what are transition metals?
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The elements in the periodic table that have partially filled d orbitals. E.G. ytterbium
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the Soviet Union\n\nThis website might help:\nhttp://en.wikipedia.org/wiki/Titanium
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Here is one : http://en.wikipedia.org/wiki/Periodic_table
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oxygen, nitrogen, every fuckin mineral and more on the periodic table...take chemistry
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Metal\n\nChemical properties\n\nMost metals are chemically unstable, reacting with oxygen in the air to form oxides over varying timescales (for example iron rusts over years and potassium burns in seconds). The alkali metals react quickest followed by the alkaline earth metals, found in the leftmost two groups of the periodic table. The transition metals take much longer to oxidise (such as iron, copper, zinc, nickel). Others, like palladium, platinum and gold, do not react with the atmosphere at all. Some metals form a barrier layer of oxide on their surface which cannot be penetrated by further oxygen molecules and thus retain their shiny appearance and good conductivity for many decades (like aluminium, some steels, and titanium). The oxides of metals are basic (as opposed to those of nonmetals, which are acidic), although this may be considered a rule of thumb, rather than an absolute condition.\n\nPainting or anodising metals are good ways to prevent their corrosion. However, a more reactive metal in the electrochemical series must be chosen for coating, especially when chipping of the coating is expected. Water and the two metals form an electrochemical cell, and if the coating is less reactive than the coatee, the coating actually promotes corrosion.\n\nPhysical properties\n\nTraditionally, metals have certain characteristic physical properties: they are usually shiny (they have "lustre"), have a high density, are ductile and malleable, usually have a high melting point, are usually hard, and conduct electricity and heat well. However this is mainly because the low density, soft, low melting point metals happen to be reactive, and we rarely encounter them in their elemental, metallic form. Metals conduct sound well, that is, they are sonorous.\n\nThe electrical and thermal conductivity of metals originate from the fact, that in the metallic bond the outer electrons of the metal atoms form a gas of nearly free electrons, moving as an electron gas in a background of positive charge formed by the ion cores. Good mathematical predictions for electrical conductivity, as well as the electrons' contribution to the heat capacity and heat conductivity of metals can be calculated from the free electron model, which does not take the detailed structure of the ion lattice into account.\n\nWhen considering the exact band structure and binding energy of a metal, it is necessary to take into account the positive potential caused by the specific arangement of the ion cores - which is periodic in crystals. The most important consequence of the periodic potential is the formation of a small band gap at the boundary of the brillouin zone. Mathematically, the potential of the ion cores is treated in the nearly-free electron model.\n\nNonmetal\n\nMost nonmetals are found at the upper right of the periodic table. The exception is hydrogen, which is usually placed at the upper left with the alkali metals, but behaves like a nonmetal under most conditions. Unlike metals, which are electrically conductive, nearly all nonmetals are either insulators or semiconductors. Graphite, an allotrope of carbon, is an example of a nonmetal that does conduct electricity. Nonmetals may form ionic bonds with metals by gaining electrons, or covalent bonds with other nonmetals. The oxides of nonmetals are acidic.\n\nThere are only eighteen known nonmetals, compared to over eighty metals, but nonmetals make up most of the earth, particularly in the outer layers. Organisms are composed almost entirely of nonmetals. Many nonmetals (hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine) are diatomic, and most of the rest are otherwise polyatomic.\n\nMetalloid\n\nTogether with the metals and nonmetals, the metalloids (in Greek metallon = metal and eidos = sort) form one of the three categories of chemical elements as classified by ionization and bonding properties. They have chemical properties intermediate between those of metals and no
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The general properties of metals are:\nThey are usually solid (exception is mercury) - argon is a gas\nThey all conduct electricity - argon doesn't conduct electricity\nThey form salts with acids - argon doesn't form any compounds let alone salts.\nThey conduct heat well - argon is a very poor conductor of heat.\nSo argon doesn't qualify as a metal on any count.
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Iridium (IPA: /ɪˈɹɪdiəm/) is a chemical element in the periodic table that has the symbol Ir and atomic number 77. A dense, very hard, brittle, silvery-white transition metal of the platinum family, iridium is used in high strength alloys that can withstand high temperatures and occurs in natural alloys with platinum or osmium. Iridium is notable for being the most corrosion resistant element known and for its significance in the determination of the probable cause of the demise, by a meteorite strike, of the dinosaurs. It is used in high temperature apparatus, electrical contacts, and as a hardening agent for platinum.
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Inorganic chemistry & Analytical chemistry.\nInorganic: Branch is called metallurgy which is all about metals & the reqd alloys for making guns\nAnalytical: For preparing the bullets which should explode on impact proving fatal to the living organisms at which they r targeted
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Basically CO is a very good ligand to transtional metals because of it great pi accepting properties of it anti bonding orbital with it interation with metal d orbitals. \n\nTherefore any transitional metal form good absorber with CO, example is that of Fe.
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Transition elements have some anomolous properties . The transition shows horizontal similarity and they have variable valencies. Instead of the gradation in properties, they show variety in properties. The groups like lanthanides and actinides are separated from the transition metals due to their unique properties. The transition elements includes differents  group of elements with  unique properties
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http://chemistry.allinfoabout.com/features/nonmetals.html
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Yeah, there are some special cases with some transition metals, and you're right with groups 6 and 11.  \nYou'd expect for the Cu (and the other elements in that column) to have the electron configuration [Ar]4s2 3d9.  \nInstead, the configuration is [Ar]4s1 3d10.  This configuration is more stable because the d sublevel is completely filled.  Cr's valence electron configuration (and the rest of the column's) is expected to be 4s2 3d4, but it is actually 4s1 3d5.  There is added stability in the exactly half-filled d sublevel.
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Iron = Transition Metal\nCobalt = Transition Metal\nSodium = Metal (oddly enough)\nOxygen = Nonmetal (gas)\nHelium = Nonmetal (noble gas)
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A 'transition metal'  11,4,d
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Intermetallic bonding is definitely confusing....\n\nFirst to review titanium chemically....All 'transition' metals are called as such because the the electrons in their outer-most shells keep shifting from one orbital to another and never stay put. This is why transition metals form compounds with variable oxidation states/valencies, as they don't always donate a fixed number of electrons, unlike group 1 and 2 elements which always donate 1 and 2 electrons respectively. So if a transition metal like titanium is to combine with another metal, then the resulting compound would not have a fixed formula, as you justified by mentioning TiAl and TiAl3.\n\nWhen 2 metals are to combine, both of them would donate electrons and since neither of the 2 metals would accept them, the donated electrons form an electron cloud around the atoms. Imagine it as 2 positive charges (nuclei of both metallic atoms) surrounded by a negatively charged cloud. The electron cloud is held in place by the attractive force of the nuclei for the electrons. \nIf 2 non-transition metals combine, the electron cloud formed would contain the fixed number of electrons that each metal would donate. If 2 transition metals combine or a transition metal combines with a non-transition metal, the electron cloud would vary in the number of electrons in it. \n\nConsider the electronic configuration of Ti and Al: \n1s2, 2s2, 2p6, 3s2, 3p6, 3d2, 4s2. [titanium]\n1s2, 2s2, 2p6, 3s2, 3p1 [aluminum]\nTitanium would donate 4 electrons from 4s2 and 3d2 to achieve noble gas configuration of argon. As stated at the beginning, the electrons in 3p and 3d orbitals would keep shifting to and fro, so it may happen that at one point, 2 electrons from 3s orbital shift to 3d, and the like. So each time titanium has to bond with aluminum, it may donate 4 or more than 4 electrons.\nIf at one point, 1 titanium atom donates 4 electrons from 4s2 and 3d2 and 4 aluminum atoms donate 1 each from 3p1, then both will have a complete orbital (for Al) and a complete shell (for Ti) left. So with 1 Ti atom and 4 Al atoms, the compound formed will be TiCl4. Other compound like TiAl will be formed according to the number of atoms (of both metals), and the number of electrons they donate.
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I actually asked an inorganic chemist the very same question, and this is what he told me:\nI seperated out the section that I thought was the best reason he gave, and I think it's important to read the last paragraph.  His other reasoning seems good, too.  I'm not trying to say it doesn't make sense.  I just think the part I seperate is probably what they had in mind when designating the groups.\n\n When you say they are put into the same "group" I assume you mean the group B numbering within the transition metals columns, which would make the Fe, Co and Ni triads all part of group VIIIB.  Now with the main group, also termed group A, the significance of the roman numeral to signify the standard oxidation state of the element is obvious.  The oxidation states get more complex in the transition metal series and frequently multiple oxidation states are observed.  The Cu triad (Cu, Ag, Au) is termed IB due to stable +1 states that are common especially silver which is only found as elemental or +1, where copper may alos be found as a +2 and Au may be found as +3.  The Zn triad (Zn, Cd, Hg) are exclusively +2 and are thus labled IIB group.  You then skip back to the begining of the transition metals and number across due to stable +3 and +4 for Sc triad and Ti triad respectively.  There are a few reasons why in the classical B grouping Fe, Co, and Ni are lumped into a "group" in the middle of the transition metal series.  First as you go across the transition metals the +2 state is becomeing continuously more stable and prevalent.  For Fe there are several oxidations states that are common, however +2 and +3 are most stable and common.  When you move over to Co the +2 becomes the dominant oxidation state with +3 also commmon and very rare examples of higher oxidation states.  When you move over to Ni it is almost exclusively +2 or +3 with rare exceptions.  The second point that I would consider in grouping them together would be their adherence to the 18 elecron rule.  These elements in the middle of the transition metall series follow the rule almost always where earlier elements frequently violate the rule with lower electron counts or even odd number counts and the later elemnts are frequently content with 16 or even 14 electron counts, the later condition is common for group IIB.  \n\n\nAnother consideration to give this group the lable VIIIB is the d8 configuration that is common (Fe(0), Co(I), and Ni(II)) are all d8 systems and frequently analogous compounds can be made with the different metals.  \n\nI hope this shed some light on your question.  I also should note that the system that groups these elements together is an older group numbering system and the new and current grouping system avoids the grouping by groups A and B and simply numbers across the table from 1 to 18, with groups 3-12 being the transition metals.
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Common valences are the normal number of chemical bonds that must be formed to stabilize an atom. For example, for oxygen its 2-, because O shares 2 electrons to become stable. For hydrogen its 1+, since hydrogen receives one electrons.\n\nSome metals have more than one valence. For instance:\nCu: 2+, 3+\nHg: 2+, 4+ (I think)\n\nAnyway, these valences are the common valences for these atoms. Under extreme conditions the common valences may change.