d-block
| Period 4 after [Ar] | Period 5 after [Kr] | Period 6 after [Xe] | Period 7 after [Rn] | |||||||||||
| Scandium | 21 | 4s2 3d1 | Yttrium | 39 | 5s2 4d1 | Lutetium | 71 | 6s2 4f14 5d1 | Lawrencium | 103 | 7s2 4f14 7p1? | |||
| Titanium | 22 | 4s2 3d2 | Zirconium | 40 | 5s2 4d2 | Hafnium | 72 | 6s2 4f14 5d2 | Rutherfordium | 104 | 7s2 4f14 6d2? | |||
| Vanadium | 23 | 4s2 3d3 | Niobium | 41 | 5s1 4d4 | Tantalum | 73 | 6s2 4f14 5d3 | Dubnium | 105 | (unknown) | |||
| Chromium | 24 | 4s1 3d5 | Molybdenum | 42 | 5s1 4d5 | Tungsten | 74 | 6s2 4f14 5d4 | Seaborgium | 106 | (unknown) | |||
| Manganese | 25 | 4s2 3d5 | Technetium | 43 | 5s2 4d5 | Rhenium | 75 | 6s2 4f14 5d5 | Bohrium | 107 | (unknown) | |||
| Iron | 26 | 4s2 3d6 | Ruthenium | 44 | 5s1 4d7 | Osmium | 76 | 6s2 4f14 5d6 | Hassium | 108 | (unknown) | |||
| Cobalt | 27 | 4s2 3d7 | Rhodium | 45 | 5s1 4d8 | Iridium | 77 | 6s2 4f14 5d7 | Meitnerium | 109 | (unknown) | |||
| Nickel *[3] | 28 | 4s2 3d8 or 4s1 3d9 |
Palladium | 46 | 4d10 | Platinum | 78 | 6s1 4f14 5d9 | Darmstadtium | 110 | (unknown) | |||
| Copper | 29 | 4s1 3d10 | Silver | 47 | 5s14d10 | Gold | 79 | 6s1 4f14 5d10 | Roentgenium | 111 | (unknown) | |||
| Zinc | 30 | 4s2 3d10 | Cadmium | 48 | 5s2 4d10 | Mercury | 80 | 6s2 4f14 5d10 | Copernicium | 112 | (unknown) | |||
The d-block is the portion of the periodic table that contains the element groups 3-12.[4][5] These groups correspond to the filling of the atomic d-orbital subshell of the second outermost shell (inside an outermost shell only containing 1 or 2 s-orbital electrons) with electron configurations ranging from s2d1 (Group 3) to s2d10 (Group 12). There are some irregularities in the sequence; for example Cr is s1d5 (not s2d4) and the Group 11 metals are s1d10 (not s2d9), so that the d-subshell is actually complete at Group 11.
The d-block elements are often also known as transition metals or transition elements. However the exact limits of the transition metal region are usually not considered to be identical to the d-block. Although some authors do identify the entire d-block as transition metals,[4] most define transition metals as elements with partly filled d subshells either in the neutral atom or in ions in common oxidation states.[5][6] This definition has now been adopted by IUPAC corresponds to including only Groups 3-11 as transition metals. Group 12 metals lack the characteristic chemical and physical properties associated with incomplete d subshells and are considered post-transition metals. Jensen has reviewed the historical usage of the terms transition element (or metal) and d-block.[7]
In the s-block and p-block of the periodic table, similar properties across the periods are generally not observed: the most important similarities tend to be vertical, down groups. However the d-block is notable in that horizontal similarities across the periods do become important.
Although lutetium and lawrencium are in the d-block, they are not considered transition metals but a lanthanide and an actinide, respectively, according to IUPAC.[8] Group 12 elements are also in the d-block but are sometimes considered post-transition metals as their d-subshell is completely filled.[8]
| Group → | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 |
|---|---|---|---|---|---|---|---|---|---|---|
| ↓ Period | ||||||||||
| 4 | 21 Sc |
22 Ti |
23 V |
24 Cr |
25 Mn |
26 Fe |
27 Co |
28 Ni |
29 Cu |
30 Zn |
| 5 | 39 Y |
40 Zr |
41 Nb |
42 Mo |
43 Tc |
44 Ru |
45 Rh |
46 Pd |
47 Ag |
48 Cd |
| 6 | 71 Lu |
72 Hf |
73 Ta |
74 W |
75 Re |
76 Os |
77 Ir |
78 Pt |
79 Au |
80 Hg |
| 7 | 103 Lr |
104 Rf |
105 Db |
106 Sg |
107 Bh |
108 Hs |
109 Mt |
110 Ds |
111 Rg |
112 Cn |
[edit] See also
[edit] References
- ^ G.L. Miessler and D.A. Tarr, "Inorganic Chemistry" (2nd ed., Prentice-Hall 1999) p.38
- ^ See references in the article: electron configurations of the elements (data page)
- ^ Scerri, Eric R. (2007). The periodic table: its story and its significance. Oxford University Press. pp. 239–240. ISBN 0195305736. http://books.google.com/?id=SNRdGWCGt1UC&pg=PA239.
- ^ a b R.H. Petrucci, W.S. Harwood and F.G. Herring “General Chemistry” (8th ed, Prentice-Hall 2002), p.341-2
- ^ a b C.E. Housecroft and A.G. Sharpe “Inorganic Chemistry” (2nd ed, Pearson Prentice-Hall 2005), p..20-21
- ^ F.A. Cotton and G. Wilkinson “Advanced Inorganic Chemistry” (5th ed, John Wiley 1988) p.625
- ^ Jensen, William B. (2003). "The Place of Zinc, Cadmium, and Mercury in the Periodic Table". Journal of Chemical Education 80 (8): 952–961. Bibcode 2003JChEd..80..952J. doi:10.1021/ed080p952. http://www.uv.es/~borrasj/ingenieria_web/temas/tema_1/lecturas_comp/p952.pdf.
- ^ a b IUPAC Provisional Recommendations for the Nomenclature of Inorganic Chemistry (2004) (online draft of an updated version of the "Red Book" IR 3-6)
