What is the Lewis Structure for NCS(minus) and how do you determine it?
912160
[N=C=S]-  with 2 pair of electrons for each: N & S. Count the valence electrons for each atom (5 for N, 4 for C & 6 for C) plus an electron for the minus. You have a total of 16 electrons. Draw the structure. Every bond contains 2 electrons, so inicialy you'll see that you only have 4, put the other as pair of electrons around each atom (respecting the octect rule- 8 electrons for each atom-except for H that only can have 2- and families after period 2 don't necessarly respect it, but for now you can ignore this last fact). After you do this you'll see that you have more electrons than needed, this is where you have draw double or triple bonds. Count the bonds and pair of electrons (each have 2) until you are sure you have your 16. [ ] are to indicate charge.
761407
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
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.
503103
No - methanol, ammonium\nYes - formic acid, sulfur troxide\nKinda - carbonate, nitrate, chlorate (all can be drawn as resonance structures, so the bonds aren't quite single and aren't quite double)
426762
you know its ionic because Na is a metal while Cl isnt. a metal and nonmetal almost always from an ionic bond. to draw a lewis digram, determine how many valence electons are in each and draw the diagram.. its kinda hard to explain without actually drawing it.. consult a chem bk.
855087
Ca2+=[Ar]\nMg2+=[Ne]\nI-=[Xe]\nF-=[Ne]
727505
1. M1X1 (no subscripts), because alkali metals are +1 and halogens -1.\n2. M2X1 (subscript 2 for the metal), because group 6a elements are -2 in binary compounds\n3. MX2, because alkaline earths are +2.\n4. MX (subscripts each 1) because alkaline earths are +2 and group 6a elements -2.\n5. MX3, because group 3a metals are mostly +3. An important exception is thallium, which is either +3 or +1. So thallium chloride could be TlCl or TlCl3.
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
361732
Lewis structure of CH2Br2\n\nIts identical to the lewis structure of methane but just replace two hydrogen atoms with bromine atoms (remember to add the three lone pairs around both bromine atoms).\n\nNow about polarity:\n\nThe C-Br bond is then considered to be polar. Having bromine slightly negative and carbon slightly positive. Over all the molecule is polar.\n\nSymmetry:\n\nAnd yes dibromomethane (CH2Br2) has two planes of symmetry, one horizontal and one vertical. In order to verify this, you have to look at the molecule in three dimension and not two dimentional (as drawn on a paper)
825026
what you need to do, get a SI data book, and look up their natural state. not bonded with anything else, and possibly itself.\n\nPhophorus - white: molecular (P4). red: Chain. Black: Layer\nIodine - molecular (I2)\nMagnesium - hexagonal closest-packing\nNeon - cubic closest-packing\nArsenic -grey: 3d structure - Layer formation. yellow: molecular As4\nSulfur- molecular S8\nBoron - complicated structure.\nSelenium - grey: chain, Red: molecular: Se8\nGallium - Complicated\nCesium - body-centred cubic\nOxxygen - O2, O3 molecular
429906
Never trust materials science majors ...\n\n1. NaCl (s) --> Na+ (aq) + Cl- (aq)\n2. Ca (s) + 2H2O (l) --> Ca(OH)2 (s) + H2 (g)\n3. Ca(OH)2 (s) --> H2O (g) + CaO (s)
105132
3 Sn(NO3)4 + 4 AlCl3 --> 4 Al(NO3)3 + 3 SnCl4
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C4H10\n\nCH3-CH2-CH2-CH3
130061
Yes, CN- has a triple bond, and N is slightly more EN than C, Remember that electronegativity increases up and to the left in the periodic table!
958410
1.\nMn(s) + SnCl2(aq) --> MnCl2(aq) + Sn(s)\nCr(s) + 2HBr(aq) --> CrBr2(aq) + H2(g)\nCo(s) + CaBr2(aq) --> N.R\n2Al(s) + 3Ni(NO3)2(aq) --> 2Al(NO3)3(aq) + 3Ni(s)\n\n2.\nMg + 2AgNO3 --> Mg(NO3)2 + 2Ag\nmole of Ag = 3.580 / 108 = 0.033 mole\nmole of AgNO3 = 0.033 mole = 33 mmole\nmolarity of AgNO3 = 33 / 50 = 0.66 M\n\n3.\na.soluble\nb.soluble\nc.soluble\nd.insoluble\ne.soluble\nf.soluble\ng.insoluble in water, soluble in acid\nh.soluble\n\n4.\n3NaOH(aq) + Fe(ClO4)3(aq) --> Fe(OH)3(s) + 3NaClO4(aq)\n3Na+ + 3OH- + Fe3+ + 3ClO4- --> Fe(OH)3 + 3Na+ + 3ClO4-\nFe3+ + 3OH- --> Fe(OH)3\n(NH4)2SO4(aq) + Pb(NO3)2(aq) --> PbSO4(s) + 2NH4NO3(aq)\n2NH4+ + SO42- + Pb2+ + 2NO3- --> PbSO4 + 2NH4+ + 2NO3-\nPb2+ + SO42- --> PbSO4\n\nHope it helps\npeace\nvixklen
916756
non polar  \nit's linear in shape ,so the magnet moment equals zero \nthe lone pairs around the two O atoms \nevery O atom has 2 lone pairs\nthe central atom is C atom
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!