What hybrid orbitals are used in the following species?
823206
CO-sp\nCO2-sp2\nCN-sp
231898
There are a few isomers possible.\n\nEssentially there are two C's double-bonded, with either 2H's off one C and 2Br's off the other C.\nOr 1H and 1Br off each C
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
283215
[Cu(NH3)4]SO4*H2O (s) + 2HCl(aq) --->\n\nCu(NH3)4 +2 (aq) + H2SO4(aq) + H2O(l) + 2Cl-(aq)
927770
1. NaCN\n2. NO2\n3. CuCl2\n4. NaC2H3O2 \n5. F2\n6. bonding involves transfer of electrons between atoms
98049
Some of the matals have multiple oxidation states and these must be indicated in the names:\nAmericurium (III) fluoride\nIndium (III) fluoride\nBarium permanganate\nNeodymium (III) iodide\nCadmium sulfite\nSilicon tetrathiocyanate\nVanadium (III) fluoride\nIron (III) dichromate\nGold (I) cyanide\nBarium bromate\nMagnesium molybdate\nPlutonium (III) bromide\nSamarium (III) sulfate\nTungsten (II) iodide\nPotassium borate
880509
Hey, Blond fuss?  Good luck if U can't find help @ this late hour. Keep working on it.  Something from what U learned so far must b in your head - find it. No one else working on this problem awake?\n  I'm tired (12:35 a.m. here @ UMAss Amherst).  Had 1st-yr Chem 100 in 1978, not Chem 1111 !! Barely remember orbitals.  U do have books there, don't U?   Library maybe not open now as ours is.    \n Aces 2 computer. So U have awhile 2 figure it out.  Good luck.
401509
I don't know that question.\n\nI can tell you that it's an octahedral complex. The two isomers would be CIS (Both chlorides adjacent to each other) and TRANS (both chlorines opposite each other)
435560
you determine the hybridization of a particular atom by seeing how many electron pairs there are around a particular atom.  For example, if you draw the structure for ethylene (C2H4) you get \n\nH3C=CH3\n\nthis means that there are 3 electron pairs around both C atoms and they are both show sp2 hybridization.  \n\nIn another example, d2sp3 hybridization, you will have 6 electron pairs around the d2sp3 hybridized atom.  \nIn dsp3 hybridization, you will have 5\nin sp3 hybridization, you will have 4, etc...
534537
1 Hydrogen 2 Helium 3 Lithium 4 Beryllium 5 Boron. 6 Carbon 7 Nitrogen 8 Oxygen 9 Fluorine 10 Neon
231884
There needs to be something you are binding oxygen to.  Oxygen itself will not have any hybridized orbitals. With H2O for example there would be four sp3 hybrid orbitals. two of the orbital will have hydrogen bound to it and the other two will be taken up by the 2 lone pairs.  Once the orbitals are hybridized to sp3 there is no place left to put any electrons in a p orbital since they were all hybridized to sp3.
332147
Those ions do follow Hund's rule, though. The d orbital looks like this:\n\n\n_________ ___________\n\n__**_______ ____*____ ___*____\n\nThe electrons are only paired when absolutely necessary.
56480
Hybridisation (Commonwealth English) or hybridization (American English) is the mixing of atomic orbitals belonging to a same electron shell to form new orbitals suitable for the qualitative description of atomic bonding properties. Hybridized orbitals are very useful for rationalizing in hand waving discussions the shape of molecular orbitals for molecules made of atoms of the groups 2,3,4 of the periodic families of elements. On the other hand, groups 1,5,6 and 7 in the periodic table do not hybridise, i.e. this approach is in that case not useful. Hybridisation is an integral part of the valence shell electron-pair repulsion (VSEPR) theory.\n\nAcid: acid is a molecule or ion that is able to give up a proton (H+ ion) to a base, or accept an unshared pair of electrons from a base. An acid reacts with a base in a neutralization reaction to form a salt.\n\nBase:Base is a chemical compound that absorbs hydronium ions when dissolved in water (a proton acceptor).\n\nSalt:Salt is a term used for ionic compounds composed of positively charged cations and negatively charged anions, so that the product is neutral and without a net charge. These ions can be inorganic (Cl-) as well as organic (CH3-COO-) and monoatomic (F-) as well as polyatomic ions (SO42-).\n\nFor further queries email me:trust_amplifier@yahoo.com
929337
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.
142302
Resonance in the pi-electron orbitals.
466437
interesting answer above.\n\nCarbon has 4 valance electrons which because of the relatively small size of the atom can move about and create all sorts of hybrid orbitals and molecular bonding orbitals allowing it to suit the bonding needs of many other atoms, thus making many varied combinations.\n\nIt is also in the middle range of electronegitivities therefore resisting in most situations becoming an ion.
712728
choose the noble gas that comes before the element.   in Mn(2+)'s case, that's Ar\n\nwrite the noble gas down in brackets, and continue on with the electron config. as normal\n\n[Ar}4s23d3\n\nFor O(2-), it turns into Neon so it would just be [Ne]