How octet is formed in Sulphur dioxide and Sulphur trioxide molecules?
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You have to make double bonds. These are made by moving a nonbonding electron pair from an atom that already has an octet to a position where it can bond an atom that does not have an octet.\n\nSulphur dioxide has 18 electrons. There are electron pairs below the first O, above the S, and above and below the second O.\n\n:O::S:O:\n\nClicking on "Procedure 5 Example" at this site will give you the structure for sulphur trioxide.
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as i have explained with the formation of ionic compounds. this is an ionic compound like table salt (NaCl)\nLithium gives up the one outermost electron to Chlorine which has a stable octet.\nLithium then has just two. Remember, this is the first orbital (s orbital) with a maximum of two electrons.
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lewis dot structure shows the molecule's valence e-s and the bonding of the molecule \n\nit is very easy to draw \nhere are some hints for drawing lexis structure\nfirst you need to find out the valence e-s of that molecule i.e. h2O have 8 VALENCE e-s 2 from the hydrogens abd 6 from oxygen \nthere is is Carbon present in a molecule than carbon should be placed in the middle  if there is no carbon present than least electronegative atom should be in the middle \nput one or two or three pair(s) of electrons in the middle depending on the octet rule which states that all atoms want 8 valence e-s other than H, Be, and S. H bond to get 2 valence electron, Be bonds to get 6 valence e-s and S can get more than 8 valence electrons \nif you are confused or need help with any of the models just email me i will try my best to reply
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d) basic\n\n[Non-metal oxides do the opposite and form acidic solutions if they are soluble e.g. sulphur dioxide dissolves to form sulphurous acid)
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SO3 is sulfur trioxide and has a slightly more complex molecular structure than SO2, sulfur dioxide.
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Yes.  NH3 obeys the octet rule because nitrogen shares two electrons in each of three covalent bonds to hydrogen, and has a free electron pair. 2*3+2=8.
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There are several.  Most are non-metalic oxides.\n\nCarbon dioxide:\nCO2 + H2O --> H2CO3 (carbonic acid)\n\nSulfur trioxide\nSO3 + H2O  -->  H2SO4 (sulfuric acid)\n\nSulfur diodixe\nSO2 + H2O  -->  H2SO3 (sulfurous acid)\n\nNitrogen dioxide\n3NO2 + H2O --> 2HNO3 (nitric acid) + NO\n\nThere are many others.
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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.
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Dipole moment is a vector quantity. It is the vectorial sum of all the bond moments in the molecule. \n\nIf the molecule is symmetrical and the bond moments are cancelled by each other then the dipole moment is zero.\n\nIn case of SO3, the dipole moment is zero because the molecule is trigonal planar.\n\nWhereas the BrF5 is square pyramidal and hence has some dipole moment. The Flourine present above the square plane causes this dipole moment.
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Ozone is trigonal planar.  The lone pairs on the terminal oxygens give the trigonal structure, and the molecule is planar (2 dimensional) mainly due to the double bonds in the most stable resonance structure of ozone.\n\nH2Se should be a bent molecule.  The lone pairs take up maximum available space forcing the tiny hydrogen atoms closer together than they's like to be at an angle of about 91 deg from the Se atom.
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Elements with octet configuration are more stable because the last layer of electrons is complete, so it doesn't have empty spaces to be filled by other elements (not easily). It is not impossible, but hard and not likely to happen under normal conditions. Under special circumstances, I suppose they do mix, like your case with Xenon.
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The Claus process is catalytic reaction of hydrogen sulfide with sulfur dioxide to give elemental sulfur.\n2H2S + SO2 ===> 3S + 2H2O\nSome of the H2S is oxidized in air to SO2. The elemental sulfur is isolated in pure form. This makes it suitable for re-oxidation to SO2, further catalytic oxidation to SO3, and passage through the contact process to make pure, concentrated H2SO4. Amine sweetening refers to reaction of H2S innatural gas with amines, R3N, to give ammonium sulfides, 2R3NH+ + S=
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You should expect a molecular compound to form between N and O (as opposed to an ionic compound).  This is because N and O are both nonmetals.  An ionic compound will form when a metal and a nonmetal combine.  I believe that this is what your question is getting at.
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a=oxygen diflouride\nb=dichlorine octoxide\nc= sulfur trioxide\nd=phosphorus pentoxide
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HF + H2O => F + H3O+\nNH4+ + H2O => NH3 + H3O+\nH2CO3 + H2O => HCO3- + H3O+\nHNO2 + H2O => NO2 + H3O+\n\nbasically, the oxonium ion is formed in each one, when a proton is donated to water.
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You mean the electron configuration?\n\n1s2\n2s2 2p6\n3s2 3p4
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well, i do not know if this is correct but I'll give it a bash.\n\nfor your sulphuric acid there it undergoes a single H dissociation to create the HSO4- conjugate base (well i suppose technically it's amphoteric but for my purposes that doesn't matter) this is an extremely stable ion since it is resonance stabilised.  Thus it resists accepting back the proton and it resists losing it's other proton, because in doing so it would lose a degree of it's resonance.\n\nIn the group 2 hydroxides mentioned they obviously have ionic bonds and not covalent therefore they cannot have have resonance structures.  The reason they lose both hydroxides or none would be if the enthalpy of solution, that is if the polarity of the water molecule and the other factors of electron affinity/ionisation is strong enough to break the M--OH bond then it will do so twice and there is no way to stabilise a single dissocation product.\n\ni think.