does transition metals have more than one oxidation state?
920446
Yes, they do. The simplest example I can do is Fe (iron): it's a transition metal and has 3 oxidation states: 0 (Fe as a metal), +2 (FeO), and +\n3 (Fe2O3).
6677
Group I elements almost always have an oxidation number of +1, so the K (potassium) has a +1.  Unless they're in peroxide compounds, which is not the case here, oxygen usually has an oxidation number of -2.  The hardest one is the Mn.  We know that the whole compound has to have an oxidation number of 0, so let's do some math.  There is one +1, and there are 4 oxygens, each with -2.  \n+1 + ? + 4*(-2)=0\nThe answer is +7.  Therefore, Mn must have an oxidation number of +7. \nK=+1, Mn=+7, O=-2
761557
Any atom in main group chemistry can only have a maximum of 8 electrons in its valence orbital (outter shell).\n\nelements want to have this magic number of 8 electrons in there outter shell.  For example the formation of NaCL.  Sodium (Na) has 1 electron in its outter oribital, chlorine (CL) has 7 electrons in its outter shell.  Therefore Na and CL want to form an ionic compund so they both have 8 electrons in there outter shell.\n\nCovalent compounds work in a similar way, except There will be transfer of electrons rather than electron sharing.\n\nThe reason its 8 is because of the S and P orbitals.  there can be a maximum of 2 in the S orbital and 6 in the P orbital.  \n\nThis is an over simplification though as there are orbitals which can hold more than 8 electronsd and f orbitals in the transition metals), but its the basic idea you are taught at your level of chemistry ^^
827746
oxidation state for oxygen is usually -2 but it sumtimes have -1
266785
General \nName, Symbol, Number osmium, Os, 76 \nChemical series transition metals \nGroup, Period, Block 8, 6, d \nAppearance silvery, blue cast\n \nAtomic mass 190.23(3) g/mol \nElectron configuration [Xe] 4f14 5d6 6s2 \nElectrons per shell 2, 8, 18, 32, 14, 2 \nPhysical properties \nPhase solid \nDensity (near r.t.) 22.61 g/cm³ \nLiquid density at m.p. 20 g/cm³ \nMelting point 3306 K\n(3033 °C, 5491 °F) \nBoiling point 5285 K\n(5012 °C, 9054 °F) \nHeat of fusion 57.85 kJ/mol \nHeat of vaporization 738 kJ/mol \nHeat capacity (25 °C) 24.7 J/(mol·K) \nVapor pressure P/Pa 1 10 100 1 k 10 k 100 k \nat T/K 3160 3423 3751 4148 4638 5256 \n \nAtomic properties \nCrystal structure hexagonal \nOxidation states 8, 6, 4, 2, -2\n(mildly acidic oxide) \nElectronegativity 2.2 (Pauling scale) \nIonization energies 1st: 840 kJ/mol \n2nd: 1600 kJ/mol \nAtomic radius 130 pm \nAtomic radius (calc.) 185 pm \nCovalent radius 128 pm \nMiscellaneous \nMagnetic ordering  ? \nElectrical resistivity (0 °C) 81.2 nΩ·m \nThermal conductivity (300 K) 87.6 W/(m·K) \nThermal expansion (25 °C) 5.1 µm/(m·K) \nSpeed of sound (thin rod) (20 °C) 4940 m/s \nShear modulus 222 GPa \nPoisson ratio 0.25 \nBulk modulus 462 GPa \nMohs hardness 7.0 \nBrinell hardness 3920 MPa \nCAS registry number 7440-04-2 \nNotable isotopes \nMain article: Isotopes of osmium iso NA half-life DM DE (MeV) DP \n184Os 0.02% >5.6×1013y α 2.966 180W \n185Os syn 93.6 d ε 1.013 185Re \n186Os 1.58% 2.0×1015y α 2.822 182W \n187Os 1.6% Os is stable with 111 neutrons \n188Os 13.3% Os is stable with 112 neutrons \n189Os 16.1% Os is stable with 113 neutrons \n190Os 24.6% Os is stable with 114 neutrons \n191Os syn 15.4 d β- 0.314 191Ir \n192Os 41.0% Os is stable with 116 neutrons \n193Os syn 30.11 d β- 1.141 193Ir \n194Os syn 6 y β- 0.097 194Ir \n \nReferences \nOsmium is a chemical element in the periodic table that has the symbol Os and atomic number 76. A hard brittle blue-gray or blue-black transition metal in the platinum family, osmium is the densest natural element and is used in some alloys with platinum and iridium. The extraordinary density of osmium is a consequence of the lanthanide contraction. Osmium is found native as an alloy in platinum ore and its tetroxide has been used to stain tissues and in fingerprinting. Alloys of osmium are employed in fountain pen tips, electrical contacts and in other applications where extreme durability and hardness are needed.\n\nand real close to it is Iridium
950877
Stock numbers are used when an element has multiple oxidation states. Oxygen's only oxidation state is -2, helium's is 0, and hydrogen is always +1 or -1 (the charge will be obvious based on whatever it's bonded to). Thus, the answer is Sulfur, with oxidation states of -1, +/- 2, 4, and 6.
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.
473338
It's all the elements in the d-block of the periodic table. Basically, the group starting from column three to column twelve. These transition metals commonly have many oxidation states and have either partially filled d-orbitals or full d-orbitals (like mercury). They also form complex ions quite readily.\n\nIf all of that doesn't make sense, just remember it's the metals in that "lowered" part in the middle.
486351
Cu.\nIt is a transition metal with ions of Cu+ and Cu2+.
427299
They are different terms for talking about the same thing.  Many elements have several valences. Iron, for instance has common valences of 0, +2 and +3.  You can say that iron metal exhibits a valence of 0 or that iron as metal is in the 0 oxidation state.\n\nSimilarly, iron (II) oxide  (FeO) exhibits a valence of 2 or is in the +2 oxidation state.\n\nI guess there is a fine point here: iron always has valences of 0, 2, 3 etc. but it doesn't exhibit them all at once.  Note that it can exhibit more that one valence at a time.  Iron in Fe3O4 exhibits +2 and +3 valences at the same time and so has a mixed oxidation state.
977688
Metals are reductants. that is they cause reduction in a reaction and are themselves oxidised. This means they must GIVE UP electrons. If you look at the periodic table, as you go down a group (say 1st gorup), atoms have more and more shells ( the outer which contains only 1 electron). As you know, the more shells there are, the lesser tehy will be bound to the nucleus (as they experience weak core charge). This means at the bottom of the 1st group, atoms will almost willingly get rid of its valence electron. So that's why as you go down a group, they are more metallic.\n\nAs you go from the left to the right of the PT, there are more electrons in the outer shell. THis means they more and more act as an oxidant (causing oxidation to others, but in turn gets reduced). Thus, they are less metallic
37559
A 'transition metal'  11,4,d
852794
dobereiner's like that mendeleev guy right? if my memory is right, all  of the elements above have similar chemical properties, that's why he placed them in his "triads". This means that all of them act similarly. Remember that it is the VALENCE electrons that causes the specific reaction of an element. So, as all three elemnts have the same number of valence electrons, they act similarly.
333129
An element will become stable when it's outermost electron (valence) shell is full.  In most cases, the valence shell will contain 8 electrons when stable.  Hydrogen and helium only require 2 electrons.  \n\nIn order to achieve a full set, atoms can gain or lose electrons forming ionic compounds.  This normally happens between metals and nonmetals on the periodic table.  Alternatively, atoms can share electrons forming covalent compounds, which generally occurs between two nonmetals.
932025
You mean the Valence Shell Configuration?\n\nIt is easy to find this by simply looking at the Group # (these are the column numbers). \n\nElements in Group 1 all have 1 electron in their valence shell, Elements in group 2 have 2 and so on...\n'\nIf you mean how many shells there are then look at the Period #  this is the horizontal groups) the Period # corresponds with the number of electron shells.\n\nElements in Period 2 have 2 electron shells, elements in Period 3 have 3 and so on...
373061
yes. in order for an atom to be stable, it must have eight valence electrons. In other words, each atom wants to have eight valence electrons. On the periodic table, you can determine what element can form a bond with any other elements. There are some elements which are an exception to the eight valence rule.
173111
Well, they're both transition metals, so they can have multiple charges, or oxidation states. Rhodium exists in the 0 state (elemental), +2, +3, and +4. Palladium exists in the 0 state, -1, and +1.