A compound that is electron deficient has too few valence electrons for the connections between atoms to be described as covalent bonds. Electron deficient bonds are often better described as 3-center-2-electron bonds. Examples of compounds that are electron deficient are the boranes, including diborane. In chemistry, valence electrons (vay-luhhn-cee) are the electrons contained in the valence shell of an atom, and which are likely to participate in a chemical reaction through bonding with other atoms, molecules, or ions. ... Covalently bonded hydrogen and carbon in a molecule of methane. ... The 3-center-2-electron bond is an electron deficient chemical bond where three atoms share two electrons. ... A borane is an inorganic chemical compound of boron and hydrogen. ... Diborane is a colorless gas at room temperature with a repulsive, sweet odor. ...
The electrons are passed from one carrier molecule to another in a downhill direction, like individuals in a bucket brigade passing water from the top of a hill to the bottom.
Each electron carrier is at a lower energy level than the one before it, and the result is that electrons release energy as they move down the chain.
P680 in Photosystem II is now electrondeficient because it has donated electrons to P700 in Photosystem I. P680 electrons are replenished by the water that has been absorbed by the plant roots and transported to the chloroplasts in the leaves.
Electrondeficiency occurs when a compound has too few valence electrons for the connections between atoms to be described as covalent bonds.
Electrondeficient bonds are often better described as 3-center-2-electron bonds.
The term electrondeficient is also used in a more general way in organic chemistry, to indicate a pi-system such as an alkene or arene that has electron withdrawing groups attached, as found in nitrobenzene or acrylonitrile.
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