How do you do Lewis Dot Structures?
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In the formation of a molecule only the outer shell electrons are involved and they are known as valence electrons.It is, therefore, quite reasonable to consider these valence electrons while discussing chemical bonds and other chemical properties as the case may arise.\n          G.N.Lewis introduced simple symbols to denote valence electrons in an atom.The outer shell electrons are shown as dots surrounding the symbol of the atom. These symbols ignore inner shell electrons. This type of representation is known as Lewis dot representation.Structures of molecules denote by this representation is called Lewis dot structure. \n The common valency of the element is either equal to the dots in Lewis symbol (if less than equal to 4) or 8 minus these dots (if these are more than 4)\n\nFor examples of dot structures click the following link:\nhttp://img106.imageshack.us/img106/3875/untitled1ju.jpg
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This site is a good resource for chemical structures and their properties.\nhttp://www.chemicalland21.com/\n\nSpecifically for Sodium erythorbate:\nhttp://www.chemicalland21.com/lifescience/foco/SODIUM%20ERYTHORBATE.htm
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The octet rule refers to Lewis dot diagrams and how electrons are arranged in molecules. During covalent bonding, atoms have eight electrons in their orbit, whether or not they are shared with another atom. An example of the octet rule would be oxygen atoms (each with 6 electrons) in a diatomic oxygen molecule sharing a total of four electrons between each other while keeping four electrons to themselves. Of course, the octet rule does not apply to hydrogen, which can only hold two electrons. The octet rule also applies to ionic bonding, where the anion (the negatively charged ion) gains a number of electrons to  have a total of eight electrons in its orbit.
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C4H9N3O2 For the structure goto http://www.cwu.edu/~chem/courses/chem388488f00/coulombe/CREATINE1.GIF
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Doing the Lewis dot structure for lead is a little hard here since I can not necessarily draw the structure on the screen, but here is how to do it.\n\nFirst, take out your periodic table and see where Pb, lead, is located.  Then, determine how many s and p electrons you have, do not count the center electrons is basically what you do, meaning it has 4 outer electrons.  Thus, draw 4 dots around Pb, and you have a Lewis dot structure.
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a the number of outer electron that will bond with other atoms to fill thei valence shells
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In the Lewis structure, dots left alone want to pair up with those of another atom.  If there are 5-6-7 dots all around, the atom will accept electrons to fill it last layer.  If there are 1-2-3 dots, the atom will want to give those electrons away.\n\nSo you look at your Lewis structures, and try to pair up alone dots from one giving atom to a receiving atom. \n\nFor your peroxyde, you would get H.   and :.O.: twice so one link between and H and a O, another link between the other O and the other H, and then the two O's link together.\n\nFor you chlorine, there are 7 dots all around each atom, so they will share their un-matched electron in a covalent bond.  \n\nFor the CH4O, their are 4 dots all around the carbon, so you would think that one H will bond to each (that's 4 H then) but to add the oxygen, you have to insert it between a H and the C (that the hydroxyde radical).  It is written CH3H usually to show the -OH polyatomic ion.\n\nFor the C2H4, the carbon has 4 dots all around it, and they will bond to each other.  Each will link to two hydrogen (to make up the four in the molecule), leaving two dots on each C, so this means that there will be one double bond between the two carbon atoms.\n\nFinally, the CH2O os trickyer.  That carbon, with its four dots, will have one H bond to each one dot, so there are two free electrons left.  That oxygen has six dots, two pairs and two free.  This means that each free electron of the O will link up to one of the free electrons on the C, which means that there is one double bond between the carbon and the oxygen.  You'll have H-C-H for the first part and C=O for the second part.\n\nIt's kinda hard to type these :-)  Hope this helps anyway
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Due to differences in chemical structures
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8 dots around each element. this is a salt, so is realtively stable. hope that helps!
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go to encarta.msn.com and search for keys mass/solid structure, surface Structure
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You should consult a chemistry textbook, if possible, or if not, look online for an answer; I'm sure there is information or a guide describing how to do it better than I can in a few short sentences. That said, the basic way to draw a molecule (often abbreviated mlcl) is to use each element's symbol(ie sodium=Na, carbon=C, etc) to denote an atom, and to draw a single, solid line for each bond between elements. This line/bond represents 2 electrons, aka one orbital. Most elements like to have 8 electrons in their valence (outermost) shells in order to be stable, but this doesn't always happen; there are many exceptions, hence my suggestion to look at a textbook or online text/guide.\n\nIt gets more complicated when you're dealing with things like organic chemistry or complexes or chelating agents where sharing of bonds/electrons is pretty common and there are more types of bonds. For a simple example, if you had a 6-carbon atom ring, each carbon has 6 electrons in its valence; it wants 8, so what happens, does it get frustrated with its misfortune and self destruct, destroy our little universe? Of course not... there are a total of (6)(6)=36 electrons, and we need (6)(8)=48. How is this possible? Clearly, 36 is not equal to 48. We can't create more. So what happens? As it turns out, carbon, along with most other elements, passed kindergarten with flying colors- they SHARE them, and since it's a symmetrical hexagon shape of identical atoms, they are shared equally. There are all kinds of crazy combos in which the electrons are shared unequally between atoms because of something called electronegativity, but our rules for drawing those lopsided things aren't very different. However, that's for another 'lesson;' don't worry about it for now.\n\nSo, in order to make the carbon happy, we have to share 12, or 6 pairs, of electrons. ([48 needed]-[36 that we have] = 12) \nSince this carbon ring has multiple resonance structures (atom config the same but electron pairs on different atoms), we draw six carbons in a hexagon, with one solid line bond between each, and a dotted circle in the middle- this accounts for all of its resonance structures and provides us with more info, in addition to only needing one drawing to display that info, than using single bond lines only.\n\nSo in conclusion, I've said way more than I really had to... from the level of generality of your question I assume that you don't know too much about chemistry; if you are confused with what I said, then do as I said- look up the info online or get a book. It's not too easy to understand right away but with some patience you should be able to figure it out just fine; good luck.
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The Lewis Dot diagram shows the number of electrons in the outer shell of an atom. These are also known as valence electrons. You simply determine the number of outer electrons an atom has, write the chemical symbol of the atom and by twos, place the same number of dots as there are outer electrons around the chemical symbol. Place the dots at the top, bottom, left, and right of the symbol.\n\nHow do you determine the number of outer electrons? Look at the periodic table. \n1. All the elements in the first column from Hydrogen to Francium all have 1 outer electron.\n2. All the elements in the second column from Beryllium to Radium have 2 outer electrons.\n3. Skip all the way to Boron. All the elements in that column have 3 outer electrons.\n4. Carbon's column has 4 outer electrons\n5. Nitrogen's column has 5. Oxygen's has 6. Fluorine's has 7\n6. Helium only has two, but the rest of the column under Helium has 8.
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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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Go to http://rutchem.rutgers.edu/Courses_f04/Chem161/Lecture19k.pdf#search='lewis%20structure%20for%20nitrous%20oxide' and scroll down until you see it
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You proffered the example of XeF4.  Now the Lewis structure for XeF4 gives an expanded octet, viz: AX4E2, where A represents the central atom (Xe) in this example; X represents a shared pair of electrons; and E represents an unshared pair.  Thus for XeF4 we have 4 shared pairs and 2 unshared pairs, i.e. 6 pairs.  \n\nNow whatever the principal energy level(n), there is 1 s orbital; and for n=2 and higher, there are 3 p orbitals; and for n=3 and higher there are 5 d orbitals. For n=4 and higher there are 7 f orbitals.\n\nNow considering XeF4 hybridization, for the 6 pairs of electrons there will be 6 orbitals [each orbital holds a maximum of two electrons with opposite spin]. That means sp3d2 hybridization.  That is the one s orbital, the three p orbitals and two of the five d orbitals form six sp3d2 orbitals.  Of course, we are talking here about valence shell electrons.  How would these orbitals fill?  Well, electrons are added to orbitals such that electrons with the same spin are added until there are no more empty orbitals, then the orbitals with one electron fill (i.e. add a second electron) by acquiring an electron of opposite spin.\n\nThis gives XeF4 sp3d2 hybrid orbitals and an octahedron orientation. \n\nConsidering the Lewis structure for water, as another example, we obtain a AX2E2 form. Thus sp3 hydrid orbitals and a tetrahedron orientation. The 4 hybrid orbitals come from 1 s and 3 p atomic orbitals.
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determine how many valence electrons each atom has. locate the central atom and spread out its valence electrons(each electron is represented by a dot). then pair up one from the atoms attached to the central atom. finally put all the other electrons for each outer atom around it.\nyou should see all electrons paired up, many times each atom will end up with eight electrons around it but many times there will be more or less than eight.
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build a model of the element tungsten? chemists generally dont build models of single atoms but do model compounds. Maybe you're after a Lewis dot structure of tungsten describing the nuclear charge and the electrons in the orbitals. So, get a periodic table and look at where tungsten is...its the 74th element with symbol W. That means it will have 74 protons, so the nuclear charge with be 74+ and to balance it will have 74 electrons arranged in shells. The periodic table tells you how these shells are filled. The rows of the table indicate which shell an atoms is in and the shells are can accomodate electrons as follows;\n\n1st shell (first row, H and He) - 2e\n2nd shell (2nd row, Li all the way to Ne) - 8e\n3rd shell ....       8e\n4th shell ....      18e\n5th shell           18e\n6th shell            32e\n\nTungsten is in the 6th row... 74 electrons so in your lewis diagram you draw 6 big concentric circle around your 74+ charge. In the first (closest to nucleus) you put to 2e, the 8e, then 8e, then 18e, 18e which in total adds up to 54... 20 left over to put in the final outer shell.\n\nNow this is one way to represent the atom Tungsten, amodel if you will...but its a pretty crap one since it suggests that Tungsten has 20 electrons in the outer shell to bond to other atoms - this just isnt true! Lewis models are fine for small atoms like O or nitrogen but they just dont work well on transition metals...most stuff after the third row really. To accurately predict the bonding of tungsten and other atoms like it you really have to use atomic orbital theory and its complicated so dont worry about it for now.\n\nanyway, hope this helps