Potassium, Research Paper Example

Abstract

The history, qualities, chemical characteristics and physical characteristics of potassium were ewr3eviewed. The biological requisites of potassium in the human body were explored. The abundance of potassium in the Earth’s crust and the solar system were reviewed. The works of Acton (20139, Gupta (2015), Salunkhe & Deshpande (1991) were accessed.

Potassium

Physical Characteristics

Potassium is a metal which has the lightest density of all metals with the exception of lithium.  Potassium is a pliable metal which has a soft silvery quality.  In oxidation, Potassium exudes a light purple color.  The highest emission wavelength of potassium is 76.5 micrometers. (Acton, 2013).

Chemical Qualities

Potassium is composed of nineteen electrons.  Potassium is similar in its electron formation to argon, which is one of the noble gases.  Potassium has a low energy for ionization which gives it a great likelihood of contributing the electron when experiencing reactions with the oxidation process.  The majority of compounds which are formed by potassium are found in the electron state where it acquires a positive charge of one.  Potassium readily reacts with oxygen and the hydroxide ion.  When it reacts, the potassium molecule emits a purple color while releasing heat and hydrogen during the reaction (Acton, 2013).

Compounds

 As a result of the exothermic quality of potassium, it is applied in the form of NaK in order to desiccate materials prior to combining them with solvents.  Potassium is non-reactive with the majority of hydrocarbons. Potassium dissolves easily in hydroxide or ammonia where it can reach a saturation of as much as 480 g per thousand grams of ammonia.  Potassium has substantial use in its reductant qualities which are to reduce magnesium into Ricke magnesium.  Potassium reacts readily with the carbonate ion in order to form potassium carbonate (Acton, 2013).

Potassium carbonate is applied in order to extract minute amounts of gas.  Potassium has an excellent index of solubility with water.  This is attributed to the contributing charge of one that potassium manifests. In the oxidation process, potassium oxidizes more readily than any other metal with oxygen with the exclusion of lithium. The outcomes of the oxidation reactions with oxygen are potassium superoxide, potassium peroxide and potassium oxide (Acton, 2013).

Abundance

Potassium composed approximately 2.6 % of the crust that encases the Earth. It is one of the seven most abundantly found elements in the Earth. Potassium is one of the twenty most abundantly found elements in the solar system.  The saturation of potassium encountered in seawater is 0.39 mg/ ml (Gupta, 2015).

Isotopes

The isotopes which are formed from potassium are applied for dating. A potassium isotope which dates items by their saturation of potassium and the quantity of radiogenic is 40 Ar. Volcanic feldspars, hornblende, metamorphic hornblende, muscovite and biotite are isotopes of potassium. The radio- isotope that is most frequently encountered in the human body is 40K.  It is also the largest radioactive emission source in the human body (Gupta, 2015).

Biochemical Applications

The indexes of potassium affect a variety of physiological functions. Potassium affects the resting cellular membrane operation and the distribution of the action potentials in cardiac, neuronal and muscular tissues.  Potassium ions have the quality of being larger than the sodium ions.  The pumping systems which serve the body have the capacity of differentiating between sodium and potassium, while blocking the potassium and enabling the sodium to pass. Potassium is responsible for the action and secretion of hormones. In addition, potassium maintains the rigidity of the vascular system and the systemic blood pressure (Salunkhe & Deshpande, 1991).

 Potassium is responsible for the movement of food in the gastro digestive tract.  Furthermore, potassium in the human body is responsible for a number of fluid balancing activities including the maintenance of the equilibrium between the fluids and electrolytes, concentration of renal fluids and activates of the mineral corticoids.  The potassium content in the body is responsible for the glucose and insulin absorption and the balancing of the acids and bases within the human body (Salunkhe & Deshpande, 1991).

Applications of Potassium

Potassium is applied as a primary ingredient in fertilizer.  It is applied in potassium nitrate, potassium sulfate and potassium chloride. In addition, potassium is found in food.  It is required for the substance of human life. Potassium bicarbonate and potassium chloride are applied in the administration of hypertension.  Potassium sodium tartrate is found in baking powders.  Potassium bromate is applied as leavening.  Potassium sulfate is utilized as a food preservative. The industrial uses of potassium are potassium nitrate (saltpeter) which is derived from evaporates and guano applied as gun powder (Gupta, 2015).

Potassium cyanide is used is order to dissociate precious metals and copper. Potassium carbonate is applied in the production of vitrine products. Potassium permanganate is applied as a sweetener is the creation of saccharin.  Potassium bromate is applied a sedative and dye in photography.  Potassium chromate is applied in inks. Potassium oxide is applied in the filtration respiratory systems applied in mining and space exploration (Gupta, 2015).

History

 Potassium was initially encountered and classified by Sir Humphry Davy of England in 1807.  The first potassium was a caustic potash derivative which had been encountered by means of electrolysis of the melted potassium hydroxide in the voltaic piles use in batteries.  Justus Liebig discovered that potassium was a requisite for plant growth. At first, the ashes from wood had been applied a source of potassium. Potassium chloride mineral deposits had been found in Germany during the nineteenth century.  In the late 1960s, the potassium chloride production had become dominated by Canada (Gupta, 2015).

Conclusion

Potassium is one of the lightest density metals.  Potassium has an electron configuration similar to argon.  Potassium cannot be dissolved in hydrocarbons; however, it has a high saturation point in ammonia.  Potassium is a required element in human life and plant life processes.

References

Acton, A. (2013). Potassium Compounds- Advances in Research and Application. Atlanta, GA: Scholarly Editions.

Gupta, A. K. (2015). Origin of Potassium- Rich Silica Deficient Igneous Rocks. New York, NY: Springer.

Salunkhe, D. K.  and Deshpande, S. S. (1991). Foods of Plant Origin: Production, Technology and Human Nutrition.New York, NY: AVI.