What do you know about complex ions and transition metals?
337610
Transitional metals are the metals in the middle of the periodic table of elements.
974325
You should probably need your periodic table.\nGenerally chemical formulas are for ionic compounds, hence you need to know the charges of the ions formed.\nAll Group I metals form ions of +1 charge, Group II metals forms +2 charged ions, Group III (like Al) forms +3 charge, Group IV prefers to share, seldom will they form ions, hence we shall keep them out of the picture.\nGroup V non-metals form -3 charge, Group VI -2 and Group VII -1. Group O elements have full outermost shell, hence they seldom participate in bonding.\nSo if you are looking at magnesium oxide, the ionic compound is formed between magnesium ion (Group II, hence Mg2+) and the oxide ion (from oxygen, Group VI, hence O2-).\nYou will realise that to balance the charges, you need exactly 1 Mg2+ and 1 O2-. Hence the chemical formula of magnesium oxide is MgO.\nAnother example, for sodium chloride. Sodium ion (Na+) and chloride ion (Cl-). Hence 1 of each is needed to balance the charges and the formula is NaCl.\nAnother example, lead (IV) oxide. Lead is a transition metal and transition metals form ions of variable valencies. Lead (IV) means the charge of the lead ion here is Pb4+. Thus you need 1 Pb4+ and 2 O2- (so that the charges are cancelled) for lead (IV) oxide, PbO2.\nYou have also polyatomic ions, like hydroxide (OH-), sulphate [(SO4)2-], nitrate [(NO3)-] and carbonate [(CO3)2-]. Similarly, ionic compounds formed will require the balance of charges.\nExample, with sodium sulphate.\nYou have Na+ and sulphate [(SO4)2-].\nYou will need 2 sodium ions to balance the -2 charge of the sulphate ion. Hence the chemical formula is Na2SO4.\nHope this helps. :)
364266
Metal carbonyls are organometallic complexes of transition metals with carbon monoxide.
1053722
Here's are a few:\nhttp://www.science-house.org/learn/CountertopChem/exp25.html\nhttp://www.chymist.com/copper%20silver%20gold%20expl.pdf\nhttp://chemlearn.chem.indiana.edu/demos/15-7%20TheGold1.htm
978327
When a ligand binds to Cu, it splits the 5 d orbitals into two groups (off the top of my head I cant remember the names but I think they are t2g and eg).  The color results from electrons transitioning between the two d orbital levels.  Different ligands split the orbitals different amounts so you get different wavelengths of light emitted.  \nAlso, since it is technically forbidden to have an electron transfer within an orbital level, the d-d transition peaks are much smaller than other electron transitions.
706761
Ok I honestly don't remember learning complex chemistry in the 7th grade, but it wasn't too far ago (I'm a senior). For any chemistry test, I study the equations and rules used. As for chemical bonding, remember the differences between single replacement, double replacement, etc. depending on how complex or simple it is. For making ions, study up on their rules, and the number of valence electrons it has and which other elements it can combine to. \n\nHope this helps! :)
1008643
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.
125410
Do you mean "transition" metals?  I guess you could call them intermediate metals, I have just never heard anyone use that term.\n\nTransition [intermediate] metals tend to develop positive charges when ionized.  Two positively charged ions will repell eachother, there is not too good of a chance they will interact, much less bond.
303566
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.
581650
Give an example.  Cr2 is not a common ion.  Molecules usually have two Cr(+3) or two Cr(+6) ions.\n\n******************************\n\nIt is two Cr(+6) atoms.\n\n2 (+6) + 7(-2) = -2   \noxygen is -2 valence / ox #
84628
the study of metals. their characteristics, and behaviours, etc.
892250
Zirconium is a metal (transitional metal, to be precise).\nChlorine is a non-metal (halogen).\nGold is a metal (also a transitional metal).\nUnunnilium (now called darmstadtium) is a metal (transitional metal, too.).
418822
metals: give up electrons in ionic bonds. They also form metallic bonding.  sodium, potassium, lithium, to name just a few. There are a lot of metals\n\nnonmetals: this is more more difficult group to describe. They materials like to form covalent bonds--a joint sharing of two electrons. Both hydrogen and oxygen are nonmetals. But hydrogen gives up its electon in an ionic bond. For example HCl. It that repect it acts similar to a metal. Carbon is also a nonmetal\n\nMetaloid: silicon, germanium, boron, arsenic, antamony. These elements are right on the line between metals and nonmetals. As a result they make good semi conductors.
1013102
Temporary electrostatic complexes where each ion retains their coordinated waters, but they are still close enough to effectively form a complex between the metal and the ligand.  \nUsually form beween Hard cations and anions \nAnother term is outer sphere complex.  These complexes are difficult to analyze directly, and are normally estimated from coulombic attraction and Bejerrum's ion association model; \nThe log Kstab of ion pair complexes range from ~0 to 4, depending on charge density \nThere can be ion pair or coordinative complexes for the same pair of ions, with an equilibrium established between them.  The major ion pairs in water are: \nCaHCO3+, ; CaSO4°; CaOH+; MgCO3°; MgSO4°\n\nThe degree of interaction is only slightly greater than the electrostatic interactions accounted for by the DeBye-Huckel theory, but this is enough to change activities. \nIon pairs become more important in saline waters and brines, where the interactions must be specifically accounted for using the Pitzer Equations. \n\n\n\nget to this link and you find the whole :)
868490
assuming you know basic chemistry:\nall metals are cations, right? that means they have + electrons and will bond with non metals easily to form salts. NaCl for example, sodium being the metal, chlorine being the nonmetal.\n\nwell what happens with metal solids and aloys is this: all those extra "valence" electrons floating around their full largest P full shell (you know, 1s2, 2s2, 3p6 and so on..) create a system of delocalized electrons which allow the metals to bond together. since this free system of electrons exists all around the metals that explains why electrons are able to pass through solid metals so easily. (conductivity). the system also give various metals and alloys the ability to be very strong, or rust proof, etc.
1057954
Yes, metals can form complexes.  Like, Pt2(PPh3)6 and things of that nature.  I wasn't exactly wholly attentive in inorganic, but we discussed many complexes of that sort.  I hope this answers your question, I'm not sure what you meant by "sea of electrons".  Usually that term talks about metal in it's elemental state, made into sheets/wires, where the electrons are free to move when voltage is applied.
201939
a.)ionic b.)covalent c.)covalent d.)metallic