why organic compounds are quite stable?
954824
Because they have stable valence orbits. The ability of a chemical to react with another chemical is decided by the number of electrons in its outermost orbit. In case the number are such that it can attain stability by transfering (giving or taking) one electron, they easily react, and are therefore unstable. Incase their outermost orbit is full, as in the case of organic compounds - they do not give or take electrons easily, and are therefore stable.
1077307
not all of them..\n\nH2O, CH3CL, CH3COONa are weak.. (also any organic substance eg. CH3COOH)\nNaOH, KF are categorized as strong ones due to the formation of ionic bond bet. them, + they're inorganic..
641799
It depends on the octet rule. If the element fulfills its octet, or has 8 valence electrons(such as the noble gases) then it will be very stable. The farther they are from fulfilling the octet rule, the less stable the element is.
882356
organic compound class is  base on functional groups.
1088347
At a simple level, leaving groups are typically stable ions or molecules
816705
Organic molecules are found in living things..and organic fits, try that.
116145
If I remember my chemistry correctly, an organic molecule is one containing carbon and at least one other element.  So, a non-organic substance would be anything else.
870926
in order of increasing stability: 1, 2, 3.\n\nThe hyperconjugative and inductive effects are complimentary to each other and can not be mutually excluded.  \n\nThe empty P orbital on the carbocation interacts with the neighboring C-H sigma bonds resulting in transfer of electron density and formation of pi-bond character between the carbocation carbon and neighboring carbons.  This is the hyperconjugative effect.  The more neighbors you have, the more sharing can happen and the more stable the carbocation is.\n\nAttraction of electron density to the positively charged carbon results in induced dipoles between the carbocation carbon and its neighbors.  This allows for delocalization of the positive charge away from the carbocation carbon to its neighbors.  The neighbors become somewhat electron deficient due to electrons density herding toward the carbocation.  The more neighbors you have the more carbons the positive charge can be delocalized to and the more stable the carbocation.\n\nThe attraction of electron density referred to in the inductive argument is the partial pi bond formation in the hyperconjugation argument.
859386
Due to differences in chemical structures
324321
The same array of inorganic and simple organic molecules would be able to exist on an earth-like planet. This includes the different chiralities.\n\nComplex organic molecules, manufactured by living individuals (plants/ animals) have developed through evolutionary processes, and evolution is driven by random chance. So I would expect differences in the particular proteins etc. that have evolved.\n\nOn a non-earth-like planet (different temperatures/ pressures etc.), different molecules would be stable so you might get a completely different chemistry.
768752
it is due to the fact that most organic compounds are non polar in nature and water is a polar substance.
1176289
there is no such thing as an imbalaced biostructure.  Unstable molecules are a piece of fictional technology.  Do you mean free radicals?  most of them are produced, or were there in the beginning.  They self-replicated and had very low 'life'.  that's all I can do for now.
184098
has to do with intermolecular bonds. The bonds that hold a solid together are more ridgid than that of a liquid.
987874
http://en.wikipedia.org/wiki/Organic_chemistry
362869
Keywords:\n              Help\n\nCarbon has a unique place in our lives. Each living cell, food, wood, paper, petro-chemicals, cooking gas, perfumes, etc are all made up of carbon. Chemistry of carbon compounds is known as organic chemistry. Organic chemistry encompasses study of all carbon-hydrogen compounds. These are also called hydrocarbons. Inorganic carbon chemistry is the study of oxides, nitrides and allotropes of carbon.\n\nThere are many differences between organic and inorganic compounds. Organic compounds are mostly insoluble in water. They have low melting points and exist by forming covalent bonds. Inorganic compounds on the other hand usually dissolve in water and have high melting points. Inorganic compounds can be formed due to either ionic or covalent bonds. Another characteristic of organic compounds is that they are inflammable.\n\nCarbon has 6 protons, 6 neutrons and 6 electrons. Its chemical symbol is 12C 6. Its electronic configuration is 2 electrons in the K-shell, and 4 electrons in the L-shell. In principle it should either give up or borrow 4 electrons while forming compounds. But it doesn’t form ionic bonds at all. It likes to share its four electrons with other atoms and form covalent bonds instead. Carbon covalent bonds are the strongest in nature.\nWe might expect that a carbon atom to form three bonds of one kind using the p orbital electrons and one bond of another kind using the s orbital electron. But this does not happen!! The one 2s and three 2p orbitals mix together and give rise to four new altogether different types of orbitals. This is called  hybridization and is seen only in carbon atom. The four orbitals are at an angle of 109028’. This is called tetrahedral or sp3 (pronounced as sp three) type of hybridization. There are sp2 and sp types of hybridization also.
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.
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Silicon carbide is not organic. It is, however, very hard. It is used on the edges of cutting tools because it wears better than steel.\n\nOther carbon compounds exist that are not organically derived such as calcium carbide (used to generate acetelyne gas by reaction with water), carbon disulfide, etc. See the Wikipedia reference for others.