. | ||
In the past the group 12 elements [[zinc]] (Zn), [[cadmium]] (Cd), and [[mercury]] (Hg), that are included in the "d-block" of the periodic table, | In the past the group 12 elements [[zinc]] (Zn), [[cadmium]] (Cd), and [[mercury]] (Hg), that are included in the "d-block" of the periodic table, have often been considered as transition elements, but they are nowadays rarely considered as such, because their compounds lack some of the characteristic properties. | ||
A strict application of the definition would describe [[lutetium]] (Lu) as a transition element as it has a singly occupied 5''d'' orbital in its ground state, but | A strict application of the definition would describe [[lutetium]] (Lu) as a transition element as it has a singly occupied 5''d'' orbital in its ground state, but according to IUPAC.<ref>{{cite news| url=http://www.iupac.org/reports/provisional/abstract04/connelly_310804.html | title =IUPAC Provisional Recommendations for the Nomenclature of Inorganic Chemistry (online draft of an updated version of the "''Red Book''" IR 3-6)| date =2004| accessdate = 17/9/2009}}</ref> it is a [[lanthanoid]] (previously known as lanthanide) It appears most commonly as a positive ion without ''d''-electrons in the valence shell and without the characteristic properties of a transition element. For the same reason [[scandium]] (Sc) and [[yttrium]] (Y) are often omitted from the list of transition metals. | ||
The | The first three series of the transition elements are shown in the two tables. The elements in Period 7, although formally transition elements, are man-made [except for Actinium (''Z'' = 87)] and are not shown. | ||
<br> | <br> | ||
| Line 18: | Line 18: | ||
background: #ffe; font-family: helvetica; font-weight: 500"> | background: #ffe; font-family: helvetica; font-weight: 500"> | ||
<caption> | <caption> | ||
< | <h4> | ||
Rows and columns of the [[Periodic Table of Elements]] containing transition elements </ | Rows and columns of the [[Periodic Table of Elements]] containing transition elements </h4> | ||
<center> The [[atomic number]] ''Z'' is between brackets</center> | <center> The [[atomic number]] ''Z'' is between brackets</center> | ||
</caption> | </caption> | ||
| Line 36: | Line 35: | ||
<th align="center" > 11 | <th align="center" > 11 | ||
<tr> | <tr> | ||
<td align="left" style="background:silver;font-weight: 600" > | <td align="left" style="background:silver;font-weight: 600" > 1st series </td> | ||
<td align="center" > Sc (21) </td> | <td align="center" > Sc (21) </td> | ||
<td align="center" > Ti (22) </td> | <td align="center" > Ti (22) </td> | ||
| Line 48: | Line 47: | ||
</tr> | </tr> | ||
<tr> | <tr> | ||
<td align="left" style="background:silver;font-weight: 600" > | <td align="left" style="background:silver;font-weight: 600" > 2nd series </td> | ||
<td align="center" > Y (39) </td> | <td align="center" > Y (39) </td> | ||
<td align="center" > Zr (40) </td> | <td align="center" > Zr (40) </td> | ||
| Line 60: | Line 59: | ||
</tr> | </tr> | ||
<tr> | <tr> | ||
<td align="left" style="background:silver;font-weight: 600" > | <td align="left" style="background:silver;font-weight: 600" > 3rd series </td> | ||
<td align="center" > La (57) </td> | <td align="center" > La (57) </td> | ||
<td align="center" > Hf (72) </td> | <td align="center" > Hf (72) </td> | ||
| Line 73: | Line 72: | ||
</table> | </table> | ||
</center> | </center> | ||
<br> | <br><br> | ||
<br> | |||
<center> | <center> | ||
<table width="45%" border="1" | <table width="45%" border="1" | ||
| Line 136: | Line 129: | ||
</table> | </table> | ||
</center> | </center> | ||
==Reference== | |||
<references /> | |||
Revision as of 07:49, 28 September 2009
(Under construction)
A transition element is a chemical element element whose atomic electron configuration of the ground (lowest energy) state has an incompletely filled d sub-shell. The electron configuration contains (nd)k, with 1 ≤ k ≤ 9, and where n is a principal quantum number. The incomplete electronic d subshell gives rise to some characteristic magnetic properties and brightly colored solutions of transition metal complexes.
Also the atoms copper (Cu), silver (Ag), and gold (Au) that have in their lowest energy state a filled d sub-shell, but after ionization have an incomplete d sub-shell, are usually seen as transition elements. As seen in the table of electron configurations below, they have the configurations of outer electrons: (nd)10(n+1)s1, with n = 3, 4, and 5 for copper, silver, and gold, respectively.
In the past the group 12 elements zinc (Zn), cadmium (Cd), and mercury (Hg), that are included in the "d-block" of the periodic table, have often been considered as transition elements, but they are nowadays rarely considered as such, because their compounds lack some of the characteristic properties.
A strict application of the definition would describe lutetium (Lu) as a transition element as it has a singly occupied 5d orbital in its ground state, but according to IUPAC.[1] it is a lanthanoid (previously known as lanthanide) It appears most commonly as a positive ion without d-electrons in the valence shell and without the characteristic properties of a transition element. For the same reason scandium (Sc) and yttrium (Y) are often omitted from the list of transition metals.
The first three series of the transition elements are shown in the two tables. The elements in Period 7, although formally transition elements, are man-made [except for Actinium (Z = 87)] and are not shown.
| Group | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 |
|---|---|---|---|---|---|---|---|---|---|
| 1st series | Sc (21) | Ti (22) | V (23) | Cr (24) | Mn (25) | Fe (26) | Co (27) | Ni (28) | Cu (29) |
| 2nd series | Y (39) | Zr (40) | Nb (41) | Mo (42) | Tc (43) | Ru (44) | Rh (45) | Pd (46) | Ag (47) |
| 3rd series | La (57) | Hf (72) | Ta (73) | W (74) | Re (75) | Os (76) | Ir (77) | Pt (78) | Au (79) |
| Z | Symbol | Element | Core | Configuration |
|---|---|---|---|---|
| 21 | Sc | Scandium | [Ar] | (3d)1 (4s)2 |
| 22 | Ti | Titanium | [Ar] | (3d)2 (4s)2 |
| 23 | V | Vanadium | [Ar] | (3d)3 (4s)2 |
| 24 | Cr | Chromium | [Ar] | (3d)5 (4s)1 |
| 25 | Mn | Manganese | [Ar] | (3d)5 (4s)2 |
| 26 | Fe | Iron | [Ar] | (3d)6 (4s)2 |
| 27 | Co | Cobalt | [Ar] | (3d)7 (4s)2 |
| 28 | Ni | Nickel | [Ar] | (3d)8 (4s)2 |
| 29 | Cu | Copper | [Ar] | (3d)10(4s)1 |
| 39 | Y | Yttrium | [Kr] | (4d)1 (5s)2 |
| 40 | Zr | Zirconium | [Kr] | (4d)2 (5s)2 |
| 41 | Nb | Niobium | [Kr] | (4d)4 (5s)1 |
| 42 | Mo | Molybdenum | [Kr] | (4d)5 (5s)1 |
| 43 | Tc | Technetium | [Kr] | (4d)6 (5s)1 |
| 44 | Ru | Ruthenium | [Kr] | (4d)7 (5s)1 |
| 45 | Rh | Rhodium | [Kr] | (4d)8 (5s)1 |
| 46 | Pd | Palladium | [Kr] | (4d)10 |
| 47 | Ag | Silver | [Kr] | (4d)10(5s)1 |
| 57 | La | Lanthanum | [Xe] | (5d)1 (6s)2 |
| 72 | Hf | Hafnium | [Xe*] | (5d)2 (6s)2 |
| 73 | Ta | Tantalum | [Xe*] | (5d)3 (6s)2 |
| 74 | W | Tungsten | [Xe*] | (5d)4 (6s)2 |
| 75 | Re | Rhenium | [Xe*] | (5d)5 (6s)2 |
| 76 | Os | Osmium | [Xe*] | (5d)6 (6s)2 |
| 77 | Ir | Iridium | [Xe*] | (5d)7 (6s)2 |
| 78 | Pt | Platinum | [Xe*] | (5d)9 (6s)1 |
| 79 | Au | Gold | [Xe*] | (5d)10(6s)1 |
| [Ar] stands for: | (1s)2(2s)2(2p)6 (3s)2(3p)6 | [18 electrons]. |
| [Kr] stands for: | [Ar](3d)10(4s)2(4p)6 |
[36 electrons]. |
| [Xe] stands for: | [Kr](4d)10(5s)2(5p)6 |
[54 electrons]. |
| [Xe*] stands for: | [Xe](4f)14 | [68 electrons]. |