which orbitals are excited states in he hydrogen atom?
352211
Any orbital other than the 1s  orbital is excited if populated.  2s, 2p, 3s,3p, 3d....
62040
Two.  "Normal helium has 2 protons and 2 neutrons in its nucleus, giving it an atomic weight of 4."
443303
It only has 7 valence electrons :)\n\nRival
29638
The internal structure of an atom (in terms of its protons and neutrons) will create regions which are called orbitals.  We commonly think of atoms according to the Bohr model, where electrons orbit the nucleus like little planets.  This model is wrong.  the truth is that we can only determine the location of an electron based on a statistical model, and that gives us regions where electrons are more likely or less likely to be found if we searched for them there.  These areas where electrons are most likely to be found are called orbitals.\n\nThe orbitals differ in energy states.  An electron in a high orbital needs high energy, and electrons with less energy will be at lower orbitals.  When the number of electrons and protons are equal (ie the atom is not an ion) and the electrons occupy all of the lowest energy orbitals possible, that is called the ground state.\n\nif an electron at the ground state gets extra energy, it can jump to a higher orbital.  However, the various orbitals require certain, specific amounts of energy, and the energy gaps between the orbitals are specific amounts of energy, based on the orbital structure dictated by the nucleus (the details of all of this require some of the ugliest differential equations and eigenfunctions you're likely to ever see).  So the energy absorbed by an electron to jump from a low orbital to a high orbital must be of a specific amount.  After time, the electron will eventually relax back to the lower orbital.  When it does, it will release its excess energy in the form of a photon with the precise amount of energy that spearates the two orbitals.\n\nFor a given atom, there is a certain number of specific orbital transitions possible, and each possible transition will correspnd to a single band on the spectrum produced by the pure element when heated to.  So while a given atom can give several colors, the number of colors it can give are limited.
773257
Re:  For Helium, the "2" is called the atomic number and it means that Helium has 2, protons, 2 nuetrons and 2 electrons.\n\nFor Lawrencium (Lr) it should show 103 as its atomic number.  That means that Lr has 103 protons, 103 neutrons and 103 electrons.  \n\nThe 2, 8, 18, 32, 32, 8, 3 numbers are showing electrons per shell (different subject) but you'll see that if you added all the numbers 2+ 8+ 18+ 32+ 32+ 8+ 3 = 103.  103 is the total number of electrons Lr has.   \n\n____________________________________________\n\n\n\n\nFor a Normal Neutral Atom, the number of protons (p+), neutrons (n) and electrons (e-) are all the same. \n\nJust look up the atomic number from the periodic table to determine them.\n\nFor example:\n\nC: 6p, 6n, and 6e-.\nN: 7p, 7n, and 7e-.\nK: 19p, 19n, and 19e-.\n\nNow, Determine the number of p, n, and e- for Ca.\n\n\n\n\n\n\nIf you guessed, 20p, 20n, and 20e-, you are Correct!\n\n\nNote that, if you add the number of the atom's p and n you will get the Mass number (Z). \n\nThe periodic table shows Z of calcium as 40.078 because 20p + 20n = 40 (amu) \n\nAnother Example: Oxygen, having atomic number of 8, will have:\n8p, 8n, and 8e-. This means that Oxygen will have the mass number of 16 because; p + n = Mass number (Z).\n\n______________________________...\n\nFor Isotopes:\nIsotopes are atoms that have same number of protons but different number of neutrons.\n\nYou've already seen that normal Carbon has: 6p, 6n, and 6e-.\n\nThis normal carbon is called "Carbon-12". The "12" denotes its Mass number (Z). Which is p + n.\n\nThere are isotopes of Carbons and one of them are Carbon-13. Since you already know that Carbon must have 6p, Carbon-13 has 7n. 13 - 6 = 7. The number of the electrons are still the same as number of proton. \n\nIn another words, simply subtract the number of protons from mass number to determine the number of neutrons.\n\nNow, determine the number of p, n and e- of Fluorine-19:\n\n\n\n\n\nIf you guessed 9p, 10n, and 9e-, you are Correct!\n\n______________________________...\n\nFinally, there are ions. Ions means that an atom has either gained or lost electrons. Keep in mind that eletrons are NEGATIVE in nature (e-) and when an atom Gains e-, it becomes More negative.\n\nFor example: Fluoride ion, F- means that it has GAINED one electron compared to its neutral F state. Therefore;\n\nF has 9p, 9n, and 9e-, But F- has 9p, 9n, and TEN e-.\n\nO has 8p, 8n, and 8e-, But O2- has 8p, 8n and TEN e-, because O2- means that it has Gained 2 more electrons than its normal O state. \n\nNow, determine the p, n and e- for P3-.\n\n\n\n\n\nIf you guessed 15p, 15n, and 18e- you are Correct!\n\nFor atoms that have positive charges (cation), remember that they LOSE e- to become positive. So, Li+ has 3p, 3n and 2e-. \n______________________________...\n\nKeep in mind that you need to know how to combine all three of the ideas mentioned above. For example, you may be requested to determine the p, n and e- of Magnesium-25 ion. \nYou need to know that since Magnesium is in Group IIA, it will turn into 2+ ion. Therefore Magnesium-25 ion will have 12p, 13n, and 10e-. \n\nI hope this answers your question. Good luck!
132115
1\nThere are 2 Hydrogen atoms, 1 Sulfur atom (as idicated by the absence of any subscript) and 4 Oxygen atoms.
174685
Is this row-echelon form of diagonal? Dirac, Heisenberg matrix? Isn't -Psi just the unlikely probability of the electron function? Does Psi have anything to do with energy? Could you explain further.
979155
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!
831362
n = 1,2,.....\n l = 0, 1, 2..... n-1\nm = -l, -(l-1)\n\nThe labels  are called quantum numbers, and made their debut in Sommerfeld's elliptical orbit model. They correspond to certain classical features of the orbit: \n\nn= sr. root of (semi major axis)\nl = orbital angular momentum\nm = orientation of the orbit
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Selenium will have 6 valence electrons just like oxygen.  Place the Se as the central atom.  Two OH groups will single bond to the Se (remember H has only one valence electron).  One O will double bond to the Se. \n\nDraw it a couple times till you get it looking good, and you'll remember it. You can cheat and look at the last link below, and substitute Se for the S in the structure given.
178616
The orbital radius in H is about an anstrom 10^-10 M\nFor Dirac and some calculations it is a point source with a wave function and a propability of finding the particle.
70540
oxygen, nitrogen, hydrogen, methane, helium
76628
By "shells," do you mean the energy levels of the electron orbitals?  If that's what you mean, all you do is look on the period table and count how many rows from the top the element is.  So H and He each have one electron shell, C, N, O, F, etc. all have two, Si, B, Na, Cl, etc. all have three, and so on.  Sorry about the scattered examples (I was listing them by memory), but hopefully you get the idea.
136024
The electron of a hydrogen atom orbits around the hydrogen atom nucleus. If there was no electron it wouldn't be an atom of any kind. In other words, the electron is "inside" a hydrogen atom.\n\nThis website for graphics of the hydrogen atom and suggestions for a science project:\n\nhttp://education.jlab.org/qa/atom_model.html
132339
An atom has a nucleus and electrons orbiting around it. Not all possible orbits have electrons, though. The electrons arrange themselves in the lower energy orbits (those closer to the nucleus). When an electron is excited, it means it has absorbed enough energy to jump to a higher energy orbit (one further from the nucleus). When it comes back to its non-excited orbit (closer to the nucleus), it releases the extra energy by producing a photon --that is, the electron emits light. The color of the light will depend on how much energy it is releasing.\n\nAnd excited atom is one that has one or more excited electrons.
786500
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.
1128901
An electron/energy shell, is a group of atomic orbitals with the same value of the principal quantum number n. \nThus in a silicon atom (1s^2  2s^2 2p^6 3s^2 3p^2)  the number of energy shells with electrons in them is 3.\n\n(just for info: There are 5 occupied subshells (1s, 2s, 2p, 3s, 3p) and 8 occupied orbitals 1s 2s 2px 2py 2pz 3s 3px 3py, out of which the first 6 have 2 electrons and 3px and 3py have one electron each; Hund's rule doesn't allow an electron pair in 3px while the other 3p orbitals are empty)