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Formally, a carbanion is the conjugate base of a carbon acid: R 3 CH + B − → R 3 C − + HB. where B stands for the base. The carbanions formed from deprotonation of alkanes (at an sp 3 carbon), alkenes (at an sp 2 carbon), arenes (at an sp 2 carbon), and alkynes (at an sp carbon) are known as alkyl, alkenyl , aryl, and alkynyl anions ...
As a rule, however, these neutral oxocarbons are less stable than the corresponding anions. Thus, for example, the stable carbonate anion corresponds to the extremely unstable neutral carbon trioxide CO 3; [2] oxalate C 2 O 2− 4 correspond to the even less stable 1,2-dioxetanedione C 2 O 4; [3] and the stable croconate anion C 5 O 2−
Other uncommon oxides are carbon suboxide (C 3 O 2), [96] the unstable dicarbon monoxide (C 2 O), [97] [98] carbon trioxide (CO 3), [99] [100] cyclopentanepentone (C 5 O 5), [101] cyclohexanehexone (C 6 O 6), [101] and mellitic anhydride (C 12 O 9). However, mellitic anhydride is the triple acyl anhydride of mellitic acid; moreover, it contains ...
The net charge of an ion is not zero because its total number of electrons is unequal to its total number of protons. A cation is a positively charged ion with fewer electrons than protons [2] (e.g. K + (potassium ion)) while an anion is a negatively charged ion with more electrons than protons. [3] (e.g. Cl − (chloride ion) and OH − ...
Carbon trioxide (CO 3) is an unstable oxide of carbon (an oxocarbon). The possible isomers of carbon trioxide include ones with molecular symmetry point groups C s , D 3h , and C 2v . The C 2v state, consisting of a dioxirane , has been shown to be the ground state of the molecule. [ 1 ]
Its average bond length is 0.14 nm. Each carbon atom in the structure is bonded covalently with 3 others. [30] A carbon atom in the C 60 can be substituted by a nitrogen or boron atom yielding a C 59 N or C 59 B respectively. [31] Energy level diagram for C 60 under "ideal" spherical (left) and "real" icosahedral symmetry (right).
The valence is the combining capacity of an atom of a given element, determined by the number of hydrogen atoms that it combines with. In methane, carbon has a valence of 4; in ammonia, nitrogen has a valence of 3; in water, oxygen has a valence of 2; and in hydrogen chloride, chlorine has a valence of 1.
Electron affinity can be defined in two equivalent ways. First, as the energy that is released by adding an electron to an isolated gaseous atom. The second (reverse) definition is that electron affinity is the energy required to remove an electron from a singly charged gaseous negative ion.