what would the lewis dot structure for COCl2 be?
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.
950288
1)  Only the valence orbitals matter, and all the valence orbitals count (more complicated version: all valence orbitals which are of the correct symmetry to hybridize to form MO.  If you don't know what that means then you're in a lower level class and it doesn't matter).  # of atomic orbitals = # of molecular orbitals, and the molecular orbitals may be bonding, nonbonding, or antibonding.  Not depending on the particular class you're taking your teacher may or may not want you to draw the non-valence orbitals, but they don't matter at all.\n\n2)  You start filling all the MOs with electrons, starting with the lowest energy and moving up.\n\n3)  You wouldn't determine that for C2 because that's not correct.  The bonding and antibonding orbitals formed from the 2s atomic orbitals would both be filled (net bond order of zero) the lowest bonding (sigma) MO from the 2p AO would be filled, and each of the higher bonding (pi) MO from the 2p AO would have one electron.  None of the antibonding orbitals from the 2p AO would be filled.\n\nThis predicts that C2 would have 2 unpaired electrons, whereas a Lewis structure would predict a quadruple bond between the carbons.  One guess as to which one is right....
315781
you are in the wrong section!!! this is math section...u need to go chemistry section....\n\nAnyway, the formula for cobalt(III)chloride plus ammonia is........\n\nCoCl3 + NH3 = NCo + 3HCl
960668
http://www.stolaf.edu/depts/chemistry/courses/toolkits/123/js/lewis/\n\nI agree it is too hard for us to draw lewis structures in a forum like this. What helped me learn lewis structures is by practicing them on sites like these. If you follow each step you can do lewis structures for anything.
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.
626516
BeCl2 disobeys. It has 4 valence electrons. XeOF4 disobeys. It has 10 valence electrons.
822762
Both CH3F and CF4 are tetrahedrons, but due to the substitution each has a different symmetry (C4v and Td respectively), as a rule the lower the symmetry the higher the polarity of the molecule. Actually, any Td (fully substituted tetrahedron), Oh (fully substituted octahedron), D4h (fully substituted square planar), D3h (fully substituted trigonal bi-pyramidal) will be non-polar molecules. This is due to the cancellation of the dipole moments.\n\nThus in order of the strongest dipole moment the answer is\n\nCH3F > CF4 (C3v < Td)\nXeO3 > XeO4 (C2v < D4h)\nSO2 > CO2 (C2v < D(inf)H)\nCOCl2 > BF3 (C2v < D3h)\n\nIf you are having a hard time understanding the Schoedinger group types, try a 3D modeling program (eg Spartan Build or ChemDraw 3D) to see the differences in the symmetry of the molecules.\n\nI hope that this helps. Please feel free to contact me if you have any further questions.\n\nKen
363082
2Ag+ + CO_33-2 -> Ag_2CO_3
980544
1) MgCO3\n2) AlF3\n3) BF3\n4) NH4F\n5) SnO2\n6) HCL\n7) Ca(OH)2\n8) Na2S\n9) K2SO3\n\n1) do yo mean PbCl2? then Lead (II) Chloride\n2) Lithium Bromide\n3) Potassium Sulfate\n4) Megnesium Hydroxide\n5) don't know\n6) Hydrogen Nitrate\n7) Barium Phosphate\n8) Carbon Monoxide\n9) Copper Brimide\n10) Ammonium Chloride\n11) Tin (II) Hydroxide\n12) Calcium Nitrogide\n13) Strontium Oxide\n14) Tetraiodide prefix for 9 and oxide\n\nFe^+2\nNi^2\nAg^+1
226109
It is lithium Chloride i.e. LiCl\nIt is an covalent compound rather than being an ionic compound. It is define by FAJAN's rule
770078
alcl3 is trigonal planar (bond angle 120')\nco2, straight (180')\nh20, bent (~105')\nch4 and ch2cl2 are tetrahedral. (~110')
910345
The formula would be Al2(CO3)3; the numbers are subscripts. \n\nLearn your charges for the polyatomic ions and for the other elements, it will really help.
337603
Here is the answer.. Just remember periodi table...\nElements on left most side are electro positive and elements on right most are electro negative. (The last row is nobel gases..so leave it)\nNow Cl- belongs to right most side... its more electro-ve\nRb, Ca are on left side.... they are electro positive(They will give  electron with out much force)\nSi, S are in middle-- their properties are in between...\n\nThats it!
669373
Electron Dot Formula, aka Lewis Dot Formula, comprises with the octet rule, which states that any stable compound (or element) must have eight electrons in its outer shell. But sometimes, Lewis Dot Formula is just a representation of any molecule just to give perspective on the pairing or sharing of electrons during a reaction.\n\nfor example:\n\nHydrogen gas has only 1 electron to fill up its orbital shell, Oxygen has 6 electrons on its outer shell, that's why this diatomic element needs 2 electons to become stable. Using Lewis Dot Formula:\n\n(note: i use + to indicate dot)\n\nH+ +O+ +H -------->  H:O:H \n(this H:O:H is the Lewis Dot Formula for water)
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.
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...
698948
1)   O::C::O  for CO2 because there are total 4 valence electrons in outermost orbit of carbon so it will share 2 with each oxygen and it has 3 resonance structures\n\n2)  H . . C three electrons shared from carbon and nitrogen N\nie on one side one electron sharing by hydrogen and carbon and on other side 3-3 electrons shared by both carbon and nitrogen\n\ni hope it helps you out