in a organic molecule, a sulfur atom will normally form how many bonds?
541302
Up to six, depending on the available partners and the state of oxidation.\n\nSulphur can behave like the oxygen homologue it is and form two covalent bonds or one double bond to carbon.\n\nIn combination with electronegative atoms (F, O, Cl) sulphur can exhibit a range of oxidation states and still form single bonds with carbon.
3700
Carbon is "special" for organic chemistry because of its ability to form molecules of arbitrary numbers of carbon atoms and other elements, primarily hydrogen, nitrogen and oxygen. Carbon can have up to four single bonds. Besides, it can have double or triple bonds, allowing for even more variations than its heavier homologue Silicon.\n\nOne of my old chemistry professors gave three "fundamental theorems" for organic chemistry:\n\n- Carbon always has four bonds\n- Nucleophile will react with electrophile (slightly  negative ends with slightly positive ones)\n- Whenever the opportunity to form a ring of five or six atoms offers itself during a reaction, it will be taken.\n\nBetter than 95% of organic chemistry can be deduced using these rules.
285141
All moleciles do not contain multiple bonds.\n\nIonic bonds are usually single bonds.\n\nMore than one bond may be indifferent manners.\nIn case of H2O oxygen forms one bond with each hydrogen and thus there are two bonds.\n\nIn case of O2 molecule the two oxygen atoms form a double bond with each other.\n\nMore than one bond (as H2O) or a multiple bond (as O2, N2, H2C=CH2) depend on the valency number of the atoms.
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.
179528
1 mole of a substance means 6.023 x 10^23 molecules..so thr will be 6.023 x 10^23 no of carbon disulphide molecules. now each CS2 molecule has one carbon and 2 sulphur atoms  .so there will be 6.023 x 10^23 atoms of carbon and 2 x 6.023 x 10^23 sulphur atoms
965017
You need to know the number of valence electrons.  Carbon, for example, would want to pair with 4 other atoms.  If there were fewer atoms attached as in CH2O (only 3 attached to the carbon) then one of the atoms must be double bonded.  In this case it is the oxygen that would have the double bond.  You could deduce the approximate shape from the number of bonds.  It would be slightly distorted by the slight negative polarity of the oxygen atom.  Shape of a molecule is a complicated issue that I glossed over.
838159
Sigma corresponds with "s" orbitals.  Pi corresponds with "p" orbitals.  We know that 2 electrons fill up the s orbitals.  We know that it takes 6 electrons to fill up the p orbitals.  Carbon has four bonding sites, so it could theoretically have four bonds.  That is 1 sigma bond and 3 pi bonds.  Bottom line is to remember that it corresponds with orbitals.  Hope this helps!
283736
The octet rule refers to Lewis dot diagrams and how electrons are arranged in molecules. During covalent bonding, atoms have eight electrons in their orbit, whether or not they are shared with another atom. An example of the octet rule would be oxygen atoms (each with 6 electrons) in a diatomic oxygen molecule sharing a total of four electrons between each other while keeping four electrons to themselves. Of course, the octet rule does not apply to hydrogen, which can only hold two electrons. The octet rule also applies to ionic bonding, where the anion (the negatively charged ion) gains a number of electrons to  have a total of eight electrons in its orbit.
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.
852150
My OChem teacher explains it this way, looking at carbon.\n\nCarbon has four valence electrons, 1 2s orbital and  3 2p orbitals. If you look at them separately, you see that the first two electrons go into 2s because it's lower energy, the next one goes into 2px, and the last into 2py. And we see that carbon forms two bonds. There's a technical term for this: WRONG! :)\n\nSo, imagine you have 4 guests in your house, and you have 1 tomato and 3 pieces of celery. How do you make sure that everyone gets *exactly* the same thing?\n\nYou have to blend them all together. You would put your ingredients, tomato (1 of them) and celery (3 of them), in a blender, pour into four glasses, serve chilled.\n\nSo with carbon, we take our s (1 of them) and our p (3 of them), blend them together and we have 4 s1p3 (ie. sp3) orbitals. 4 single bonds, everything even.\n\nWe could also take s (1 of them) and p (2 of them), and we'll have 3 s1p2 (sp2) orbitals. This is the case with ethylene -- the sp2 orbitals make 3 sigma bonds (2 for the single, 1 for the double), and the un-blended p orbital makes the pi bond.\n\nLikewise, sp is 1 s and 1 p orbital (s1p1).\n\nHope this helps. I've found this subject troublesome, too.
55267
There are lots of reasons why there are large number of organic compounds .I’m giving U few of them.\nCatenation: The tendency of an element to form chains of identical atoms is called catenation. This tendency is observed in the case of non-metals showing covalency of two or more. However, this property is maximum in carbon as it can combine with other carbon atoms by single, double or triple covalent bonds. The bonding can be extended to form long open chain (straight or branched) or closed ones. Catenation property depends upon the value of bond energy which is maximum in the case of carbon. \nBond:                                         C-C    Si-Si       S-S     P-P     N-N    O-O\nBond energy:                              83        54         54        50      39        35          (approximately)\n(kcal/mol)\n The stability or the strength of the bond decreases as the bond energy decreases. Hence, the tendency of catenation decreases in the following manner; C> Si ~ S > P > N > O\nTendency to combine with other non-metals: Carbon has the ability to form strong covalent bonds with many other atoms such as H, O, S, N, Cl, Br, I, etc. The C-C bond energy is approximately equals to the magnitude of bond energies between carbon and various other atoms.\nBond                                          C-C         C-H       C-O      C-Cl      C-N       C-Br\nBond energy                               83.0         97.0       86.0      81.0       73.0       68.0           (approximately)\n(kcal/mol)\nIsomerism is one of the reason also.
43823
Carbon, with 4 electrons in its outer shell is the most versatile element. It can form single, double, and triple bonds with a wide variety of elements, creating just about every living thing we see. Carbon is known to form at least 10 million different compounds. Elements, such as Nitrogen, with 5 electrons in the outer shell, and Boron with 3, are much more limited.
178276
Gain one/two electron(s):\n\nIf an atom or ion acquires another electron in a chemical reaction, it has gained an electron.  ditto for two electrons.\nExample: S has 16 electrons.  If it gains one electron it becomes a S- ion.  If it gains two electrons, it becomes a S-2 ion.\n\nSteal one/two electrons:\nIf an atom or ion looses an electron in a chemical reaction, it had to go somewhere.  That "somewhere" will be to another atom/ion.  So, the receiving atom/ion could be said to have stolen the electron.  Same goes for reactions involving two electrons.\nExample: Na reacts with Cl to produce NaCl.  Cl "steals" an electron from Na, creating Na+ and a Cl- ions.\n\n"Never ever react electron"\nI have never ever heard this phrase.  Maybe it refers to a species (atom or ion) that does not participate in the reaction.  It's valence electron(s) would not react.
976900
Chemical bonds form when electrons are shared, like in covalent bonds.  The atoms in the bond share a certain number of electrons between them usually so they both have a complete octet of electrons.  Another type of bond is ionic.  This is when one atom completely pulls off an electron from the other atom.  This results in a negative charge on the taker and a positive charge on the giver.  The bond is formed by the electromagnetic force acting between these two dissimilar charges.
884142
It is just Cl single bonded to each of the O's.  Ther are 26 available electrons (7+(6*3)+1(because it is negative)) and to fill their valence shells 32 are needed which means 6 are shared which means there are 3 bonds and since all of the atoms must be bonded there must be 3 single bonds. There are 10 lone pairs I think(you can check)
877256
these electrons are the ones that participate in chemical reactions, ie formation of bonds
801251
A single sigma bond can form between any two atoms.  It is formed by the sharing of 2 electrons directly along the line between the two atoms.  A sigma bond is defined as the bond that exists DIRECTLY  BETWEEN the two atoms along the atomic axis.  Only one sigma bond can exist between any two atoms.  Sigma bonds can be found in all types of compounds, organic, inorganic, organometallic, etc.\nThey are the most common type of bonds found in molecules.