What kind of bond does carbon form and how many of them can one C form?(biochem?
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One question at a time please!\n\nCarbon forms Covalent bonds.\n\n1 molecule of Carbon can form 4 bonds.\n\nLipids are formed from Carbon, Hydrogen, and Oxygen and consist of fatty acids, and esters, and glycerols.\n\nOkay, Organic vs. Inorganic Here are some of the most educated opinions on that subject that I have ever encountered:\n\n Ask A Scientist\nChemistry Archive  \n\nhttp://www.newton.dep.anl.gov/askasci/chem99/chem99286.htm\n\n--------------------------------------------------------------------------------\n\nOrganic / Inorganic\n\nQuestion:\nI teach sophomores an introductory biology course.  When I cover the biochemistry section the terms organic and inorganic come up.\nI am not satisfied with the simplistic statement that organic chemicals are ones that contain carbon since it does not account for carbon dioxide being an inorganic. Is there a definition of 'organic chemical' which accounts for all\nor most molecules?\n doug happ\n \nAnswer 1:\n   Given the existence of hemoglobin, "zinc fingers" in some enzymes, and buckyballs, I'd guess not.\n christopher grayce\n\nAnswer 2:\nConsidering the number of carbon containing molecules that ARE considered to be organic relative to the number that are NOT, the rule that an organic molecule is one that contains carbon,  works VERY well. The "exceptions" might serve as a lead-in to a discussion of the use of rules, such as classifying molecules as organic or inorganic, as a contrived convenience.  They are helpful for most cases.  In the cases\nwhere the rules don't work well we have to be able to turn to other tools, such as an understanding of chemical bonds or molecular orbitals so we can concentrate on the characteristic of interest -- which is very rarely\nwhether the molecule is organic or more often things like reactivity. You're at the leading edge of helping these students think for themselves\nin a field where they probably feel unsure of themselves! It sounds like you have some inquiring students there and some active\ndiscussions.  May you have many more!\nGreg\n\nAnswer 3:  An interesting question.\nI believe that "organic" vs. "inorganic" originally stemmed from the ancient idea that compounds could be divided into two categories; those isolated from plants and animals (organic) and those extracted from minerals and ore (inorganic)\n[source: Bodner and Pardue, Chemistry: An Experimental Science, 1993].\n \nAs a working definition, now we think of organic chemistry as primarily being the chemistry of carbon-containing compounds. Most carbon-containing compounds have one or more of the\nfollowing: H,N,O,S,P. Some authors describe organic chemistry as the study of compounds that contain carbon and hydrogen. By this definition, CO2 would be "inorganic." But I would\nlike to stress that in fact there is no general agreement on such semantics, and I'd bet that a lot of chemists consider CO2 to be "organic" because it contains C and O.\nTopper
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)
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In a covalent bond, both species provide 1 electron to form the 2 electron bond.\n\nIn a complex, both bonding electrons are donated from a single atom. Complexation refers to the formation of complex bonds.
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B and C.  Molecules with H bonded to N, O, or F can form hydrogen bonds.  Others cannot.  In molecules A and D, all the H's are bonded to C's, so they are not capable of hydrogen bonding.  In molecules B and C, there is an O-H bond, so they are capable of hydrogen bonding.\n\nAlthough all four structural formulas have H written next to O, that doesn't necessarily indicate that there is an O-H bond.\n\nMolecule A is an ether, so the oxygen is between two carbons.  Specifically, it's dimethyl ether, so there's a methyl group (CH3) on each side of the oxygen.  You can find a picture of it here: http://en.wikipedia.org/wiki/Dimethyl_ether\nThe oxygen in an ether doesn't allow for hydrogen bonding because none of the hydrogens are attached to it.\n\nMolecule B a carboxylic acid.  Specifically, it's acetic acid.  It consists of a methyl group attached to a carboxyl group, which is a carbon double bonded to an oxygen and also single bonded to an OH group.  The O-H bond in the carboxyl group allows the molecule to form hydrogen bonds.\nYou can find a picture of its structure here:\nhttp://en.wikipedia.org/wiki/Acetic_acid\n\nMolecule C is ethanol.  It consists of a methyl group, a methylene group (CH2), and an OH groupl.  Like with carboxylic acid, the O-H bond is capable of hydrogen bonding.\nHere's it's structure:\nhttp://en.wikipedia.org/wiki/Ethanol\n\nMolecule D might be a bit misleading at first glance, but it's actually an aldehyde, specifically acetaldehyde.  It consists of a methyl group bonded to a second carbon that is bonded to a hydrogen and double-bonded to an oxygen.  That last hydrogen is attached to the carbon, rather than the oxygen, so it can't do hydrogen bonding.  Here's a picture of it's structure:\nhttp://en.wikipedia.org/wiki/Acetylaldehyde
892646
first of all carbon is not an organic compound it is an element. and different compounds made from carbon are included in class of organic compounds.\n\ncarbon has got atomic number 6. so its electronic configuration will be 1s2,2s2,2p2. so it contains 4 electrons in its outermost orbit, we know that there should be 8 electrons to complete the octet and make the element stable, so carbon can either gain 4 electrons or lose 4 electrons to become stable, but both requires very high amount of energy.\n\nso it goes for sharing of electrons. it has the special property of catenation, ie carbon-carbon long chain formation. no other element has such property, so carbon itself has forms such high number of compounds which not even formed by rest all elements together. so it has been given special branch of chemistry called organic chemistry while rest all elements are included in inorganic chemistry. so its versatile
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.
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okay, if we draw the basic structure of H2CO, we know that the Carbon is in the center. That's usually how it is.\nCarbon likes to have four bonds because of it's position on the periodic table.\n\nNow, first, let's count how many electrons are in the H2CO molecule.\nH=1, 2(1) =2\nC = 4\nO = 6\ntotal = 12\nSo let's draw carbon in the middle, bonded to H, H, and O\nH-C-H\n....O\n(That should be like a t-shape).\nSo far we've used 6 electrons (we have 3 bonds), so 12-6 leaves us with 6 electrons.\nlet's finish the carbon quartet, so now carbon has 3 bonds and one pair of electrons\n6-2=4 electrons left\nlet's put the four electrons around O....\nbut that only puts a total of 6 electrons on O (4 in lone pairs and 2 in bonds) and Oxygen wants to have a quartet.\n\nRemember that pair of electrons that we put on carbon?\nLet's make a double bond between O and C.\n\nso now the final diagram looks like\nH2-C=O\nand there are four (two pairs) of lone electrons on Oxygen\nSo to answer your question\nthere are two bonds to oxygen and two bonds to H, a total of four bonds.\n2(4)=8\nCarbon is using all 8 electrons to bond.
50031
There r 20 amino acid,by combination of these amino acids diffirent proteins r formed.simple structure of a amino acidis like a central carbon atom(known as alpha carbon)to which a carboxilic group(-COOH) and a amine group(-NH2) and a side chain(-R group) attached,all amino acid have same structure but they differ to each other by side chain(-R group).
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each sulfur adds 6 electrons, each carbon 4 - that's a total of 20 electrons.  Logically this puts a double bond between the carbons and double bonds between each carbon and one of the sulfurs.  S=C=C=S\nH2O2 has single bonds between the oxygens and single bonds between each oxygen with one of the H. H-O-O-H\nfor the thiocyanate ion this should be a 1- charge - this means the S is double bonded to the C which is double bonded to the N (S=C=N) there is a total of 16 electrons.  However - I really think the N should have a triple bond - this means that S will be singly bonded to the C and a triple obnd between the C and N.  Cannot really show this but go the the chemistry.mcmaster link below and check it out.
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IF it is of a disaccharide, both being 6 carbon sugars, such as in the case of sucrose (i thinking glucose and mannose? or gluc and fruc?) and their are 12 Carbons, than essentially 12 CO2 molecules, thus D would be the answer.
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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.
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Becasue if you take the constituent atoms of a carbohydrate molecule and break them down, you could put them together to form water and carbon.\n\nFor example, sucrose -- C12H22O11 -- could be broken down into 12 atoms of carbon and 11 molecules of water.
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Enthalpy change of formation of 1 mole of C2H2 is the energy change when 1 mole of it is formed from its elements (2C(s) and H2(g)) in their standard states.\n\n2C(s) + H2(g) ---> C2H2(g)\n\nenthalpy of formation of C2H2= \nenergy absorbed to break H-H bond \n+ \nenergy released to form 1 C=C bond and 4 C-H bonds \n= 610 + 4(-410)\n= -1030 KJ/mol\n(If you are taking A level Chemistry, refer to your data booklet for these values under the section of bond energies)\n\nHope this helps.
451415
i think it is a polar covalent bond\nI used to remember why but I'm not in Chemistry anymore...\nHeres a website.. Look at Example #3\nhttp://users.rcn.com/jkimball.ma.ultranet/BiologyPages/E/Electronegativity.html#covalent_bond\nAnd another http://academic.brooklyn.cuny.edu/biology/bio4fv/page/polar_c.htm\nhope its not too late
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These chemicals have one thing in common, carbon atoms. Carbon atoms link in chains, like C-C-C. Carbon atoms "like" to have 4 bonds with other atoms. In each of the chemicals you named, the carbons are all single or double-bonded to other carbons; the other bonds are with hydrogen atoms.\n\nThese are the simplest "organic chemicals". It used to be thought that "organic" chemicals were produced by living things. Now they're known to be produced in outer space as well. So there are many possible "origins" for these molecules in that sense.\n\nMethane molecules have only one carbon atom; octane has 8. So you might say that all of these molecules have their origin in carbon atoms sharing bonds with other carbons.
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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.
311037
It's an organic acid having a\n\nO=C-OH group; the H of the -OH group is the proton source, \n\nthus: -O(-) H(+).\n\np.s. In aqueous solution. The fourth carbon bond is not drawn.