Publication

Polypeptide inhibitors of urokinase type plasminogen activator

Christian Heinis, Alessandro Angelini
2013
Patents

Abstract

A conjugate which is capable of specific binding to and inhibition of urokinase-type plasminigen activator (UPA) comprising a polypeptide molecule and a scaffold molecule, wherein said polypeptide molecule is attached to said scaffold molecule by at least three covalent bonds and wherein the inhibition constant (Ki) for said inhibitor is less than 500nM.

Official source

https://infoscience.epfl.ch/entities/publication/320fa293-1f8d-43bc-92a1-fc062d06ceb0

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Christian Heinis, Alessandro Angelini
2013
Patents

Abstract

Official source

https://infoscience.epfl.ch/entities/publication/320fa293-1f8d-43bc-92a1-fc062d06ceb0

About this result

Related concepts (14)

Covalent bond

A covalent bond is a chemical bond that involves the sharing of electrons to form electron pairs between atoms. These electron pairs are known as shared pairs or bonding pairs. The stable balance of attractive and repulsive forces between atoms, when they share electrons, is known as covalent bonding. For many molecules, the sharing of electrons allows each atom to attain the equivalent of a full valence shell, corresponding to a stable electronic configuration. In organic chemistry, covalent bonding is much more common than ionic bonding.

Coordinate covalent bond

In coordination chemistry, a coordinate covalent bond, also known as a dative bond, dipolar bond, or coordinate bond is a kind of two-center, two-electron covalent bond in which the two electrons derive from the same atom. The bonding of metal ions to ligands involves this kind of interaction. This type of interaction is central to Lewis acid–base theory. Coordinate bonds are commonly found in coordination compounds. Coordinate covalent bonding is ubiquitous.

Chemical bond

A chemical bond is a lasting attraction between atoms or ions that enables the formation of molecules, crystals, and other structures. The bond may result from the electrostatic force between oppositely charged ions as in ionic bonds, or through the sharing of electrons as in covalent bonds. The strength of chemical bonds varies considerably; there are "strong bonds" or "primary bonds" such as covalent, ionic and metallic bonds, and "weak bonds" or "secondary bonds" such as dipole–dipole interactions, the London dispersion force, and hydrogen bonding.

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