explain the intertness of alkanes in term of strength of bonding.?
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.
953050
If the difference in the electronegativity between the two elements is less than 1.67, the bond will be covalent.\n\nNote: As to the statement that electronegative atoms don't form covalent bonds, that's nonsense.  ALL atoms are electronegative to some extent.  Just go look up the electronegativity series in any general chem. text.  Or check out this:\nhttp://dbhs.wvusd.k12.ca.us/webdocs/Bonding/Electroneg-Bond-Polarity.html
309511
You are not breaking a double bond or a triple bond, you are breaking a pi-bond in both addition to alkenes and alkynes.\nThe rate of reaction with a nucleophile depends a lot on which nucleophile and which alkene or alkyne. The product of a nucleophilic addition produces a carbocation attached by a single bond in the case of alkenes, and by a double bond in the case of alkynes. The vinyl cation from addition to alkynes is much higher in energy than the alkane cation from addition to the corresponding alkene, so in that sense, addition would seem to be slower to an alkyne. However, there is evidence to suggest some sort of cyclic addition in the case of alkynes, which complicates the picture. Add to that the effect of solvent and other reaction conditions, and it should be clear that there is no simple answer to your question.
1047674
Intermolecular forces (vander waals, hydrogen bonds), are very much weaker than covalent or ionic bonds\nyou see, when we evaporate water in its boiling points(or other liquid), we break the intermolecular forces (in water's case, hydrogen bonds), but the heat still cannot break up covalent H-O bonds, so the chemical formula of water vapour is still H2O but with no intermolecular forces
1160360
by molecular bonds.  covalent and ionic.
8956
The similarities are\n1. Both are unsaturated.\n2. Both have pi bonds which overlap laterally.\n3. Both are susceptible to electrophilic attack.\n4. Bond length of both alkene and alkyne is less than that of alkane.\n\nThe differences are\n1. Alkene has single pi bond whereas, alkyne has 2 pi bonds.\n2. The C-C bond distance is less in alkyne compared to alkene.\n3. Carbon atoms are sp2 hybridized in alkene. On the other hand, carbon atoms involved in the triple bond in alkyne is sp hybridized.
1107805
study on intermolecular particals and there behavior
1161649
Hydrocarbons are good nonpolar molecules.
702840
Of the choices you listed above, then Alkane is the answer.  There are other compounds which fit this description, for example the cycloalkanes which is a sub-group of alkanes.\n\nThese are also called aliphatic compounds and saturated hydrocarbons.
965934
Because of the amount of energy it takes to break the bonds of the molecules in the liquid. If one liquid has a substance that has strong bonds, it will have a higher bowling point than a substance with weak bonds. (bond strength has to do with if it's a covalent or ionic bond, if its a single or double bond, and the number of bonds.)
998521
that is wrong!!!!\nthe values should have been the other way round!\nnow look:since ethane is a parafin we cannot discuss its prop\ncome to acetone. the central carbon is double bonded to an oxygen atom\nnow when an electrophile comes to this oxygen the bond attains polar character wth the oxygen having partial negative charge(grearter electronegativity), and the carbon having partial positive charge\nnow obviously the electrophile will go towards this oxygen atom, showin its basic character\nlook at the other way(the one described above)\nwhen the oxygen atom reduces the electron cloud density, the carbon atom is more strogly attached to the hydrogens which means that it cannot be released easily which once agains shows its basic character\nhence the values should have been the othr way round
163434
NaCl, the bonding is stronger
1008726
Strong Love!\n\nIn other words, it's a covalent bond because sharing of electrons takes place in these elements when they combine with each other.
625615
the answer is a, the number of outer shell electrons it can gain or lose.\n\nthia is because that outer electrons are the ones the define the atom in terms of bonding. \nmass nubmer and atomic number dont matter much [as lower level chemistry] for bonds. we know that the number of molecules it can form is infinite, and inner shells dont matter, leaving us wiht (A), the only right answer
1153182
Heats of Combustion are quoted in kJ/mole. However, the amount of Carbon and Hydrogen that you have in bigger molecules is larger for 1 mole. \n\nHeat is released because Carbon - Oxygen and Hydrogen - Oxygen bonds are more stable than  Carbon - Carbon or Carbon - Hydrogen bonds. When you burn an alkane, you break the Carbon - Carbon and Carbon - Hydrogen bonds and form Carbon - Oxygen and Hydrogen - Oxygen bonds. A way of thinking of this is that because these  Carbon - Oxygen and Hydrogen - Oxygen bonds are more stable, less energy is required to hold the pieces together. The energy you no longer need is released as heat.\n\nSo why release more when you have longer chains? 1 mole is a set number of molecules, but the longer the carbon chain is, the more Carbon and Hydrogen you have. \n\nAs a result, more Carbon - Carbon and Carbon - Hydrogen bonds are being converted to Carbon - Oxygen and Hydrogen - Oxygen bonds. Result, you have to get rid of more heat.\n\nSo the Heat of Combustion becomes more negative, that is to say you release more heat to the surroundings.\n\nAny help?
1068373
If you know you're dealing with an organic compound, you take the formula weight and divide by 12.  This gives the number of carbon atoms.  You look at the remainder and determine if it could be the number of hydrogen atoms.  Alkanes have 2n + 2 hydrogen atoms (where n = number of carbons).  Alkenes have 2n and alkynes have 2n - 1.
950410
Mainly H-bonding (intermolecular forces)