All carbon-carbon bonds in a hydrocarbon are?
816025
b) the electronegativities of both atoms involved in the bond are identical.
244326
Saturated means that all the Carbon-Hydrogen bonds are 'single' bonds.  Thus, the previously double and triple bonded carbon-hydrogen atoms cannot not take anymore H atoms...they are saturated with them!\n\nStructure is very simple. They are pretty much straight floppy chains.  Think of a shoelace flopping around.\n\nSaturated hydrocarbons are in the 'ane' family of names.  Pentane, Octane, Butane, etc.\n\nProperties:  One great property is that they flop around a lot.  This makes them pass through tight spaces easier, and contribute to clogging far less than unsaturated hydrocarbons (double and triple bonds are rigid, and thus not floppy).  This floppyness is especially important for arteries.  Eat more unsaturated hydrocarbons (fats), get more clogged arteries.  Eat saturated (floppy), and they don't get stuck.\n\nUses:  One use is gasoline (Octane).  Straight-chain (saturated) burns more efficiently.\n\nHope this helps.
950410
Mainly H-bonding (intermolecular forces)
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Carbon (C), Hydrogen (H), and Oxygen (O)
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benzene has 6C and 6H.it has 3 double bonds and three single bonds.It has a cyclic hexagonal shape. it forms aromatic compounds when attached to other hydrocarbons. Benzene is also carcinogenic(causes cancer)
136157
Mostly because of its sp3 hybridization - that is, the fact that 4 atoms or molecules can bond with great stability to the carbon atom. For example, methane (CH4) is the simplest of the carbon compounds. But now, replace any of those H's with almost any other kind of molecule and you get the meat & potatoes of what organic chemistry is all about.
855406
alkanes are sp3 hybridized and tetrahedral. (there are single bonds between the carbons)\nalkenes are sp2 hybridized and triangular planar. (there is at least one double bond in the carbon chain)\nalkynes are sp hybridized and linear (there is at least one triple bond)\n\nwhether or not they are polar depends on their substituents. if they only have hydrogen atoms attached they will be nonpolar.
463321
Alkanes have a C-C single sigma bond which is very strong and has a high bond dissociation energy to be broken. For this reason, alkanes only undergo free radical substitution reactions i.e they are only capable of substituting one or more of their H atoms with another atom, but they cannot undergo a complete change of structure, making them relatively inert as compared to alkenes.
1037366
Ethene, C(2)H(4) contains a double bond between Carbons and is relatively unstable compared to CH(4), which contains only single bonds.  A brute force method would be to apply heat (raising the temperature) to rupture the double bond to produce the more stable methane.  As a practical consequence, however, recall that methane, as a gas, is combustible.
47652
Because of its valence shell carbon atoms always have 4 bonds. In addition to this carbon atoms are unique in thier ability to form strong covalent bonds to each other while at the same time bonding atoms of other nonmetals strongly.
70470
Methane is a very easily made hydrocarbon.  With abundant carbon and hydrogen in space, and plenty of solar radiation, the reaction is not difficult.  Many hydrocarbons have been found in interstellar clouds.
1112022
An alkene, or olefine, in organic chemistry is an unsaturated hydrocarbon containing at least one carbon to carbon double bond. The simplest alkenes, with only one double bond, form a homologous series with general formula CnH2n.\n\nThe simplest alkene is ethylene (C2H4), which has the International Union of Pure and Applied Chemistry (IUPAC) name ethene. Alkenes are also called olefins (an archaic synonym, widely used in the petrochemical industry) or vinyl compounds.\n\nShape of alkenes\n\nAs predicted by the VSEPR model of electron pair replusion, the molecular geometry of alkenes includes bond angles about each carbon in a double bond of about 120°. The angle may vary because of steric strain introduced by nonbonded interactions created by functional groups attached to the carbons of the double bond. For example, the C-C-C bond angle in propylene is 123.9°. The alkene double bond is stronger than a single covalent bond and also shorter with an average bond length of 133 picometres.\n\n\nMolecular geometry\n\nLike single covalent bonds, double bonds can be described in terms of overlapping atomic orbitals, except that unlike a single bond (which consists of a single sigma bond), a carbon-carbon double bond consists of one sigma bond and one pi bond.\n\nEach carbon of the double bond uses its three sp2 hybrid orbitals to form sigma bonds to three atoms. The unhybridized 2p atomic orbitals, which lie perpendicular to the plane created by the axes of the three sp2 hybrid orbitals, combine to form the pi bond.\ncis-2-Butylene\nEnlarge\ncis-2-Butylene\ntrans-2-Butylene\nEnlarge\ntrans-2-Butylene\n\nBecause it requires a large amount of energy to break a pi bond (264 kJ/mol in ethylene), rotation about the carbon-carbon double bond is very difficult and therefore severely restricted. As a consequence substituted alkenes may exist as one of two isomers called a cis isomer and a trans isomer. For example, in cis-2-butylene the two methyl substituents face the same side of the double bond and in trans-2-butylene they face the opposite side.\n\nIt is certainly not impossible to twist a double bond. In fact, a 90° twist requires an energy approximately equal to half the strength of a pi bond. The misalignment of the p orbitals is less than expected because pyridalization takes place. trans-Cyclooctene is a stable strained alkene and the orbital misalignment is only 19° with a dihedral angle of 137° (normal 120°) and a degree of pyramidalization of 18°. This explains the dipole moment of 0.8 D for this compound (cis-isomer 0.4 D) where a value of zero is expected.[1] The trans isomer of cycloheptene is only stable at low temperatures.
712626
Yes, as long as they are separated...eg\nCH2=CH-C---CH (where ---is a triple bond, cannot type that here), which is vinyl acetylene, a stable but v reactive compound.\nBut CH2=C---CH is obviously impossible because the central C would have five bonds, whereas C can only have four.
51155
bond energies: CH 413, CC 346, CO single bond 358, OH 463, CO triple bond 1072. CO double bond 732. Add up all the bond energies on the left side of the arrow, then add up all the bond energies on the right and subtract one from the other.  Be sure to multiply the bond energy of each type with how many of each type you have.
126756
Organic compounds are ones containing carbon.  Methane is nothing more than a single carbon atom surrounded by four hydrogen atoms, making the molecule very much reduced.  The methane there can be used to react with other reagents to build larger organic molecules with methane as a building block.
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!
650823
Carbon, Hydrogen, and Oxygen.