112 In the 1880's, Louis Pasteur published his work on cellular aerobic respiration and glycolysis. In 1931, Otto Warburg won the Nobel Prize for his work on the metabolism of tumors and the respiration of cells, which was later summarized in his 1956 paper, On the Origin of Cancer Cells. His work on cancer expanded upon Pasteur's findings and described respiratory insufficiency and a cellular metabolism of glucose fermentation as the primary trigger for cancer progression.
Warburg's conclusions on cancer were much discussed in scientific circles, as they are academically elegant, but were not accepted by most members of the scientific community engaged in cancer research. Most cancer researchers in the late 1950's believed that the anaerobic metabolism of cancer cells and their accompanying output of lactic acid was a side effect or an adjunct effect of cancer, not a cause. Cancer research since the 1960's has focused primarily on genetic aberrations as causative for cancer, and has ignored the body of research on cancer pH and its implications for therapeutic approaches. Warburg's work was a catalyst for yet another research effort on the nature of cancer cells, beginning in the 1930's. A. Keith Brewer, PhD (physicist) performed experiments on the relationship between energized, oxygenated cell membrane and elemental uptake, vs. cellular membranes in an unenergized state such as cancer cells exhibit. He wrote a number of papers discussing the cellular mechanisms of cancer cells and the changes in metabolism induced or indicated by the lack of or presence of oxygen in combination with other elements, particularly potassium and calcium. He noted that cancer cells share one characteristic no matter what type of cancer: they have lost their pH control mechanism.
127 To reach this state of stability, both hydrogen and oxygen atoms create covalent bonds with each other, as illustrated in the diagram on the right. In a water molecule, two hydrogen atoms are covalently bonded to the oxygen atom. But because the oxygen atom is larger than the hydrogen atom, its attraction for the hydrogen's electrons is correspondingly greater so the electrons are drawn closer in to the orbit of the larger oxygen atom and away from the hydrogen orbits. This means that although the water molecule as a whole is stable, the greater mass of the oxygen nucleus tends to draw in all the electrons in the molecule including the shared hydrogen electrons giving the oxygen portion of the molecule a slight electronegative charge. The orbits of the hydrogen atoms, because their electrons are closer to the oxygen, take on a small electropositive charge. This means water molecules have a tendency to form weak bonds with other water molecules because the oxygen end of the molecule is negative and the hydrogen ends are positive. A hydrogen atom, while remaining covalently bonded to the oxygen of its own molecule, can form a weak bond with the oxygen of another molecule. Similarly, the oxygen end of a molecule can form a weak attachment with the hydrogen ends of other molecules. Because water molecules have this polarity, water is a continuous chemical entity. These weak bonds play a crucial role in stabilizing the shape of many of the large molecules found in living matter. Because these bonds are weak,
they are readily broken and re-formed during normal physiological reactions. The disassembly and re-arrangement of such weak bonds is in essence the chemistry of life. Water is a universal solvent due to the marked polarity of water molecules and their tendency to form hydrogen bonds with other molecules. To illustrate water's ability to break down other substances, consider the simple example of putting a small amount of table salt in a glass of water. Table salt, also known by its chemical name sodium chloride [NaCl], is an example of an ionic compound, which means that one of the atoms involved stole a valence electron from the other. In this case, the chlorine atom [Cl], stole an electron from the sodium atom [Na], resulting in the creation of an electronegative chloride ion [Cl-] and an electropositive sodium ion [Na+]. The two ions are bonded together because of the attraction of opposite charges. better understand ionic bonds After salt is placed in water, the ionic bond between the sodium and chloride ions is broken due to the competitive action of the water molecules that outnumber the salt molecules. The electronegative oxygen pole of the water molecule is attracted to the positively charged sodium ions [Na+], and the electropositive hydrogen pole of the water molecule is attracted to the negatively charged chloride ions [Cl-]. As with the example of table salt, water has the ability to dissolve many unwanted substances that have accumulated in our bodies over time, such as solid waste and toxins, and to flush them away through the body's natural elimination channels such as lungs, colon, kidneys, liver, and skin.