oxidative burst

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).