electron configuration and periodicity?
828272
You will find all the answers here:\n\nhttp://library.thinkquest.org/10429/high/eleconfig/electron.htm
193226
All atoms do this. The Noble gasses have the most stable electron configurations because they fill/do not have "open shells".\n\nFor example, Calcium's nearest noble gas is behind it, so it will LOOSE two electrons, since losing two is easier than gaining 6 to act like the next noble gas ahead of it, that's why you see Calcium as a 2+ ion. (Ca2+). Iodine, on the other hand needs to gain one electron (instead of losing 7) to be like it's nearest noble gas, so you get the ion of I-. For a metal like silver, it just has one "valance" electron, so you'll see silver as Ag+. Copper has two extra : Cu2+, Iron typically has 3 valance electrons so it make Fe3+
8019
Name: niobium \nSymbol: Nb \nAtomic number: 41 \nAtomic weight: 92.90638\n\nGround state electron configuration: [Kr]4d4 5s1 \nShell structure: 2.8.18.12.1\n\nThe Noble Gas Configuration is the preferred configuration for the arrangement of electrons on all atoms.  All atoms will strive to create an electronic configuration that simular to that of a Noble Gas by gaining or losing electrons.\n\nPlease note that this does not mean that it is a Noble gas configuration but rather an electron configuration.
223202
goto http://www.webelements.com/ or better stillhttp://www.schoolscience.co.uk/periodictable.html run over the element with your mouse it tells you what it is
892647
The electron configuration of Oxygen is:\n1s2\n2s2\n2p4\n\nThe valence orbital (2) has 6 electrons (2 from the 2s and 4 from the 2p).  Thus oxygen has six valence electrons.
946929
all the electrons are located in the electronic orbitals of the ion.\n\nYou may find this useful:\n\nhttp://www.owlnet.rice.edu/~chem251/documents/Vollhardt_1.ppt
697038
This is kinda hard to draw on here...\n......_\nK--Br|\n......_\n\nThe lines around Br represent 2 electrons, and the -- represents a bond...ignore the periods
72228
http://www.webelements.com/webelements/elements/text/H/key.html\nhttp://periodic.lanl.gov/elements/1.html\nhttp://www.chemicalelements.com/elements/h.html\nhttp://education.jlab.org/itselemental/ele001.html
825026
what you need to do, get a SI data book, and look up their natural state. not bonded with anything else, and possibly itself.\n\nPhophorus - white: molecular (P4). red: Chain. Black: Layer\nIodine - molecular (I2)\nMagnesium - hexagonal closest-packing\nNeon - cubic closest-packing\nArsenic -grey: 3d structure - Layer formation. yellow: molecular As4\nSulfur- molecular S8\nBoron - complicated structure.\nSelenium - grey: chain, Red: molecular: Se8\nGallium - Complicated\nCesium - body-centred cubic\nOxxygen - O2, O3 molecular
332147
Those ions do follow Hund's rule, though. The d orbital looks like this:\n\n\n_________ ___________\n\n__**_______ ____*____ ___*____\n\nThe electrons are only paired when absolutely necessary.
766178
The electron configuration of Si is:\n\n[Ne] 3s2 3p2\n\nSi2+ is Si with 2 less electrons so the electron configuration is:\n\n[Ne] 3s2\n\nThe 2 electrons are taken from the p orbital as it requires less energy to remove 2 electrons.
964369
Huge order. Let's see how far it can be served.\n\n1. Monoatomic negative ions: take the element name (sometimes shortened) and add "-ide" (as in hydride, nitride, oxide, sulphide, phosphide, chloride...)\nPositive ions: element-name, charge (if several charges are possible), ion (sodium ion, iron II ion...)\n\n2. Polyatomic ions:\nComplexes with various ligands list the ligands and the central ion/atom.\nOxygen as ligands has its own nomenclature, depending on oxidation state. E.g. Sulphate, sulphite, perchlorate, chlorate, chlorite, hypochlorite...\n\n3. Binary molecular compounds: Halogen, oxygen and sulphur compounds usually have the correspondent "-ide" as if you had ionic compounds. Usually the more electropositive element is used as center.\n\n4. Acids: Oxygen acids have a similar nomenclature to oxygen ions.
1069221
Electron configuration is related to the number of protons in the nucleus, hence, the element. In theory, all isotopes of a certain element should have the same electron configuration.\n\nWhat u were asking for is an electron configuration for oxygen anion, it has the same electron configuration as Neon\n\nelectron configuartion of O^2- = [Ne] (Neon core) = 1s^2 2s^2 2p^6
1164545
It's easy. I'de do it for you, but I'm about to leave work.\n\nIf you know the order of electron configuration, and how many electrons go into each sublevel, all you have to do is know how many electrons you've got. Whatever atomic number it has, that's how many electrons the atom has. Use the electron configuration model to place all the electrons in their proper energy level, and if you have it right, you'll know how many valence electrons you have. \n\nIf your clueless, then I can't help you. Research electron configuration. You should be able to find a chart showing you the order. \n\nThe levels go all the way up to 7, and within each one, is a sublevel, s, p, d, and f. s has 2 electrons, p has 6, d has 10, and f has 14. Helium for example has two electrons. \n\nHe = 1s^2\n\nHelium has only one level, and two valence electrons. \n\nOxygen = 1s^2, 2s^2, 2p^4\n\nOxygen has 6 valence because on the two outermost levels, there are 6 electrons, and also you see the ground state.
613790
Maybe this wil lhelp.         \n\n ELECTRON DOT DIAGRAMS\n1. Let the element's SYMBOL represent the nucleus and inner energy level .\n2. Write the ELECTRON CONFIGURATION for the element (or look at the PERIODIC table).  Count the electrons in the OUTER energy level.\n3. Let the top, bottom, and two sides represent the ORBITALS.\nPlace the appropriate number of DOTS in each "orbital".\nUse ONE dot if the orbital has 1 electron and TWO dots if the orbital has 2 electrons.  The electron dot diagrams for:\n \nNa(Z=11)  1s2   2s2   2p6  3s1       Na\n \nMg(Z=12)  1s2   2s2   2p6  3s2             Mg\n \nAs(Z=33)  1s2   2s2   2p6  3s2  3p6  4s2  3d10  4p3      As\n \nThe periodic table can also be used to write electron dot diagrams.\nAll the elements in the first column have ONE outer electron(s).  They have ONE dot(s) in their electron dot diagram. All of the elements in column 2 have TWO outer electrons.  They have TWO dots in their electron dot diagram.  Most of the elements in column 18 have EIGHT outer electrons except HELIUM which only has TWO outer electrons.  All of the elements in column 18 have EIGHT dots in their electron dot diagram except HELIUM  which only has TWO.
977750
Mn(+3) has the electronic configuration of 1s(2) 2s(2) 2p(6) 3s(2) 3o(6) 3d(2)\n\nthe one before me missed the 4s2 so his is wrong
747161
Answer:  SIX electrons\n\nI drew a diagram for you: http://server6.theimagehosting.com/image.php?img=untitled.34c.JPG\n\nElectron Configuration of Fe: 1s2 2s2 2p6 3s2 3p6 4s2 3d6 \n\nExplanation:  As you can see in the electron configuration above, there are 6 electrons in 3d orbitals of Fe in its ground state.