what is the preferred state of an electron in an atom? why?
111879
The question seems ambiguous but I'll give my take.  \n\nNature prefers lower energy states.  If you ever end up studying equilbrium and solution chemistry you will find that the product with lower energy electrons tends to be favored in a reaction.  So on that same note the preferred energy state of an electron is the lowest possible, this is because electrons in lower energy states are less likely to leave the atom, making the atom stable.  For example, the noble gases are the ultimate stable atoms because their valence octets are filled making them inert.  Further, electrons in molecular bonds are much more stable when they are in bonds resulting in the lowest energy, making them less reactive and more likely to stay in that bond.
12647
What might cause some confusion is that the electron resides in an "electron shell", and some theorize that the electron can be at any position in that shell at any time.\nMost do consider the electron a particle, but it depends on how you define the behavior.
850007
The electron configuration of Sc3+ is [Ne] 3s2 3p6\nThe value of "n" is the energy level, which is 3 here.\nThe value of "l" is the orbital type. For a "p" orbital, l = 1. \nSo, the statement is true.\n\nChromium has an unusual electron configuration.\nIt is actually 1s2 2s2 2p6 3s2 3p6 4s1 3d5.\nIt seems that the atom is more stable when it has all of the orbitals in a group filled the same way, ie. half-full.\n\nGround state means that the electrons are in the lowest energy levels available. In an excited state, energy has been added to the atom, and the electrons are (temporarily) at higher levels. Which ones depends on how much energy you put into the atom.  Too much, and you remove the electron entirely.\nSo, it's not really predictable without the energy values.
566511
Electrons, which are a Fermion particles, obey the Pauli Exclusion Principle. This means in a system there can never be 2 identical fermions (in this case no 2 electrons in an atom) that occupy the same quantum state. This is different to Bosons (photons for example) where any number of bosons can occupy the same quantum state.\n\nIn a bit more depth:\nThe Pauli exclusion principle plays a profound role in a huge number of physical phenomena. One of the most important, it results in "rigidness" or "stiffness" of fermions as contrast to bosons - impossibility to squeeze identical fermions into each other - thus in "rigidness" of ordinary matter (Young and bulk moduli of solids are direct consequences of Pauli principle). Another consequence is the elaborate electron shell structure of atoms and of the way atoms share electron(s) - thus variety of chemical elements and of their combinations (chemistry). (An electrically neutral atom contains bound electrons equal in number to the protons in the nucleus. Since electrons are fermions, the Pauli exclusion principle forbids them from occupying the same quantum state, so electrons have to "pile on top of each other" in atom).\n\nFor example, consider a neutral helium atom, which has two bound electrons. Both of these electrons can occupy the lowest-energy (1s) states by acquiring opposite spin. This does not violate the Pauli principle because spin is part of the quantum state of the electron, so the two electrons are occupying different quantum states. However, the spin can take only two different values (or eigenvalues). In a lithium atom, which contains three bound electrons, the third electron cannot fit into a 1s state, and has to occupy one of the higher-energy 2s states instead. Similarly, successive elements produce successively higher-energy shells. The chemical properties of an element largely depend on the number of electrons in the outermost shell, which gives rise to the periodic table of the elements.\n\nAstronomy provides another spectacular demonstrations of this effect, in the form of white dwarf stars and neutron stars. In both types of objects, the usual atomic structures are disrupted by large gravitational forces, leaving the constituents supported only by a "degeneracy pressure" produced by the Pauli exclusion principle. This exotic form of matter is known as degenerate matter. In white dwarfs, the atoms are held apart by the degeneracy pressure of the electrons. In neutron stars, which exhibit even larger gravitational forces, the electrons have merged with the protons to form neutrons, which produce a larger degeneracy pressure. Neutrons are the most "rigid" objects known - their Young modulus (or more accurate, bulk modulus) is 20 orders of magnitude larger than that of diamond.\n\nAnother physical phenomenon for which the Pauli principle is responsible is ferromagnetism, in which the exclusion effect results in exchange energy that induces neighboring electron spins to align (whereas classically they would anti-align).
961493
You need to know more than just the electron configuration.  There is contraction from left to right on the periodic table, plus additional periodic trends that must be considered.   \n\nEven more importantly, you need to define whether you are looking for the largest element IN ITS NATURAL  STATE (i.e. Cl2, Hg metal, etc) or AS THE ION.   Atomic and ionic radii differ.\n\nMore clarity is needed here.
905298
when electrons get energy or heat, they use that energy to move from their ground state to their excited state.  \n\nthey release the energy in the form of a color when they return to their ground state.\n\nthe amount of energy the electron absorbs (and then releases) determines the color.  purple has the most energy, and red has the least.\n\ni hope this was helpful!
792772
it's basically a system to put electrons in an atom and although they are arbitrarily placed, the place where they are more likely to be is called atomic orbital. there are several of these. \nthe first, called s orbital, will only acommodate 2 electrons, the second, called p orbital, 8 electrons and so on. read more on the source link
263276
You mean the electron configuration?\n\n1s2\n2s2 2p6\n3s2 3p4
1114892
Most likely lost from both S and P subshells but two electrons parked in a D or F subshell associated with one main quantum number lower. Ions want to achieve a noble gas configuration, which means no or all electrons of the same main quantum number S and P orbitals filled.
1067423
The change of energy  between energy levels.\n\nEnergy of electron in it's higher state  - energy of electron in it's lower state = h*f\n\nI forgot how to calculate the electron's energy at a specific energy state, but it should be easy to find.
343761
This is a homework question & better not be one of my students! LOL\n\nThe answer is atom.\n\nClassic textbook question. For those of you who thought the question was confusing, take it up w/ the authors of high school textbooks. I will gladly back you up on it. LOL\n\n:)
785300
Electrons have a negative charge and are held in the atom by the positively charged nucleus.  The further away from the nucleus that the electrons are, the easier it is to remove the electron.
476212
Atoms want to be like a "noble gas" with a filled outer shell.  I think it has to do with being in a stable state.  For Mg, it's a lot easier to drop 2 electons to look like Ne rather than gain 6 to look like Argon.\n\nThis very basic premise only works for things on the "sides" of the table.  The transition elements in the middle are a bit different.
445231
It describes electron location in terms of probabilities.  The energy levels around a nucleus are not well-defined orbitals.  Rather, they are regions of space where an electron may be found.  Withing the orbitals, the electron's precise location can not be known.  According to Heisenberg's Uncertainty Principle, the more accurately we measure an electron's location, the more imprecise the measurement of its velocity becomes, and vice-versa.\n\nSo, the best description of an electron's location is that of an "electron cloud", which represents the region in space where an electron has the highest probability of being.
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.
570126
It all comes down to two forces: the attraction between electrons and the nucleaus and the repulsion between the individual electrons.  This leads to a complex set of equations that do not have a solution. \n\nIf we assume that molecules behave as a combination of atomic states of only one electron, then we can try to formulate solutions of the equations (because the electron-electron repulsion term is zero). \n\nUnfortunately, the equations do not have a single answer. They have multiple answers. These answers have been called electronic configurations and are your different shells, sub-shells, etc. The actual quantum numbers are seen in the equations as solutions to the Schroedinger equation(HY=EY): n, l, ml, and ms.\n\nThe prevailing intepretation are that these states are energy levels which can be occupied by electrons as the form molecular bonds. \n\nMy university professor would probably remove my liver for such a poor description of the phenomenon, but this was always my best understanding of it.
45899
Start thinking of electrons in an atom as probability clouds...or regions of space around the atom at a given radius where the probability is high that the electron will exist.  Bohr theory ("orbits") is not complete, in fact it's not an accurate depiction of the electrons in an atom.\n\nThe reason the electron's don't radiate while "orbiting" is that they don't "orbit" anything!!  Instead, there are regions of space around the atom where the probability of an electron existing at any instant is non-zero.  Excited electrons may lose energy and drop to a lower energy level (to a smaller radius from the atom), in which case the electron will radiate energy in the form of a photon whose energy is equal to the difference in energy levels (excited state - lower state).  \n\nAs a concrete example, this radiation from dropping to lower energy states is the basis of lasing action and the principle on which lasers operate.\n\nAs I said, think in terms of the quantum mechanical description of the electron rather than the Bohr theory.  It's not over your head, believe me, just study quantum mechanics.  Start with the electron in a Hydrogen atom, it's the simplest case (a 1 electron atom!!)\n\nI hope this helps.