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This bond is a covalent, single bond, meaning that carbon shares its outer valence electrons with up to four hydrogens. This completes both of their outer shells, making them stable. [2] Carbon–hydrogen bonds have a bond length of about 1.09 Å (1.09 × 10 −10 m) and a bond energy of about 413 kJ/mol (see table below).
In this reaction a variety of reagents add "across" the pi-bond(s). Chlorine, hydrogen chloride, water, and hydrogen are illustrative reagents. Polymerization is a form of addition. Alkenes and some alkynes also undergo polymerization by opening of the multiple bonds to produce polyethylene, polybutylene, and polystyrene.
In ethene, the two carbon atoms form a σ bond by overlapping one sp 2 orbital from each carbon atom. The π bond between the carbon atoms perpendicular to the molecular plane is formed by 2p–2p overlap. Each carbon atom forms covalent C–H bonds with two hydrogens by s–sp 2 overlap, all with 120° bond angles. The hydrogen–carbon bonds ...
Hydrogen is a chemical element; it has symbol H and atomic number 1. It is the lightest element and, at standard conditions, is a gas of diatomic molecules with the formula H 2, sometimes called dihydrogen, [11] hydrogen gas, molecular hydrogen, or simply hydrogen. It is colorless, odorless, [12] non-toxic, and highly combustible.
Covalent bonding of two hydrogen atoms to form a hydrogen molecule, H 2. In (a) the two nuclei are surrounded by a cloud of two electrons in the bonding orbital that holds the molecule together. (b) shows hydrogen's antibonding orbital, which is higher in energy and is normally not occupied by any electrons.
In the secondary structure of proteins, hydrogen bonds form between the backbone oxygens and amide hydrogens. When the spacing of the amino acid residues participating in a hydrogen bond occurs regularly between positions i and i + 4, an alpha helix is formed. When the spacing is less, between positions i and i + 3, then a 3 10 helix is formed.
An alkane has only C–H and C–C single bonds. The former result from the overlap of an sp 3 orbital of carbon with the 1s orbital of a hydrogen; the latter by the overlap of two sp 3 orbitals on adjacent carbon atoms. The bond lengths amount to 1.09 × 10 −10 m for a C–H bond and 1.54 × 10 −10 m for a C–C bond.
Each carbon atom of the double bond uses its three sp 2 hybrid orbitals to form sigma bonds to three atoms (the other carbon atom and two hydrogen atoms). The unhybridized 2p atomic orbitals, which lie perpendicular to the plane created by the axes of the three sp 2 hybrid orbitals, combine to form the pi bond. This bond lies outside the main C ...