What is the Lewis Dot Structure of Selenium?
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Selenium element is located in Group 6A of the periodic table. This in dicates that it has 6 electron in its valence or outermost shell. The Lewis dot structure of Selenium shoulde be written with Se surrounded by six dots. These six dots don't have to be an all four sides but if you do then that is the conventional way of doing it.
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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.
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http://www.chemicalelements.com/elements/be.html\n\nthis website may help you!!!!!! ( hope you get an A)
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Actually I think there would be three dots:\n                    .B: \nRemember that Boron has three electrons in the second energy level and five total.\n\nThe sites below should have some good answers for your future Chemistry related questions.\n\nGood luck on your homework,\nArmus
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An electron pair acceptor is a Lewis Acid, while a electron Pair donor is a Lewis Base. Sodium wants to give its electron away because that is the easiest way to make itself electronically more like a noble gas, therefore it is a Lewis base compared to Chlorine. Chlorine wants to accept an electron to make itself more like a noble gas, therefore it is a lewis acid compared to sodium. also see electronegativity, and electron affinity.\n\nhttp://www.abacusscience.com/electronegativity.html\n\nhttp://en.wikipedia.org/wiki/Lewis_acid
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see if this page helps:\n\nhttp://www.chemsoc.org/visElements/pages/data/intro_groupi_data.html
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Xe, element # 54 I believe
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First you should draw the Lewis structure.\n\nBr\n|\nC=O\n|\nBr\n\nThere are 3 lone pairs of electrons on each bromine and two lone pairs on the oxygen.\n\nVSEPR tells us that the molecule is trigonal planar and the oxygen is a bit more electronegative than the bromine, therefore this molecule is polar.\n\nTake care,\nDavid Roth
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If you're referring to Lewis structures, dashes represent pairs of electrons being shared between 2 atoms and dots represent one electron (see link below).  When there is more than one line connecting atoms, that means they are sharing more than one pair of electrons.  Ionic bonds aren't usually represented this way. But to do this, each atom is surrounded by dots representing the electrons present after they are transferred to bond, surrounded by brackets individually (brackets can be left off if there are no electrons after bonding), and the charge is marked in the upper right corner.  The second link shows an example with salt (NaCl).
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well family 13 has B and Al.  they are metaloids that are great lewis acids.  they have interesting bonding strategies that defy the normal octet rule.
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1) O(2) = dioxide\n\n2) SeF(6) = selenium hexafluoride\n\n3) Si(2)Br(6) = disilicon hexabromide\n\n4) SCl(4) = ? sulfur tetrachloride\n\n5) CH(4) = carbon tetrahydrogenide\n\n6) B(2)Si = diboron silicide\n\n7) NF(3) =nitrogen trifluoride\n\ni just learned that today they might not all be right
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It is a tetrahydrate of Iron III salicylate.  The structure can be found in the paper listed below:
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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.
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There is a LIST of them in the link below:\nhttp://www.alltheinternet.com/texis/open/all?q=lewis+structure+of+ions
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The ligand will accomodate electrons from the ligands, forming dative bonds.\n\nThe sub-shell also ceases into two groups of orbitals.  One group will be at a higher energy level as compared with the other.  The difference in energy level is acounted by the strength of the ligand, in other words, by its polarising power.  The stronger the ligand, the greater is the energy difference between the two groups of orbitals.
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start from here---\n\nhttp://en.wikipedia.org/wiki/Lewis_dot_diagrams\nhpe this helps
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You can approach this is one of two ways:\n\n1)  By analogy with H2O (because O and S are both in the same group)\n\n2) From first principles ie octet rule, Lewis diagram, hybridisation, shape. \n\nNow S has 6 electrons in outer shell, while H has 1 each, therefore, S will share 1 e- from each H to complete its octet and each H will share an e- with S so H (which is too small to have 8e-s in outer shell) will have a full outer shell. So S is now covalently bonded to to H atoms, accounting for 4 e-s, with 2 non-bonding pairs. That makes 4 pairs of electrons around S all together, so hybridisation is sp3. Shape is tetrahedral minus two vertices ie bent (just like H2O).\n\nI hope this helps.