an excited state and a ground state of an atom....?
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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
1117389
in the protons: positive charge in the nucleus, and the electrons (negatively charged) orbiting around the nucleus
446643
The movement of an electron from one place to another.
30961
Since the spectra of a given element shows a discrete number of color bands (rather than a continuous specturm), and since the color of light relates to its energy, and since photons are released by the relaxation of electrons from a higher to a lower energy state, it follows that the gaps between energy levels are distinct and finite.  This means that the energy levels are quantized.
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See if this helps.\n\nhttp://hyperphysics.phy-astr.gsu.edu/hbase/atomic/hund.html
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atomic number represents the number of protons or electrons in an atom
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You mean the electron configuration?\n\n1s2\n2s2 2p6\n3s2 3p4
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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
30976
to explain how two electrons can be near each other
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alright. Electron configurations. I had the exact same problem three weeks ago. I was SO confused. But i got it in the end.\n\nLet me explain.\nThere are two types of electron configurations. One is the simple electron shell configuration. Let's say 2-8-16 and the other is called spdf notation like 1s2 2s2(i can' t type the two after the s like an exponent so bear with me)\n\nNow the first one is simple. Shell notation. An atoms outer shells are divided into shells that each have a maximum limit for the number of electrons that they can contain. the first can hold 2, the second 8 and so on. They all follow a rule. It is always 2 time the shell number squared. lets say level 1. Square it. You get 1. Multiply it by 2. You get 2. Therefore 2 is the maximum # that level one can hold. You said 15. So fill each level so that each contains the max. It would be 2-8-5. (The last one is five so that the all ad up to 15). Got it?\n\nNext, we have spdf notation. This takes a lot of time to explain so i'll just give you a site to go to. \n\nhttp://www.fordhamprep.org/gcurran/sho/sho/lessons/lesson36.htm\n\nGood luck!
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Four.\n\nThe first one is usually called "n" and it gives what people think of when they say "energy level".  It's also called the "principal quantum number", I think.\n\nThe next one is usually called "l" (el) and for a given energy level, it can be anything from 0 up to "n-1".  These correspond to what people sometimes call "shells", such as the s, p, d, f, etc. shell.\n\nThe next one is called "m" and is sometimes called the "sub-shell".  Each shell can have up to "2*l+1" sub-shells.  So an "s shell" (l=0) can have 1 sub-shell.  A "p shell" (l=1) can have 2*1+1=3 sub-shells, etc.\n\nThe final quantum number is called "s" or "spin".  For each sub-shell, this can take on one of two values, +1/2 or -1/2  in some books.  This means that only two electrons are allowed in any given sub-shell.\n\nSo for n=1, the only option is l = 0, which means further that m must be 1, with 2 choices for s.  This all means that the first energy level can only hold 2 electrons.\n\nFor n=2, l can be either 0 or 1.  For l =0, m must again be 1, allowing 2 electrons.  For l = 1, m can be as much as 3, each allowed to have 2 electrons.  So adding the 2 electrons for the l=0 subshell to the 6 allowed in the 3 possible subshells for l=1 (6 electrons we get a total of 8 electrons allowed in the second energy level.\n\nYou can continue on to get totals of 18 (2 + 6 + 10) for the 3rd energy level (n=3; l =0, 1, or 2;  and m = 1, 3 and 5, each with 2 electrons allowed).\n\nThis is where the numbers that correspond to "filled energy levels" come from in the periodic table.
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proton and neutron, the electrons are on the outer shell
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it does not have to end with the s, and in the case of calcium, which has 20 electrons, the ground state would have the configuration ending in 3d2, because it is the lower energy state, see the link it is pretty cool\n\nhttp://www.webelements.com/webelements/elements/text/Ca/econ.html
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Protons and neutrons.
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Whatever its atomic number is, would be the number of electrons. If it's an ion, then add for every negative value and subtract for every positive one.
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energy levels/orbitals
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positive or negative charge\n\nif it has an equal number of protons and electrons, it is neutral\n\nif it has an unequal number of protons and electrons, it has a charge and is an ion