how do you do a lewis dot electron structure?
397844
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.
960765
to attain an octet electron config.\n\nzinc has 10 electrons in its valence shell. it gives up 2 when it ionises so it can form the magic 8 that is stable. fyi, many atoms in the the table strive to attain this 8, and this principle drives the understanding of many compounds formed from the elements.
199063
Al has atomic no.13,\nits e.c will be 2,8,3\nin lewis dot structures we represent the valence shell electrons by dots.\nIn case of Al,the valence electrons are 3.so,Al with 3 dots around it is the answer.
80472
I'm trying to work with this info:\n\nOctet Rule - atoms want to have eight electrons in their valence shell (two for H) (most will form octets, some will not)\n\nMultiple Bonds\nSingle bond - a covalent bond in which a single pair of electrons is shared by two atoms\ndouble bond - two pairs of electrons are shared by two atoms\ntriple bond  - three pairs of electrons are shared by two atoms\n-generally form with C, N, O, S\n-------\nOkay, oxygen might attach easily to one of the Cls, leaving no spaces, but I'm not sure if there is a doule bond or something weird like that. Same with C.\nIf I remember correctly, CO2 looks like this:\nO=C=O\n------\nWait, check this out- I found the following (and no further info) somewhere on the net.\n\nE) COCl2\n      (C is the \n       central atom)\n\n----------\nWait. No.\n_______\nCl- C -Cl\n___O___\nI'm going to try that...\nI don't know. It lacks the symmetry that you normally see and it's kinda weird looking. What do you think of what I got?\n__________\nI found a pic: http://www.chem.ox.ac.uk/inorganicchemistry3/C/COCl2.html\nLooks kinda like yours.\n______\nHoly Mother of God - http://www.chem.ox.ac.uk/inorganicchemistry3/C/COCl2.html\nI found the name of the compound- phosgene- and did an image search. *exclamation of glee*\n___\nLol, better be right. Later.
908581
C, Al(OH)3...\nWould you like an explanation? Okay, I'm supposed to be learning about this in Chemistry right now, so, I think this is how it works...\n\nIf you study the periodic table of elements, then you will find the number of valence (or outer) electrons each element has. Al has 3, O has 6, and H has 1. Before we start, it is important to know that a filled orbital has 8 valence electrons... okay? \nO and H combine, so they have a total of 7 valence electrons. You can imagine this by thinking of the letters OH surrounded by 7 dots in a circle, 2 pairs of dots on each side and 1 alone (a filled orbital with have four pairs opposite each other). The lone pair needs an electron, so it can borrow one from aluminum, which has 3 electrons. Aluminum loses its electron, so now it has 2, and the OH is now full, because it has 8 electrons. However, the aluminum has to get rid of its other two electrons, so another OH is brought in. The aluminum gives up an electron and the second OH is now full. Finally, the last OH pair is brought in and the aluminum gives away its last electron. So now, it is empty and the OH's are full. I guess they're balanced. Anyway, you are now left with 1 Al and 3 OH's, making Al(OH)3. Do you understand now? \n\nAl (3), and OH (7) (because O=6 & H=1, which equals 7)...\nAl - 1 = (2), so now OH = (8) (now it's full)\nAl - 1 = (1), so a 2nd OH (7) is brought in, making it OH (8)\nAl - 1 = (0), so a 3rd OH (7) is brought in, making it OH (8)\n\nIt took 1 Al and 3 OH's, so the new compound is Al(OH)3\nHope this helps!!!\nP.S. sorry for any confusion earlier when I tried to "draw" them. The computer changed the spacing so all you could see was a mess of stars and stuff. : )
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!
603525
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.
575353
That is simple- Just write down the the electronic configuration of the atomic number of that element. And the number of electrons in the last shell are the valence electrons.\n\nFor eg: Na(Sodium) has the atomic number 11, now there are four shells in which the distribustion takes place- namely- K,L,M,N.These shells are also known as energy levels. \n\nThe max no of electrons in K is 2, In L is 8, M is 16 and finally in N its 32.\nAnd you cant fill the next shell till the total number is completed in one shell.\n\nThere fore for Na the configuration is: K= 2 L= 8 M= 1\nAnd hence the valence electron is 1. That is only one electron partcipates in bond formation and in chemical reactions.
4115
You always want to place the formal charges in the places they will spend the most time--hence, the formal charges are what you'd draw up first, based generally on the electronegativity and stability of the place.  The resonance structures are just to give you an idea as to where the electrons might wander over to.\n\nTechnically, all the Lewis structures are just to help you understand the charges.  In reality, the elecetrons are constantly moving about, with their locations only localized by a probabilistic model.  The formal charges are indicative of the highest probability that a given electron will be found, while the resonance structures are the less probable locations to find the electron.
735086
Lewis diagrams are two-dimensional diagrams, used to draw on paper the basic nature of the chemical bonds between atoms.  By representing valence electron orbitals as dots (each dot representing an electron in the valence orbital), it is easy to see how each atom in a molecule is bonded to each other atom.  It is also easy to imagine which chemicals will and will not react with one another based on the Lewis diagrams.\n\nWhat the Lewis diagram lacks, however, is a 3-Dimensional representation of the molecule.  The ball-and-stick models (aka "chemical tinkertoys") allow the student or researcher to much better visualize the molecule as it really exists.\n\nMany physical or mechanical properties of substances (such as crystal formation, viscosity, soluability, etc.) are much more closely related to the SHAPE of the molecule than to the BONDS within the molecule.  This is where the 3-dimensional ball-and-stick models overcome the disadvatages of their bulk and the time needed to assemble them.
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
950942
Selenium will have 6 valence electrons just like oxygen.  Place the Se as the central atom.  Two OH groups will single bond to the Se (remember H has only one valence electron).  One O will double bond to the Se. \n\nDraw it a couple times till you get it looking good, and you'll remember it. You can cheat and look at the last link below, and substitute Se for the S in the structure given.
835765
1) one s + three p + one d give five equivalent sp3d orbitals\n2) O=C=O, two sigma, 2 pi bonds\n3)a) 10e-; α2s2 α*2s2 π2p4 α2p2; diamagnetic\nb) 12e-; α2s2 α*2s2 π2p4 α2p2 π*2p2; paramagnetic (isoelectronic as o2)\nc) 14e-; α2s2 α*2s2 π2p4 α2p2 π*2p4; diamagnetic\nd) 10e-; same as a) above\n4) No molecules shown!\n5) The structure of graphite is planer, all sp2 carbons with an electron in the p-orbital. There are planes of carbon atoms well bonded together. Between these planes there are pi electrons and they are free to move; they are said to be aromatic pi electrons. When you apply a voltage, these electons do move - and moving electons is current - ie it conducts electricity. On the basis of MO theory:  Because the MO theory holds that electrons are not held to only one position. Instead they are spread across the entire molecule. \n6) No, it is trigonal planar, any individual dipoles from the B-F bonds are negated by the symmetry of the molecule.
17774
It doesn't give me room to list them all and explain them on here so let me direct you to a website I found that does a pretty good job:\nhttp://vergil.chemistry.gatech.edu/notes/quantrev/node20.html
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.
712147
The way I learned it was that the dots were part of an electron dot diagram.  It showed how many electrons (the little dots) were in the electron cloud of an atom.  I think they were left over after the electron levels were filled in as much as they could be. (Did you learn that?) Here's a link if it wasn't clear: http://en.wikipedia.org/wiki/Electron_dot_diagram
981192
http://periodic.lanl.gov/default.htm\n\nClick on the element, and it's in the top section of information. To write out the electron configuration for every element would take quite a while, so if you need it for a specific element or a few elements, I'd reccomend asking just for the few.