Which orbitial is considered the ground state for the electron in hydrogen?
354063
yes, it's the 1s orbital. The electron configuration of hydrogen is 1s1.  The electron configuration of helium is 1s2.
779218
Here's a great and simple explaination from Wikiopedia: \n\nIn atomic physics and quantum chemistry, the electron configuration is the arrangement of electrons in an atom, molecule, or other physical structure (eg, a crystal).\n\nLike other elementary particles, the electron is subject to the laws of quantum mechanics, and exhibits both particle-like and wave-like properties. Formally, the quantum state of a particular electron is defined by its wavefunction, a complex-valued function of space and time. According to the Copenhagen interpretation of quantum mechanics, a particular electron is both "nowhere at all" and "everywhere all at once" until an act of measurement causes it to be detected. The probability that the act of measurement will detect the electron at a particular point in space is proportional to the square of the absolute value of the wavefunction at that point.\n\nElectrons are able to jump from one energy level to another by emission or absorption of a quantum of energy, in the form of a photon. Because of the Pauli exclusion principle, no more than two electrons may exist in a given atomic orbital; therefore an electron may only leap to another orbital if there is a vacancy there.\n\nKnowledge of the electron configuration of different atoms helps us understand the structure of the periodic table of elements. The concept is also useful for describing the chemical bonds that hold molecules together. And in a macro sense this same idea helps explain the peculiar properties of lasers and semiconductors\n\n\nThe other links are also good sources for review and expaination\n\nGood luck
576205
Electrons are in orbitals of a set quantum energy levels. There are normally empty orbitals above the filled orbitals. When an electron is excited to a higher energy level it does not want to stay there it want back to the lowest energy level, or at least a lower energy level. When it drops into the various possible energy levels it releases light at various frequencies equal to the energy of the electrons drop plus or minus any coupling. Hydrogen spectrum is the various frequencies of light that can be emitted by this process from hydrogen. It is solvable using Schrodinger's Equation.
226718
Anywhere is the best answer.  But, let's look at why.  Orbitals tell us where the electron is most likely to be found, but there is no actual guarantee that it will be there, so it could be anywhere.
463572
The reality of the situation is the electron doesn't orbit around the nucleus like the earth orbits around the sun.  \n\nThe electron is in what is called the "electron cloud."  You can only say that the electron is at a certain place with a certain probability: not certainty.  \n\nTherefore, there is no way to visualize how the electron moves about the nucleus.
1010723
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.
784377
This is true.  The Px, Py, and Pz orbitals are degenerate in all atoms provided the atom is not subjected to a magnetic field. \n\nIn hydrogen and other single electron systems (He+ etc) only the n quantum number matters to determine energy.  So you can actually say that the 2s, 2px, 2py and 2pz are all degenerate.  \n\nThe s, p etc orbitals lose this degeneracy when there is more than one electron due to electrostatic repulsion between the electrons, so then you need both the n quantum number and the l quantum number to determine energy.
390703
In the Bohr model of the atom, it was thought that electrons orbit the nucleus in the same way that the planets orbit the sun. However, the situation was found to be much more complicated than the simple planetary orbits. There are different levels of orbitals and energy levels. Also, the position of an electron can never truly be defined because of the uncertainty principle and the electrons have to be thought of as a "cloud" where any electrons could possibly be at a given moment. So, the internal structure of atoms is much more complicated than the planetary orbits.
263276
You mean the electron configuration?\n\n1s2\n2s2 2p6\n3s2 3p4
1132990
with the help of atomic number & electronic configuration. the electronic configuration of the outermost orbit gives you no. of valance electrons
642453
proton and neutron, the electrons are on the outer shell
894776
According to quantum mechinics, an electron is not confined to an orbit as we know for satellites, it has a 'shell' of probability where it is most likely to be found. It also has the small but finite chance of being found inside the nucleus of the atom, so the anwer is 0.
1107546
1. There are two molecular orbitals for hydrogen, the lower energy orbital has its greater electron density between the two nuclei. This is the bonding molecular orbital - and is of lower energy than the two 1s atomic orbitals of hydrogen atoms making this orbital more stable than two seperated atomic hydrogen orbitals. The upper molecular orbital has a node in the electronic wave function and the electron density is low between the two positively charged nuclei. The energy of the upper orbital is greater than that of the 1s atomic orbital, and such an orbital is called an antibonding molecular orbital.\nNormally, the two electrons in hydrogen occupy the bonding molecular orbital, with anti-parallel spins. If molecular hydrogen is irradiated by ultra-violet (UV) light, the molecule may absorb the energy, and promote one electron into its antibonding orbital (s*), and the atoms will seperate. The energy levels in a hydrogen molecule can be represented in a diagram - showing how the two 1s atomic orbitals combine to form two molecular orbitals, one bonding (s) and one antibonding (s*). This is shown below - by clicking upon either the s or s* molecular orbital in the diagram - it will show graphically in a window to the right.\n\n2.Hybridisation\nThe Valence Bond model suggests that for a covalent bond to form, two atomic orbitals must overlap sufficiently so that electrons can be shared. However, if the hydrogen atoms are positioned tetrahedrally, not all of them will overlap with orbitals on the carbon atom. This is because the carbon's p orbitals are positioned octahedrally, whereas the hydrogen atoms are orientated tetrahedrally. How does the VSEPR model account for this problem? By inventing hybrid orbitals (N.B. these were proposed by Linus Pauling). In the carbon atom, the 2s and 2p orbitals have different energies. If the 2s orbital combines with the three 2p orbitals, four new sp3 hybrid orbitals will be formed. These new hybrid orbitals are identical - they are arranged tetrahedrally and have the same energy (they are degenerate). The 1s orbitals from the hydrogen atoms can now overlap with the sp3 hybrid orbitals, forming single covalent bonds.\n\nImportant: insert a picture of formation of hybrid orbitals (energy levels)\n\nGeometries of Hybrid Orbitals\n\nsp\n sp2\n sp3\n sp3d\n sp3d2\n \n[edit]\nLone Electron Pairs\nThe VSEPR model treats lone electron pairs in a similar way to bonding electrons. In ammonia (NH3) for example, there are three hydrogen atoms and one lone pair of electrons surrounding the central nitrogen atom. Because there are four groups, ammonia has a tetrahedral shape but unlike methane, the angle between the hydrogen atoms is slightly smaller, 107.3°. This can be explained by theorising that lone electron pairs take up more space physically than bonding pairs. This is a reasonable theory: in a bond, the electron pair is distributed over two atoms whereas a lone pair is only located on one. Because it is bigger, the lone pair forces the other electron pairs together.\n\nTesting this assumption with water provides further evidence. In water (H2O) there are two hydrogen atoms and two lone pairs, again making four groups in total. The electron pairs repel eachother into a tetrahedral shape. The angle between the hydrogen atoms is 104.5°, which is what we expect from our model. The two lone pairs both push the bonds closer together, giving a smaller angle than in ammonia. The scientific method has succeeded again!
923442
At the outermost limits of the ionosphere which extends some one thousand kilometres above the surface of the earth individual atoms are held in position by the gravitational effect of binary electrons with frequencies of or above 150 hertz (that is with small particle orbit diameters of 2000 kilometres or more) held captive by atoms at the surface of the earth.\n\nThe orbit of the small particle of a binary electron with a frequency of 0.3Hz at the earth’s surface is large enough to encompass the moon. The combined attractive force of incalculable numbers of very low frequency binary electrons at the earth’s surface (acting in unison with very low frequency binary electrons at the surfaces of the sun and moon) exert sufficient force to hold the moon in orbit.\n\nThe sun, which is 330,000 times more massive than the earth, exerts enormous gravitational force. The orbit of the small particle of a binary electron with a frequency of 0.001Hz at the surface of the sun will encompass the earth. Colossal numbers of binary electrons within the suns mass exert sufficient influence to hold the earth in orbit.\n\n (Those who take an interest in calculation will notice that the moon is approximately one eightieth of the mass of the earth and therefore too massive to be held in orbit by the earth acting alone. It should be remembered that the moon like the earth is held in solar orbit. The gravitational influence of the earth serves only to modify the shape of the lunar orbit from a simple independent solar orbit to the more complex shape of a planetary satellite).\n\nBinary electrons with frequencies as low as 0.000025Hz at the surface of the sun have just enough influence to hold the remote planet Pluto in orbit. At some point beyond the orbit of Pluto (which has an average orbit of 5.8 billion kilometres from the sun) the small particles of binary electrons, whose large particle remains at the surface of the sun, have insufficient influence to hold matter within the solar system. \n\nIt has already been noted (see Atoms above) that the combined mass of all the planets in the solar system is closely related to the total mass of electrons within the body of the sun. From this it can be inferred that it requires some 1800 binary electrons within the body of the sun to hold one atom in orbit. This appears to be the factor which determines the quantity of matter which can be held in solar orbit. The total mass of matter which can be held in solar orbit cannot exceed the total mass of electrons associated with atoms which form the body of the sun.
1001444
As an ion, oxygen is negative.  As a molecule, 02 is neutral.  \nAn an ion, hydrogen is positive.  As a moleclue, H2 is neutral.
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)
362329
Consider that one electron will repel another electron (-ve does not attract -ve), each bond between a carbon and hydrogen is cased by a pair of electrons (2 electrons) so you have a total of eight electrons... this results in neutralising the charge on all the atoms.\n\nCarbon has 2s1, 2s2, 2p2 electrons which means it is theoretically 4 electrons short of its closest nobel gas (nobel gases are neutral).\nHydrogen has 1s1 electrons which means it is theoretically 1 electron short. Note that there is no p orbital in first row of periodic table.\n\nAs such each hydrogen shares its sole electron with the carbon, donating a total of 4 electrons, hence 4 hydrogens.\nThe Hydrogens get their electrons from the carbon, the carbon has 2s2 and 2p2 electrons, totalling 4 to share, 1 to each hydrogen... we do not count the s1 orbital because it is unlikely to operate in forming bonding.\n\nNow each pair repels eachother so they are furthest apart, if we do the mathematics...\nblah blah...\nWe end up with an optimum angle of 107.5 degrees between eah hydrogen, any more than that and a different hydrogen will repel it back, and likewise if less. this forms a 'tetrahedral' shape.\n\nIf you were to switch a hydrogen with another element... say chlorine, to produce CH3Cl (Chloro-methane) then the hydrogens (being the smaller atoms with less electrons) will be pushed further from the chlorine which will tend to determine the molecule's appearance. Ch3Cl is not a perfect tetrahedral as its angles will not equal 107.5, but we still call it that for simplicity's sake.\n\nI recommend that for further information do a search on the following phrases:\n\nVSEPR\nValence Shell Electron Pair Repulsion theory\nMolecular geometry\nMethane\nOrganic Chemistry