Determine the electron-group arrangement, molecular shape, and ideal bond angle for each of the following?
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a) Tetrahedral shape. bond angle : 109.5\nNo lone pair on central carbon\n\nb) Linear shape. Bond angle: 180\nNo lone pair on central Be\n\nc) Trigonal pyramdial shape. Bond angle less than 109.5\na lone pair on Cl. 2 oxgen double-bonded and 1 oxygen single-bonded to Cl. 0 formal charge on Cl and the O=Cl. Formal charge on Cl-O is -1.
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CH2Cl2\nThe molecule shape is tetraedric with the carbon in the middle
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Mn(+3) has the electronic configuration of 1s(2) 2s(2) 2p(6) 3s(2) 3o(6) 3d(2)\n\nthe one before me missed the 4s2 so his is wrong
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tetrahedral\n\nmethane, CH4\nCH4 is composed of 5 atoms, 1 atom of carbon and 4 atoms of hydrogen covalently bonded.\nCarbon, C, is the central atom in the molecule.\nCarbon has 4 valence electrons (electrons that can be used in bonding).\nEach of carbon's 4 valence electrons will form a bonding pair with 1 of hydrogen's electrons.\nThe central carbon atom will therefore have no lone pairs of electrons and 4 bonding pairs of electrons,\nThe bonding pairs of electrons will repel each other as much as possible, so the molecule will be tetrahedral.\n\nCH4 is tetrahedral in shape
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b. electrons\n\nI really hope you are trying to answer these first before you put them on here because although we are all certainly willing to help you, you are not going to gain anything from just having the answers given to you.  You really need to try and learn this stuff.
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The Lewis dot structure would be that N in the middle with branches off to oxygen and 2 Fs and then one single electron will be on nitrogen and it is a radical I think. It is very reactive because of this one electron. The electron geometry will be something with sp3 orbital, I am not sure since it only has one electron. I would check up on that. Hope that helps
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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
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1.) ClO2, because the O=Cl=O angle is 90deg whereas O=S=O is linear, 180deg\n2.) HCl, because Cl is more electronegative than Br\n3.) SCl2, because the Cl-S-Cl angle is 90deg, whereas Cl-Be-Cl is linear, 180deg\n4.) AsF3, because As sits at the top of a tripod of F atoms, whereas AsF5 is symmetrical.
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C3H7NO2 \n\nwww.chemfinder.com is a useful resource.  \n\nI hope this helps :)
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[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.
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Covalent single bonds.\nYou'll find carbon - oxygen\noxygen - hydrogen\ncarbon - hydrogen\ncarbon - carbon
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http://www-ec.njit.edu/~skawinsk/chem243/chap11/chap11.htm\nthis may help–near the bottom
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a) 4 "things" attached to central atom and no lone pairs then: sp3-> tetrahedral e- arrangement, tetrahedral shape, 109.5°\nb) 4 "things" attached to central atom one lone pair then: sp3 -> tetrahedral e- arrangement, trigonal pyramidal shape, < 109.5° (about 107°)\nc) 3 "things" attached to central atom one lone pair then: sp2 -> trigonal planar e- arrangement, bent shape, < 120° (guess about 115°?). This is most challanging, try to figure out how many e- in total you have (18), then arrange them around the central atom using usual valances.
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alcl3 is trigonal planar (bond angle 120')\nco2, straight (180')\nh20, bent (~105')\nch4 and ch2cl2 are tetrahedral. (~110')
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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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#10.\n\n3,4 - dimethylhept - 3 - ene\n\nI cant really draw the other ones.\nJust look up your reaction mechanisms.\n\nGood Luck!
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Protons, Neutrons, and electrons