User talk:Robert Tito/carbon in life sub: Difference between revisions
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Why does carbon hold the central place in forming living materials? The [[Physical chemistry|physical chemistry]] of the carbon atom renders it avid to form many different type of bonds to other elements, and, even more easily, to bond to itself, forming carbon-to-carbon bonds. Not only does carbon react with many other kinds of atoms, but, due to its energy content and its number of electrons available (even in hybrid form [[sp-hybridisation]]) to form bonds, carbon is able to form different ''types'' of (covalent) bonds. These bonds vary in strength as well as in conformation. The standard, most simple, bond carbon can form is that of a tetrahedron, or pyramid. That structure can be found in methane gas, for instance, and is the basis for the hardness of diamonds. Other type of bonds involve more than one shared electron, and for that reason are called double, and triple bonds; importantly, these different bonds constitute three entirely different geometries. That means that if a double bond is reduced to a single bond, for example, that region of the molecule actually changes shape. The avidity for carbon to bond to itself facilitates assembly of long chains and rings of carbon; and small carbon molecules (like [[sugar]]s, [[amino acid]]s and [[nucleotide]]s) easily join into huge [[macromolecule]]s. Those macromolecules can derive stability from their environment by electrostatic interactions such as hydrogen-bridges, and so do not disassociate | Why does carbon hold the central place in forming living materials? The [[Physical chemistry|physical chemistry]] of the carbon atom renders it avid to form many different type of bonds to other elements, and, even more easily, to bond to itself, forming carbon-to-carbon bonds. Not only does carbon react with many other kinds of atoms, but, due to its energy content and its number of electrons available (even in hybrid form ([[sp-hybridisation]])) to form bonds, carbon is able to form different ''types'' of (covalent) bonds. These bonds vary in strength as well as in conformation. The standard, most simple, bond carbon can form is that of a tetrahedron, or pyramid. That structure can be found in methane gas, for instance, and is the basis for the hardness of diamonds. Other type of bonds involve more than one shared electron, and for that reason are called double, and triple bonds; importantly, these different bonds constitute three entirely different geometries. That means that if a double bond is reduced to a single bond, for example, that region of the molecule actually changes shape. The avidity for carbon to bond to itself facilitates assembly of long chains and rings of carbon; and small carbon molecules (like [[sugar]]s, [[amino acid]]s and [[nucleotide]]s) easily join into huge [[macromolecule]]s. Those macromolecules can derive stability from their environment by electrostatic interactions such as [[Hydrogen bond|hydrogen-bridges]], and so do not disassociate easily. | ||
Because many elements are able to form bonds with carbon, organic macromolecules are capable of containing tremendous banks of information coded in their very structure. Not only can each of the constituents forming these huge molecules be one of several categories of chemicals, but each category contains several species (e.g., for nucleotides: adenine, thymine, guanine, cytosine, uracil). The order of species can be varied, and so there are exponential numbers of possible combinations. The shapes of the bonding orbitals of at least some of the carbon bonds add yet additional levels of information -for example, in double bonds, species can be connected in one of two different planes, called in [[Organic chemistry ]]''cis'' or'' trans''. | Because many elements are able to form bonds with carbon, organic macromolecules are capable of containing tremendous banks of information coded in their very structure. Not only can each of the constituents forming these huge molecules be one of several categories of chemicals, but each category contains several species (e.g., for nucleotides: adenine, thymine, guanine, cytosine, uracil). The order of species can be varied, and so there are exponential numbers of possible combinations. The shapes of the bonding orbitals of at least some of the carbon bonds add yet additional levels of information -for example, in double bonds, species can be connected in one of two different planes, called in [[Organic chemistry|organic chemistry]] ''cis'' or'' trans''. | ||
== Is this where it should be? == | |||
Should this page not be in the user space? [[User:Petréa Mitchell|Petréa Mitchell]] 14:49, 13 May 2007 (CDT) | |||
this is where it should be - they are notes for the Life article. [[User:Robert Tito|Robert Tito]] | <span style="background:grey"> <font color="yellow"><b>[[User talk:Robert Tito|Talk]]</b></font> </span> 14:54, 13 May 2007 (CDT) | |||
:This article is named [[Robert Tito/carbon in life]] in mainspace. Shouldn't it either be at [[User:Robert Tito/carbon in life]] or at [[carbon in life]]. [[User:Derek Harkness|Derek Harkness]] 13:25, 7 June 2007 (CDT) | |||
Latest revision as of 17:44, 7 June 2007
Made these changes:I think it reads better- is it still correct? n
Why does carbon hold the central place in forming living materials? The physical chemistry of the carbon atom renders it avid to form many different type of bonds to other elements, and, even more easily, to bond to itself, forming carbon-to-carbon bonds. Not only does carbon react with many other kinds of atoms, but, due to its energy content and its number of electrons available (even in hybrid form (sp-hybridisation)) to form bonds, carbon is able to form different types of (covalent) bonds. These bonds vary in strength as well as in conformation. The standard, most simple, bond carbon can form is that of a tetrahedron, or pyramid. That structure can be found in methane gas, for instance, and is the basis for the hardness of diamonds. Other type of bonds involve more than one shared electron, and for that reason are called double, and triple bonds; importantly, these different bonds constitute three entirely different geometries. That means that if a double bond is reduced to a single bond, for example, that region of the molecule actually changes shape. The avidity for carbon to bond to itself facilitates assembly of long chains and rings of carbon; and small carbon molecules (like sugars, amino acids and nucleotides) easily join into huge macromolecules. Those macromolecules can derive stability from their environment by electrostatic interactions such as hydrogen-bridges, and so do not disassociate easily.
Because many elements are able to form bonds with carbon, organic macromolecules are capable of containing tremendous banks of information coded in their very structure. Not only can each of the constituents forming these huge molecules be one of several categories of chemicals, but each category contains several species (e.g., for nucleotides: adenine, thymine, guanine, cytosine, uracil). The order of species can be varied, and so there are exponential numbers of possible combinations. The shapes of the bonding orbitals of at least some of the carbon bonds add yet additional levels of information -for example, in double bonds, species can be connected in one of two different planes, called in organic chemistry cis or trans.
Is this where it should be?
Should this page not be in the user space? Petréa Mitchell 14:49, 13 May 2007 (CDT)
this is where it should be - they are notes for the Life article. Robert Tito | Talk 14:54, 13 May 2007 (CDT)
- This article is named Robert Tito/carbon in life in mainspace. Shouldn't it either be at User:Robert Tito/carbon in life or at carbon in life. Derek Harkness 13:25, 7 June 2007 (CDT)