which orbitals are excited states?
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Any orbital can be considered within an excited state depending of the given element and its charge.
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Color requires large orbitals to absorb light.  Metal elements are larger than most common non-metal elements, and hence they are more likely to have color than, say, common organic molecules.  However, organic molecules can have conjugated orbitals, which become larger than a single atome and hence are abale to give a coloration in the visible range of the spectrum (as is seen in chlorophyll and carteinoids which color vegetables).  So metal atoms do generally give color, but large molecules with smaller atoms can also make color if the orbitals are conjugated.
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Atoms that are excited have electrons that jump out of their regular shells.  Excited atoms emit color based on how far out they jump.  Ground state of atoms are their normal electron orbit.\nHope that helped
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1.ATOMIC NUMBER\n2.ELECTRON\n3.SHELL\n4.ORBIT
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Violet12.. is right on both questions. Now, about the second question:\n\nFor the 4s orbital: n + l = 4 + 0 = 4.\nFor the 3d orbital: n + l = 3 + 2 = 5\n\n4 < 5, so the 4s orbital has less energy than 3d, so we put electrons first in 4s orbital and then in 3d.
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Here is what I got\nhttp://img.photobucket.com/albums/v628/kerahna/lewis.jpg\n\nPretend the Xs are all dots. I just draw Xs to keep track of which electron belongs to which atom. They are all the same.\nI haven't checked the formal charges yet, I'm going to do that now.\n\nEDIT: The formal charges are good.
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well i cant help you with the lewis structure cuz i dunno what that is. but the bohr diagram is   um hard to explain without drawing it out. ill try. \nfirst you draw a circle and the number of protons and neutrons in them (#protons is atomic number and #neutrons is mass=#protons). and then you draw an orbital around that circle and draw 2 dots on that orbital (corresponding to 2 electrons, there is a max of 2 electrons in the first orbital). then you draw another orbital around it and you can put up to 8 electrons (dots) on it. and then if you need another one, then you can put up to 8 on it and so on. the number of electrons you have to put is the same as the number of protons. and dont draw the empty orbitals.\n\nhope that helps. let me know if u need more help. later
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http://submarine.dyndns.org/~tofu702/Science/Physics_Book/PhysicsBookFull.pdf\n\nInduced absorption and stimulated emission in the ground state of a three-level atom\nC Mavroyannis 1992 Quantum Opt. 4 145-150   doi:10.1088/0954-8998/4/3/001\n\n   \n     PDF (237 KB) | References | Articles citing this article \n  \n   \n\nC Mavroyannis\nSci. Inst. for Molecular Sci., Nat. Res. Council of Canada, Ottawa, Ont., Canada\nAbstract. Studies the competition between absorption and stimulated emission induced by two laser fields at low intensities interacting on a two-photon resonance with a three-level atom. The induced spectrum into the ground state consists of a peak whose height and asymmetry depend strongly on the detuning. The spectra arising from the emission of a laser photon by the excited state consists of two peaks describing stimulated emission and induced absorption, respectively, where the former dominates the latter for small values of the Rabi frequencies but for higher ones, they cancel each other out. \n\nPrint publication: Issue 3 (June 1992)\n\n\nPDF (237 KB) | References | Articles citing this article
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Valence electrons are those electrons in an atom outside the noble-gas core.  Valance electrons are the electrons in the outermost principal quantum level.  Valance electrons are the electrons which are most often involved in reactions and forming chemical bonds.\n\nPotassium has a single valence electron, 4s1, which comes from the 4s subshell.\n\nChlorine has a total of seven valence electrons, 3s2 3p5, two from the 3s subshell and five from the 3p subshell.\n\nGold = 5d10 6s1\n\nNeodymium - 4f4 6s2\n\nYou can look up each element at the site below.
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a.  Expanded shell/with 6 pairs of electrons around the central molecule.\n\nb.  Expanded octet with four shared pairs and one unshared pair.\n\nc.  Not sure but free radical with one double bond between an oxygen and and Cl.
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Protons, Neutrons, and electrons
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Orbitals are solutions to the schrodinger wave equation, quantum mechanics, taking into account translation, number, and rotation, letter.  The rotational levels, s p d f, are from the symmetry of the solutions.  With lower levels of translational energy the higher symmetries do not exist.\n\nsee the source from "Solution of Schrödinger equation: Overview of results" and down for a true mathematical explaination.
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Quantum numbers are used to describe every single electron in an atom or molecule. Each electron is assigned it's own set of four different quantum numbers. no electron in the same atom or molecule can have the same set of quantum numbers.\n\nIn atoms:\nn = the principle quantum number. It is an integer, starting with 1, then 2, then 3, and so forth. This tells the principle energy level that the electron occupies. On the periodic table, the row number tells the higest principle quantum number an electron in that elemet can have. For example, the lone electron in hydrogen is always in the n = 1 energy level. However, an element like iodine in the 5th row can have electrons all the way up to the n + 5 energy level.\n\nl is the angular momentum quantum number. It is an integer that ranges from 0 to n-1. This number determines the shape of the electrons orbital. 0 is a sphere. 1 is dumbell shapped. 2 is two dumbells. 3 is 6 dumbells. These orbital shapes are usually represented with letters: 0 = s, 1 = p, 2 = d, 3 = f, 4 = g, and so on. s,p,d,f are the most commonly seen. Since l can range from 0 to n-1, n determines which orbital shapes the electrons in a given atom can have. In the first row, only s is possible. The second row adds p orbitals, and the third row adds d orbitals. Even though no atoms in the third row have occupied d orbitals in the ground state, they are still avaliable for bonding or excited state electrons (which explains why sulfer can and often does form more than 4 bonds)\n\nm is the magnetic quantum number. It simple tells the orientation of the orbitals. It ranges from -l to l. s orbitals have l = 0, so there is only one orientation. p orbitals have l = 1, so there are three, corresponding to m = -1, m= 0, and m = 1. d orbitals have 5 orientations, and f orbitals have 7. The number of orientations is also equal to the number of each type of orbital an atom (1 s orbital, 3 p orbitals, 5 d orbitals, 7 f orbitals) per energy level.\n\nm sub s (written as an m with a subscript s) is thespin quantum number. Every orbital can hold two electrons, however due to Pauli's Exclusion Principle, they can't have the same set of quantum numbers. The spin quantum number is either +1/2 or - 1/2, and it determines the direction of the electron's "spin." This isn't spin in the normal sense, as electrons don't spin like tops.
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The ligand will accomodate electrons from the ligands, forming dative bonds.\n\nThe sub-shell also ceases into two groups of orbitals.  One group will be at a higher energy level as compared with the other.  The difference in energy level is acounted by the strength of the ligand, in other words, by its polarising power.  The stronger the ligand, the greater is the energy difference between the two groups of orbitals.
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the condition of an atom or molecule after absorbing energy from exposure to light, electricity, elevated temperature, or a chemical reaction, and which may be a necessary prelude to a chemical reaction or to the emission of light.\n\nExcited state \nIn quantum mechanics, a stationary state of higher energy than the lowest stationary state or ground state of a particle or a system of particles. Customarily, only bound stationary states, which generally are at most denumerably infinite in number, are spoken of as excited, although the formal quantum theory often treats the noncountable unbound stationary states on an equal footing with the bound states
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Mn(+3) has the electronic configuration of 1s(2) 2s(2) 2p(6) 3s(2) 3o(6) 3d(2)\n\nthe one before me missed the 4s2 so his is wrong
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First the electron would have an sp1 configuration not np1.  As to which orbital it would revolve in...it doesn't matter.  The x, y, and z are just ways to distinquish the 3 different orbitals.  the point in the center is a null point.  the electrons do not actually travel through that spot.  Orbital configurations just define a volume where an electron might spend some of its time.  it could be found anywhere in the volume.