Do you know about electron shells?
535236
a) 1\n2) depends on if the outer shell is full or not. If it's full, they probably bounce off of each other, if not full, they can create a bond with each other.\n3) stable, noble\n4) becasue it has an electrical charge since the protons (positive) and electrons (negative) are unequal.
839048
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.
198620
My Chemistry teacher taught me a great story which helped me learn the elements, which groups they were in, which periods, how many electrons they had etc and resulted in me going from a grade F to B. Every kid should learn this.\n\nHorrible Heary Little Begger Boys Catch Newts On Friday Near Naples, Magnificent Albert Sits Planning Some Clever Arrangement Keeping Calm.\n\nOk, looks crazy until you break it down;\n\nH He Li Be B C N O F Ne Na, Mg Al Si P S CL Ar K Ca\n\nThen put it into the table\n\nH\n                   He\nLi Be  B C  N O F  Ne\nNa Mg Al Si P S Cl Ar \nK  Ca\n\nYou will need to line them up because Yahoo has left align, but the trick is the story. Hope this helps
1008396
positively charged protons (in the nucleus), neutrally charged neutrons (also in the nucleus) and negatively charged electrons (which circle around the nucleus) ....also they have "discovered" other matter in the atom called quarks and a couple other similarly named items....but it is generally accepted that protons, neutrons, and electrons make up an atom....
1139864
electrons were discovered by  william crooks by discharge tube experiment and named it electron by stoney and cathode rays by julius plucker .protons were discovered by  goldstein\n again by discharge experiment by placing the perforated cathode in the middle of discharge tube.\nproperties of electron:-\n1. made up of material particles\n2. carrying negative charge\n3. affect photographic plate\n4. follow the straight path\n5. e/m ratio is constant\nproperties of protons:-\n1.carry positive charge\n2. specific charge(9.58*10000c/gm)\n3. proton upon mass ratio is not constant
949019
The number of electrons in any shell/orbit is 2n^2 (2 )(n square), where "n" is the number of the orbit.\nSo in the second in the second shell, it is 2(2)(2)= 8 electrons.\n2 electrons in the "s" orbital, and 6 in the "p" orbital
680011
no one really knows yet.\n\nalthough, at one point, people thought atoms were the smallest particles, now we know about protons, neutrons, and electrons (and now there's a theory that they're made out of something called quarks, but no one really knows what they are)... it's only a matter of time until we find out what they're all made of... and what those things are made of... and what those things are made of... and so on (I seriously doubt it ever ends... like the universe)
735095
it is electron.\nit is the only one to circle the nucleus.\nwhen an electron moves with very high speed, its relativistic mass is more than its rest mass.
30976
to explain how two electrons can be near each other
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.
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.
981192
http://periodic.lanl.gov/default.htm\n\nClick on the element, and it's in the top section of information. To write out the electron configuration for every element would take quite a while, so if you need it for a specific element or a few elements, I'd reccomend asking just for the few.
924334
Well, in terms of classical physics, an electron orbits the nucleus due to the electrical force.  But the theory of electromagnetism tells us that accelerating charged particles lose energy, and anything which is orbiting something is accelerating.  So, put these two facts together and the electron should lose energy and spiral into the nucleus.  This obviously doesn't happen (if it did, there would be no atoms...), so this was a serious problem for physics in the first decade or so of the 20th century.\n\nThe semi-classical explanation, created by a physicist named Bohr to solve the problems with the classical explanation, proposed that electrons could only be in orbits where the quantity called angular momentum (which is numerically the momentum of a particle times the radius of its orbit, or formulaicly pr=mvr=m(r^2)w where w is the angular velocity [think of it as the frequency of the orbit]) was some integer number times a constant (called h-bar).  This theory prevented the electron from falling into the nucleus of an atom, and it explained the Hydrogen atom perfectly.  But it didn't work for any other kind of atom.\n\nFinally, there's the quantum explanation, which emerged about ten/fifteen years or so after Bohr did his work.  In quantum theory particles are represented by probability distributions called wavefunctions (which is, depending on how you approach it, either a result of or the reason for Heisenburg's Uncertainty Principle; also, I'm playing a bit fast and loose with my terminology:  a wavefunction isn't a probability distribution, but if you basically square the wavefunction, that's the probability distribution).  Now, if you work out the wavefunction of an electron around a nucleus, it turns out to be constant in time, which means that it doesn't fall into the nucleus (or fly off into space or whatever else;  it stays around the nucleus as desribed by the wavefunction).  Of course, one thing which is interesting to note is that in many situations (incluing the simplest) the signle point (though not the radius) where the probability of finding the electron is the highest is actually in the nucleus.  :)  But if you found the electron there at one moment the next moment you could easily find it outside the nucleus.  It's random (as far as we know).\n\nNow, if this last confuses you or seems weird, well, it *is* quantum mechanics, and quantum mechanics is renowned for being very weird and confusing.  As to why you can never just find the electron always sitting in the nucleus of an atom, it basically has to do with the Uncertainty Principle.  If you knew that the electron definitely had to be in the same place as the nucleus at any given point of time, you couldn't know how fast it was moving very well at all, so a moment later the electron could be very far away from the nucleus (but not separated from it, as the electrical attraction would still be there and would keep the electron from escaping the nucleus altogether).\n\nI hope I've shed some light on this subject for you.
215864
Protons and neutrons certainly do have a shape, in the same way that an electron in orbit around a nucleus has a shape (it's a probability cloud).\n\nI'm not aware of any measurements of proton/neutron shapes.  There are experiments that measure the shape of nuclei (groups of protons and neutrons).  Nuclei are generally spherical, but they are known to have squashed shapes due to angular momentum (some are extremely non-spherical).  Protons/neutrons are probably very close to spherical as well, but proabably slightly squashed too because they do have angular momentum (spin).
60596
Gaining an electron...
375982
it is coz of the one valance electron in the outer most shell
13297
Atoms have a nucleus ( composed of protons and neutrons) and a cloud of electrons. The number of the different components varies between different elements.\n\nElectrons can only have specific energy levels in an atom - that is the energy is not continious but quantized. This is different from, say, the solar system, because a planet could theoretically be in any orbit. But we know from quantum mechanics (and many, many experiments) that electons can only occupy certain "orbits."\n\nSometimes an electron can be bumped into a higher orbit (the higher orbits have less energy, because they are not as tightly bound) or kicked out of the atom altogether. If a second electron moves into the spot it will release energy as it falls into that level.\n\nHydrogen is the easiest element to study. The nucleus is a single proton, and it can have only one electron. The different energy levels can be illustrated like this:\nhttp://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html#c2\n(though in reality electrons don't travel on nice orbits)\n\nIf an electron in the second lowest level does a "quantum leap" to the very lowest, it will emit energy - light - at a very specific frequency. In this case 656 nanometers, which is red. If, on the other hand, an electron falls from the 3rd level down to the 1st level the emitted light is blue.\n\nA "spectrum" will show all of these distinct levels, with the brighter ones being the most common. This shows the spectrum of hydrogen with a diagram of the quantum leaps:\nhttp://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html#c4\n\nIn other atoms it becomes more complex, not every jump is allowed, and in the precense of a magnetic field a "fine structure" is seen in the spectrum, as some of the main lines look double.\n\nThe result of all of this is that each different atom will give a different characteristic spectrum. So, you can use this to identify different elements in anything from crime scene samples to distant galaxies.