oxidative burst

(noun)

A chemical reaction that occurs in phagocytes in which an engulfed pathogen is destroyed by exposure to oxidative stress from reactive oxygen species.

Related Terms

  • PMN granulocyte
  • mesenchymal cells
  • epithelial cells
  • chemotaxis

Examples of oxidative burst in the following topics:

  • Relative Resistance of Microbes

    • However, alkylating agents (e.g. ethylene oxide), and 10% bleach are effective against endospores.
    • Due to their unique cell wall, they can survive long exposure to acids, alkalis, detergents, oxidative bursts, lysis by complement, and many antibiotics.
  • Phagocytes

    • A series of chemical reactions called an oxidative burst occurs, which uses reactive oxygen species and NADPH oxidase to damage and kill the pathogen through oxidative stress.
    • Oxidative stress can kill a cell through DNA, cell membrane, or mitochondrial damage.
    • For instance, other receptors may be used to engulf pathogens, and other non-oxidative methods (such as lysozyme) exist to kill the phagocytized pathogen.
  • Phosphorus Compounds as Reducing Agents

    • Trivalent phosphorus is easily oxidized.
    • In contrast with ammonia and amines, phosphine and its mono and dialkyl derivatives are pyrophoric, bursting into flame on contact with the oxygen in air.
    • The triphenylphosphine oxide produced in reactions 1 & 3 is a very stable polar compound, and in most cases it is easily removed from the other products.
    • Triphenylphosphine is also oxidized by halogens, and with bromine yields dibromotriphenylphosphorane, a crystalline salt-like compound, useful for converting alcohols to alkyl bromides.
    • As in a number of earlier examples, the formation of triphenylphosphine oxide in the irreversible SN2 step provides a thermodynamic driving force for the reaction.
  • Corrosion

    • Corrosion can be thought of as the spontaneous return of metals to their ores through the process of oxidation.
    • The conductive properties of metal enable the oxidation and reduction steps that occur during corrosion to take place at separate sites on the metal's surface.
    • The higher a metal's reduction potential, the less likely it is to be oxidized.
    • We see its effects in rusted out car frames, the bursting of water mains and the failure of bridges.
  • Aerobic Training vs. Strength Training

    • There are two principal ways to categorize muscle fibers: the type of myosin (fast or slow) present, and the degree of oxidative phosphorylation that the fiber undergoes.
    • These fibers are suited for endurance activities and are slow to fatigue because they use oxidative metabolism to generate ATP.
    • These fibers are efficient for short bursts of speed and power and use both oxidative and anaerobic metabolisms depending on the particular sub-type.
    • With training, a higher level of effort can be sustained for extended periods, using oxygen and oxidative phosphorylation as the primary energy source.
  • Electrons and Energy

    • The removal of an electron from a molecule via a process called oxidation results in a decrease in the potential energy stored in the oxidized compound.
    • The transfer of energy in the form of electrons allows the cell to transfer and use energy in an incremental fashion: in small packages rather than as a single, destructive burst.
    • These compounds can be easily reduced (that is, they accept electrons) or oxidized (they lose electrons).
    • When electrons are removed from a compound, the compound is oxidized.
    • In the above equation, NAD+ is an oxidizing agent and RH is oxidized to R.
  • Osmotic Pressure

    • However, they are permeable to non-polar and/or hydrophobic molecules like lipids as well as to small molecules like oxygen, carbon dioxide, nitrogen, nitric oxide, etc.
    • If it is put in a solution with a lower solute concentration than its own, the cell will expand and burst.
  • Oxidation Numbers of Metals in Coordination Compounds

    • Transition metals typically form several oxidation states and therefore have several oxidation numbers.
    • This oxidation number is an indicator of the degree of oxidation (loss of electrons) of an atom in a chemical compound.
    • O2- and S2- have oxidation numbers of -2.
    • In a molecule or compound, the oxidation number is the sum of the oxidation numbers of its constituent atoms.
    • The oxidation number of H is +1 (H+ has an oxidation number of +1).
  • Problems

    • We will try to model Type-I X-ray bursts using a simple model for the instability.
    • We will calculate how much material will accumulate on a neutron star before it bursts.
    • Let's assume that the potential burst starts by the temperature in the accreted layer jiggling up by a wee bit.
    • Calculate the value of $dM$ for which $dP_\mathrm{helium}/dT$ exceeds $dL_\mathrm{surface}/dT$ and the layer bursts.
  • Oxides

    • Metal oxides typically contain an anion of oxygen in the oxidation state of −2.
    • Most of the Earth's crust consists of solid oxides, the result of elements being oxidized by the oxygen in air or water.
    • Although most metal oxides are polymeric, some oxides are monomeric molecules.
    • Those attacked only by acids are basic oxides; those attacked only by bases are acidic oxides.
    • Metals tend to form basic oxides, non-metals tend to form acidic oxides, and amphoteric oxides are formed by elements near the boundary between metals and non-metals (metalloids).
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