HOW DO U DRAW A LEWIS DOT DIAGRAM FOR Hsub2CO?
826844
H\n |    \nC=O:  (You need 2 lone pairs on Oxygen)\n |   \nH\n\nIt doesnt get much better than that :)
284075
It's fairly easy don't worry.\n\nNo need for d level splitting diagrams to answer this since we're dealing with N and F:  use the spectrochemical series to make an assumption about the ligand.  The difference in t2g and eg levels (∆o) determines whether a complex is low or high spin.  If both ligands were the same, we would have to look at the oxidation state of the ligand in the complex.\n\nHalides <  Oxygen ligands  <  Nitrogen ligands < CN- ligands\n\n   ALWAYS HIGH SPIN    ---------------            ALWAYS LOW SPIN\n\nIf ∆o > P, then a complex is low spin.  IF ∆o < P the complex is high spin.
557940
google diagrams and draw it out
234957
Check out this site: http://www.questconsult.com/~jrm/enthpres.html\n\nUse the component id for oxygen (28) and mole fraction (1.00), press submit form. Makes a nice Enthalpy-Pressure diagram.
1043018
Here are a couple sites that might help. I could not find any diagrams though. Good luck!
770561
these arent elements... they are compounds. you have to separate them first. then look at ur P.T. (periodic table) and if u look at the 8 tallest rows (the first 2 and last 6). from left to right, number the columns 1-8. whatever column number an element is in, that is how many dots are used. i hope this helped!
409909
Symbols: LIHRY,FCX,GLG AND GG.
2092
that's a trick question.. you can't have a lewis dot structure for iron.. The Lewis dot structures represent elements who's outer shell consists of electrons in the s and p orbitals, iron is in the d-block.  What i mean is that only the first two groups and the last 6 groups on the periodic table can have lewis structures, elements in the first group have one dot, second have 2, then it skips over the transition metals(which is what iron is) the 13th have 3, 14th have 4, etc up to 8.  d-orbital electrons(which are where the outer electrons of those transition metals are) are not as reactive and don't behave in the same way and so cannot have lewis structures.\n\nthat's a trick question.. you can't have a lewis dot structure for iron.. The Lewis dot structures represent elements who's outer shell consists of electrons in the s and p orbitals, iron is in the d-block.  What i mean is that only the first two groups and the last 6 groups on the periodic table can have lewis structures, elements in the first group have one dot, second have 2, then it skips over the transition metals(which is what iron is) the 13th have 3, 14th have 4, etc up to 8.  d-orbital electrons(which are where the outer electrons of those transition metals are) are not as reactive and don't behave in the same way and so cannot have lewis structures.  \n\nIf you meant electron configuration, then the electron configuration for iron is:  1s2 2s2 2p6 3s2 3p6 4s2 3d6 (where every third number is a superscript and the whole thing is written as one line) if that makes no sense, then that's not what you meant and ignore it haha...
947778
You need to make sure that there is the same number and kind of atoms on each side of the arrow.\n\nCa(OH)2 + MgCl2 ---> Mg(OH)2 + CaCl2, both Mg and Ca stay+2\n\nBaO2(s) + H2SO4 ---> BaSO4(s) +H2O2 \n\nAg2S --->2 Ag+  +  S-2\n\nHC2H3O2 + MgCO3 (s) ---> H2O + CO2 + Mg+C2H302-\n\nI may not have written net ionic form, but I did get all the atoms on each side I am unsure of the reaction producing hydrogen peroxide, but you do have to account for all atoms.
87059
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.
844758
Using the Michaelis-Menten equation.\n\nMore details on teh attached link\n\nhttp://www.le.ac.uk/by/teach/biochemweb/tutorials/michment2print.html\n\nGood luck
848068
ICl2 + should be bent like water since I will have two lone pairs and two Cl's on it.\n\nI3- will be linear\n\nSbCl6- will be octahedral
874456
If they are linear, then it's quite easy. \n\n1. Number the carbon atoms, trying to assign the lower number possible to double and triple bonds.\n2. Check for double or triple bonds an their numbers.\n3. Write a preffix that expresses the number of carbon atoms:\n\nif its 1 , "meth"\nif its 2 , "eth"\nif its 3 , "prop"\nif its 4 , "but"\nif its 5 , "pent"\nif its 6 , "hex" and now you can carry on.\n\n4. Write the number of the double or triple bonds present.\n5. Write a suffix for the type of compund (no double bonds: "ane", double bonds, "ene", triple bonds "yne")\n\nExamples are:\n\nCH3-CH2-CH=CH2     ____   1-butene (or butene)\n\nCH3-CH2-C≡C-CH3     ____    2- butyne\n\nCH3-CH2-CH2-CH=C=CH-C≡CH   ____    octa-3,4-diene-1-yne\n\nIt can be weird for some cases. So practice.
450334
Okay, cool!\nThe diagram is set up so that on the horizontal x-axis is the "reaction coordinate," which is basically just time as the reaction proceeds.  The vertical y-axis is energy.  \n\nThe potential energy of the reactants is where the graph curve starts, touching the y-axis.  The potential energy value is the y-value at this location.  \n\nWhere the graph curve levels off at the end is the products, so the potential energy of the products is the y-value where the curve levels off.  \n\nThe activation energy is how much energy had to be added into the system to get to the activated complex, located at the peak of the diagram's curve.  Take the y-value at the top of the curve and subtract from the the potential energy of the reactants.  \n\nThe heat of reaction is the difference in the potential energies of the products and reactants.  Take the potential energy of the products, and subtract from that the energy of the reactants.  \n\nIf a catalyst were added, the potential energy of the products and reactants remain unchanged, but the activation energy is less, so you draw a curve that starts in the same place and ends in the same place as the original diagram, but your curve just won't go up as high.  The hill for a catalyst is less steep.
48368
2HC2H3O2 + Ba(OH)2 --> Ba(C2H3O2)2 + 2H2O
165571
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
910312
okay. i just took the test on this and passed with a B. so i promise i know what im doing.\n\nK, look at your elements. then look them up on the periodic table. lets pick, oh say the compout Cl(subscript)2O. that is 2 chlorines, and 1 oxygen. well, chlorine is in group 17, which means that each have 7 valence electrons, and oxygen is in group 16, which means that it has 6 valence electrons. following me so far? okay, take those valence electrons, and add them up. that equals 20 valence electrons. now, position the lewis dot diagram so that the oxygen is between the two chlorines. now, distribute the 20 electrons amongst the three letters, so that each has eight. now each letter should be surrounded by exactly eight dots. keep in mind that it should look like this -- :Cl:O:Cl:, but dots on the tops and bottoms. that is the lewis dot. luckily, this one did NOT have double or triple bondage. but in the event of double bondage, it might look like this -- :Cl::O:Cl, without dots all the way around each letter.\n\nand the VSEPR theoryis quite simple. it is just talking about the potential shapes that chemicals can make. for example, there is linear, or trigonal planar, or tetrahedral. this is vital. i promise that, if you contact me, i can give you a simple cheat sheet (not really for cheating, but it helps your memorization) to remember VSEPR. it gives you the shapes, lewis dot examples for the shapes, and angle measurements.\n\nhope this helps!\n~ally