How do you draw a molecule?
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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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Cut out a cardboard circle, draw colors on that or glue the color wheel on it.\nPut a needle through the centre (as the axis) and use 2 forks to hold the needle.\n\nIf you need a lot of spin, tie a rope around the needle and pull
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the goal is to make the total amount of atoms on each side equal\n\nso you add coeficients to the front of molecules (which is multiplied by the little numbers on bottom) and see if you can get the same number on both sides. its kind of hard sometiems if you dont see it.
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One way is by growing a big, pure crystal of the material. Since all the molecules are the same, and the crystal is pure, then all the molecules must fit together a certain way to form the shape of the 'ideal' crystal. \n\nX-ray crystallography, which the previous answerer referred to, is when they shine a thin beam of x-rays through the crystal, to see how they are diffracted. This shows how the crystal is constructed inside.\n\nIn addition to this, if the molecules are large enough, an electron microscope can sometimes see the layers of molecules on the outside of a crystal, or the inner layers if it is split open. \n\nBy using techniques like this, scientist can build up a mental concept of what shape and size the basic units of the crystal must be, the molecules. Then they can make little stick-and-ball shapes that represent the molecules and build up large structures (representing very tiny crystals.) If their predictions are correct, the large shape they build up should resemble the actual crystals, with the same angles and the same shape planes, etc.\n\n19 NOV 06, 1756 hrs, GMT.
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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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N2+3H2=2NH3\n\nFirstly elemental symbols start with capital letters\n\nSecondly you need to know what they mean\nN2 = molecule of nitrogen\nH2 = molecule of hydrogen\n\nThirdly you need to know that NH3 is called ammonia\n\nThen it says 1 molecule of nitorgen + 3 molecules of hydrogen combine to form 2 molecules of ammonia (NH3)
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TCATTG\n\nT molecules connect with A molecules\nC molecules connect with G molecules
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Gotta love wiki\n\nhttp://en.wikipedia.org/wiki/Octane\n\nclick on each one of the 18 isomers, then you can draw. Basically, you shift a methyl group from carbon 1 on down the line so you don't have a straight hydrocarbon chain.
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Draw it your self on x-y plane, then determine the coordinates
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The shape of the molecule depends on how many electrons and bonds you have in the outer shell of the central atom.\nFor NH3, N is the central atom. It has 3 covalent bonds and a lone pair. Thus the repulsion of the lone pair electrons and the bond electrons will force them to arrange at the corners of a tetrahedral. The molecule will look as a trigonal pyramid (since the lone pair is not "visible" in the structure.\n\nFor BH3, B is the central atom and has no lone pair apart from the three bonds. So the repulsion of the bond electrons will force them to be in a planar trigonal arrangement.
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ask your chem prof or tutor ..it's hard to explain over the internet!
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The question is more throroughly stated as "find the minimum whole numbers of each molecule in this reaction so that it balances the number of atoms."  \n\nYou could devise a set of three of algebraic equations so that you wind up with the same amount of oxygen and hydrogens on both sides.  That would be the general way, or you can just do it semi-intuitively with a simple equation like this one.  I will walk you through it. I could just *tell* you the answer, but then you wouldn't learn!\n\n\nSince both reactants are diatomic(*), look at the products:  what is the least abundant atom there?  \n\nNow pick the smallest whole number of the reactant molecule on that still gives you a whole number of product molecules on the product side. \n\nNow see how many of the other molecule you need on the reactant side to get the right number of product molecules (determined in the last step) on the product side. \n\nFor complex reactions with some of the same atoms in multiple reactants and perhaps with multiple products on the other end, it will become harder to just "see" the answer and you will need to rely on the general solution of setting up algebraic equations to solve, so you should learn this technique.  \n\nDo this simple one and maybe a few more, and then see if you can devise the general solution technique yourself to solve them again.  Since you know the answer already you have a ready "reality check" to verify your technique.
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for one molecule of H2O, there will be one molecule of H2 and one molecule of O.\n\nfor one molecule of H2O, there will be two atoms of H and one atom of O.
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a resonance structure can be drawn if there is an allylic lone pair (a lone pair adjacent to a pi bond). you also want to draw resonance structures to delocalize (move to stabilize) a charge. generally, you want a negative charge to be on the more electronegative atom, and you want as many octets filled as possible. hope this helps :)
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Try it out in the lewis-dot diagram\n      ..        ..\nH-O-Ca-O-H\n      ..        ..
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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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There is one line (bond) between the H and the Br.  It looks like this: \nH-Br\nThat's all. To make it a Lewis dot structure, you can put 7 dots around the Br to represent the valence electrons.  \nHBr is hydrobromic acid in aqueous solution.