Carbon-carbon bond

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Topic: Carbon-carbon bond

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	Halogen addition reaction - Wikipedia, the free encyclopedia
		As it attacks and forms a bond with one of the carbons, the bond between the first bromine atom and the other carbon atoms breaks, leaving each carbon atom with a halogen substituent.
		When the first bromine atom attacks the carbon-carbon pi-bond, it leaves behind one of its electrons with the other bromine that it was bonded to in Br That other atom is now a negative bromide anion and is attracted to the slight positive charge on the Carbon atoms.
		It forms for an instant a single sigma bond to both of the carbon atoms involved, acquiring a positive charge, which it shares slightly with the two carbon atoms.
	en.wikipedia.org /wiki/Halogen_addition_reaction (328 words)

	Carbon-carbon bond - Wikipedia, the free encyclopedia
		A carbon-carbon bond is a covalent bond between two carbon atoms - a single bond is composed of two electrons, one from each of the two atoms.
		The carbon-carbon single bond is also called a sigma bond and is said to be formed between hybridised orbitals.
		Carbon atoms can also form double bonds (composed of two electrons from each atom, making four in total) or triple bonds (with three electrons from each atom).
	en.wikipedia.org /wiki/Carbon-carbon_bond (230 words)

	Stereoisomers
		In the next two examples, each double bond carbon atom has two different substituent groups and stereoisomerism exists, regardless of whether the two substituents on one carbon are the same as those on the other.
		In the case of hexane, we have an unbranched chain of six carbons which is often written as a linear formula: CH We know this is not strictly true, since the carbon atoms all have a tetrahedral configuration.
		These are also carbon, but the isopropyl group has two carbons (also orange) whereas the propyl group has only one.
	www.cem.msu.edu /~reusch/VirtualText/sterisom.htm (2179 words)

	Covalent bond - Wikipedia, the free encyclopedia
		Covalently bonded hydrogen and carbon in a molecule of methane.
		Pure covalent bonds (which are usually non-soluble, are electrically non-conductive, and tend to exist as individual molecules), and ionic bonds (which are soluble, are electrically conductive when molten or in solution, and, in general, tend to exist in a crystalline form) are on two opposite ends of the spectrum and have different properties.
		Bond order is a term that describes the number of pairs of electrons shared between atoms forming a covalent bond.
	en.wikipedia.org /wiki/Covalent_bond (1258 words)

	Bond dissociation energy (Organic chemistry) - Wikibooks
		However, a carbon-carbon double bond is not twice as strong as a single one, it is only half again stronger.
		All chemical bonds need an input of energy to be broken, as bonds allow a lower energy state for the component atoms.
		For stronger bonds, bond dissociation energy is higher as more energy is needed to break the bond.
	en.wikibooks.org /wiki/Bond_dissociation_energy_(Organic_chemistry) (132 words)

	Chemical Reactivity
		As a covalent bond begins to form between the nucleophile and the carbon, the carbon halogen bond weakens and stretches, the halogen atom eventually leaving as an anion.
		The strongest of the carbon-halogen covalent bonds is that to fluorine.
		The carbon-chlorine covalent bond is slightly weaker than a carbon-carbon bond, and the bonds to the other halogens are weaker still, the bond to iodine being about 33% weaker.
	www.cem.msu.edu /~reusch/VirtualText4/alhalrx1.htm (2518 words)

	Carbon Bond: University of Utah News Release: June 27, 2001
		Students in organic and biochemistry are taught that the longest common carbon bond is found in diamond, a form of pure carbon.
		While potential applications of such basic research are difficult to predict, Miller said the new kind of carbon bond may be important in efforts to develop nanomaterials,” which are bigger than typical molecules but smaller than the smallest manufactured parts and are being studied for possible use in faster computers, display devices and micromachines.
		Miller said the new type of bond is stable but weak – which means it breaks more easily than bonds in which carbon atoms are closer to each other – and it is conceivable that some chemists might argue it is not a true bond.
	www.utah.edu /unews/releases/releases/01/jun/carbon.html (804 words)

	Carbon
		The carbon-carbon bond distance in carbides is quite short and consitent with a triple bond; the carbide ion is isoelectronic with the diatomic nitrogen molecule and the cyanide ion.
		In the carbon monoxide molecule the atoms are joined by a triple bond and both atoms are sp hybridized.
		In the carbon dioxide molecule, the oxygen atoms are each joined to the carbon atom by double bonds.
	www.uncp.edu /home/mcclurem/ptable/carbon.htm (718 words)

	Discovery of First Six-membered Ring with Carbon-Carbon Triple Bond
		Since carbon-silicon bonds frequently are used to prepare new materials, this is an important discovery for industry.
		To make the ring, comprising two carbon and four silicon atoms--or more precisely, four silylene groups--the carbon-silicon bonds are bent at angles much sharper than they normally would adopt.
		The creation of the ring exemplifies the well-known coupling reactions that form new carbon-silicon bonds.
	www.sdsc.edu /GatherScatter/GSwinter96/gordon6.html (568 words)

	Organic Chemistry
		As you add carbon to a molecule, the empty carbon bonds are filled with hydrogen atoms (or other elements, as we will soon see).
		Since carbon needs 8 electrons to fill its valence shell, it forms 4 bonds with other atoms (each bond consisting of one of carbon's electrons and one of the bonding atom's).
		As you increase the number of bonds between carbon atoms, the number of hydrogen atoms in the molecule decreases (as can be seen in the table above).
	web.jjay.cuny.edu /~acarpi/NSC/10-organic.htm (934 words)

	The Mechanism of Carbon-Carbon Bond Activation in Cationic 6-Alkylcyclohexadienyl Ruthenium Hydride Complexes
		The rates of both carbon-carbon bond activation and dehydrogenation are dependent on the identity and concentration of the base and suppressed in the presence of excess acid.
		The protolytic mechanism for carbon-carbon bond activation is supported by deuterium-labeling studies and by the reactivity of the neutral complexes toward Lewis acids and one-electron oxidants.
		Contrary to expectations, it is the 6-exo-methyl complex and not the stereoisomeric 6-endo-methyl complex that undergoes selective carbon-carbon bond activation under exceptionally mild conditions, quantitatively converting the 6-exo-methyl substituent and the hydride ligand to methane.
	pubs.acs.org /cgi-bin/abstract.cgi/jacsat/2000/122/i12/abs/ja992987e.html (335 words)

	Alkene - Wikipedia, the free encyclopedia
		This is compatible with the idea that the carbon-carbon double bond (in alkenes) is stronger than the carbon-carbon single bond (in alkanes), however, as the majority of the reactions of alkenes involve the rupture of this bond to form two new single bonds.
		hydrocarbons with increasing bond order:Alkanes, alkenes and alkynes.
		Like single covalent bonds, double bonds can be described in terms of overlapping atomic orbitals, except that unlike a single bond (which consist of a single sigma bond), a carbon-carbon double bond consists of one sigma bond and one pi bond.
	en.wikipedia.org /wiki/Olefin (1206 words)

	Answers 9
		Will the carbon-carbon bond(s) be stronger or weaker in the excited state relative to the ground state?
		bond, but leave the carbon-hydrogen bonds largely unaffected.
		Compare the bonding in acetylene to that in the acetylene cation.
	classweb.gmu.edu /sdavis/chem332/set9/answers9.htm (160 words)

	Grignard Synthesis
		A carbon nucleophile would need to have an unshared pair or a bonding pair in which the polarity of the bond was such that the carbon was a strongly negative end of the dipole.
		In the bottom reaction, the depiction of this bond is taken to an ionic extreme in which the electron pair is shown as entirely belonging to the carbon, which emphasizes the carbon's nucleophilic character.
		Making carbon-carbon bonds is the central concern in organic synthesis, so it is important to find other compounds in which a carbon atom serves as a nucleophile.
	chemistry2.csudh.edu /rpendarvis/grignard.html (1716 words)

	lecturenotes4.html
		The carbon-carbon triple bond is not free to rotate, the bond angles are 180 degrees and the shape of the molecule is linear.
		Since the double bond is not free to rotate, when the two carbons have two different substituent groups attached to them different molecules are formed.
		A molecule containing four carbons and one double bond is named butene.
	www.clas.ufl.edu /users/tmullins/BCH3023/lecturenotes4.html (616 words)

	Alkenes and Alkynes Comments
		These bonds are called unsaturated because you can break the double or triple bond by adding a functional group to one or both of the carbon atoms, by an addition reaction, thereby making all of the bonds to the carbon atoms single bonds.
		If the bromonium ion takes a pair of electrons from the Pi bond to form a bond with either carbon atom in the molecule, the result is a three-membered cyclic intermediate wherein the Br+ is bridging the two (formerly doubly bonded) carbon atoms.
		Once all of the carbon bonds are single bonds, you can't add anything else to them, and then they are saturated.
	www.newton.dep.anl.gov /askasci/chem00/chem00260.htm (1102 words)

	Butadiene: A Molecular Mechanics Study
		The bond angles between the carbons in the cis butadiene conformers are strained because of steric interactions between the inner hydrogens on the ends of the molecules.
		The inner carbon-carbon bonds in the gauche-cis molecule are strained somewhat by the t-butyl group which alters some of the bond angles slightly (Table 2).
		The carbon-carbon and hydrogen-carbon bond angles are altered to prevent atoms from bumping.
	chemistry.umeche.maine.edu /Modeling/donmolmech.html (1036 words)

	Carboxylic Acids
		Such a bond would be much less reactive than the double bond of a carbonyl group, so it isn't surprising that the Grignard reagent reacts with carbon dioxide in preference to the carboxylate ion.
		If we have a primary alkyl halide (primary means that the carbon which is bonded to the halogen is bonded to only one other carbon atom, it's other two bonds are to hydrogen), we can react it with sodium cyanide.
		Any carbons beyond the first one are lost in this process, which is one of the few reactions which breaks a carbon-carbon bond.
	chemistry2.csudh.edu /rpendarvis/carbacid.html (1336 words)

	Carbon oxygen multiple bonds and their reactivity
		The carbon oxygen double bond is very versatile and is the cornerstone of the much synthetic chemistry.
		hybridised, the carbon oxygen distance is 1.23Å, compared to 1.33Å for a carbon carbon bond.
		To a first approximation it is similar to a carbon carbon double bond.
	speedy.st-and.ac.uk /~naismith/teaching/lectures/ch1004/topica3.htm (1106 words)

	E/Z Configurations
		Once the priorities of the substituents on the first carbon of the double bond have been determined, the same process is used to determine the priorities of the atoms on the other carbon of the double bond.
		When naming carbon-carbon double bond containing compounds, if there is only one C–C double bond in the molecule that has stereochemistry associated with it, then an E or a Z is placed in front of the name to indicate the configuration of the double bond.
		Since the two atoms directly attached to the double bond carbon are identical, you need to look at the atoms that are attached to these two carbon atoms to determine the higher priority substituent.
	www.rocky.edu /~barbaroj/EZ_Rules/EZ.html (937 words)

	Polymerization reactions
		It is the unpaired electron that "attacks" the carbon carbon double bond, as depicted below, where the free radical is designated with the letter R and the unpaired electron is the dot (a representation consistant with a Lewis dot symbol for such a species).
		The pi bond in this configuration is not as strong as a carbon-carbon sigma bond.
		The produce bonds that form the polymer - and they produce water molecules that are somehow removed from the reaction mixture in the processing of the reaction.
	www.uwm.edu /~tholme/old105/polymerization.htm (548 words)

	Alkynes
		Thus, the hydrogen attached to the carbon-carbon triple bond in ethyne, or in any alkyne where the carbon-carbon triple bond is situated at the end of a carbon chain, is able to separate from the rest of the molecule as a hydrogen ion, so that the alkyne shows acidic properties.
		The carbon-carbon triple bond of the alkynes is formed in the same way as a double bond of the alkenes, by the elimination of atoms or groups from two adjacent carbons.
		The alkynes are the third homologous series of organic compounds of hydrogen and carbon, where there is at least one triple-bond between the atoms in the molecules.
	www.ucc.ie /ucc/depts/chem/dolchem/html/dict/alkynes.html (1641 words)

	Models
		This means that as the molecule increased from a single bond to a double bond, the length between the carbon-carbon bonds became smaller.
		For example, the length of the carbon-carbon single bond was 8.2 cm versus the length of the carbon-carbon double bond which was 7.6cm.
		As the bond number between the molecule increased the lengths of the bonds decreased.
	filebox.vt.edu /users/mladley/Models.html (873 words)

	Alkanes and Cycloalkanes
		Looking along the bond between the first and second carbon atom, sketch the arrangement that you would expect to be the most stable.
		Looking along the carbon-carbon bond, arrange the molecule so that it places the atoms as far apart as possible.
		Now holding the back carbon in place, rotate the front carbon 60º so that the hydrogen atoms on the front carbon “cover” the hydrogens on the back carbon.
	www.uwlax.edu /faculty/koster/modellab.htm (534 words)

	AS unit chains and rings alkenes page
		The carbon-carbon double bond has the effect of stopping rotation of the groups attached to the carbon atoms (see bonding section later on).
		With four or more carbon atoms present the position of the double bond becomes important.
		A prefix derived from the number of carbon atoms present (see naming alkanes in the alkanes page) is capped with the suffix _ene.
	www.rjclarkson.demon.co.uk /candr/alkenes.htm (534 words)

	Example 15
		The degree of unsaturation of 2 both hints at an alkyne, although the carbon-carbon triple bond stretch 2260-2100 is not seen.
		The C-H stretching vibrations are all under 3000, indicating that there are no hydrogens on a carbon-carbon double bond or on a carbon-carbon triple bond - it is possible that the compound is a internal alkyne.
		The C-H stretch is not seen in the IR because it is not a terminal alkyne (and therefore does not have a C-H on the triple-bonded carbon.
	orgchem.colorado.edu /hndbksupport/specttutor/ex15.html (208 words)

	Alkene Molecule Geometry
		Since a double bond is present and each carbon is attached to 3 atoms (2 H and 1 C), the geometry is trigonal planar.
		Carbons #1 and 2 both have only 3 other atoms attached and one double bond, therefore both are centers of trigonal planar geometry.
		Carbon # 3 has 4 other atoms attached and all single bonds, therefore it is the center of a tetrahedron.
	www.elmhurst.edu /~chm/vchembook/209alkenes.html (238 words)

	prob3-10.html
		The conjugated bonds consist of one of the pi bonds of the carbon-carbon triple bond (green atoms), the carbon-carbon double bond (blue atoms), and the carbon-oxygen double bond (red atoms).
		The carbon-carbon double bond (green atoms) is conjugated with one of the pi bonds ot the carbon-nitrogen triple bond (blue atoms).
		The carbon-carbon double bond (blue atoms) is not conjugated with the carbon-oxygen double bond (red atoms) because the green C which separates them does not have a p orbital.
	www.du.edu /~jhornbac/organic/prob3-10.html (153 words)

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