Carbon and Potassium - Features and Application - Essay Example

Student’s Name: Professor’s Name: Course Title Date Chemical Elements Carbon Element Carbon is a group 14 semi-conductor element that falling within the second period of the periodic table. It is represented by symbol C, has an atomic number of 6 (Z=6) and its electronic configuration is of the form 1s2 2s2 2p2 at the ground state. In the figure below, the distribution of electrons, neutrons and protons within atomic structure of carbon is illustrated (Pierson 14). Figure 1: Carbon atomic structure Valence There are two forms of carbons in existence and they include divalent and tetravalent forms. Divalent carbons have a valence of two in which case only 2p orbital electrons are free for bonding. These types of carbons are only found in a few reactive transient-organic intermediates, for instance carbenes. It is important to note that stable compounds of carbon as well as the carbon’s allotropes are tetravalent meaning that there are only four valence electrons involved in bonding (Pierson 15). Physical and Chemical Properties of a Carbon Element Carbon is a semiconductor element and it reacts by sharing electrons rendering it to have chemical characteristics that lie between metals and non-metals. The average atomic mass of carbon is about 12.01115 amu which is derived after averaging the atomic weights of a natural carbon atom that consists of an estimated 1.11% weight of C 13 as well as 98.89% of C12. The atomic radius of carbon is 0.77nm which is half the symmetric distance between two planar graphite carbon atom structures. It is worth noting that the initial ionization potential of a carbon atom is 11.260V (Pierson 17). Carbon Isotopes Carbon has seven isotopes; 10C, 11C, 12C, 13C, 14C, 15C and 16C that differs with each other in terms of mass number. Among the seven isotopes, 12C is the most widespread isotope and contains six neutrons whereas the rest contains between 4 and 10 neutrons. In that case, the table below illustrates characteristics of the seven carbon isotopes. Table 1: Characteristics of seven Carbon isotopes In respect to the above, Carbon-13 and Carbon-12 are referred to as steady isotopes in that they neither spontaneously alter their structure nor disintegrate. It is worth noting that these stable isotopes do exist naturally in which case C-12 and C-13 contributes 98.89% and 1.11% weight of the naturally existing carbon. The other five carbon isotopes are radioactive in nature and they have average rate of disintegration rate regardless of any alterations that may occur within the atom’s physical or chemical conditions. Subsequently, 16C, 15C, 11C and 10C isotopes contain short half-lives and therefore their specific use is limited. 14C on the other hand contains a long half-life and therefore it has important applications especially in carbon dating. Below are atomic structures of the three most useful isotopes of carbon (Pierson 19). Figure 2: Atomic structures of the three most useful Carbon Isotopes Natural Occurrence of Carbon Element The carbon element is distributed extensively in nature. In the crust of earth, it is found in 180ppm ratio with the greatest percentage being in form of compounds. Majority of carbon’s naturally occurring compounds are crucial in production of carbon-based synthetic materials as well as various for instant anthracite and bituminous, hydrocarbons complexes such as asphalt, tar, and petroleum and gaseous hydrocarbons such as methane. It is worth noting that natural diamond and carbon polymorphs are the only ones found in form of a mineral on earth (Ibid, 3). Industrial and Everyday Use Of Carbon Products that are derived from carbon element are commonly found in everyday life facets and they are for instance chimney grimy soot and jewellery box diamond (Pierson 17). Furthermore, broad application of carbon element are as outlined below, Natural graphite for shoe polish and lubricants Black carbon reinforcement vital to all automobile tires Black carbon and black lamp contained in every printing ink Black acetylene in conductive rubber Bone chars and vegetable to purify and decolorize sugar as well as other food Activated charcoal for catalytic and gas purification Essentiality of Carbon in Life Other than the above uses, Carbon is utilized by plants during photosynthesis in the form of Carbon Dioxide gas. This ensures that there is life continuation on earth. Potassium Element Potassium element is a group one metal in the fourth period of periodic table. It is represented by the symbol K with its Atomic Number being 19 (Z=19) whereas the Relative Atomic Mass is 39.098. Electronic configuration of Potassium is of the form ‘1s2, 2s2, 2p6, 3s2, 3p6, 3d1’ and in the figure below, the atomic structure is illustrated (Tiecke 1). Figure 3: Potassium atomic structure Valence Potassium has a valence of one with an oxidization state of K+1 which is the main one and another of K-1 in NH3 liquid. Isotopes of Potassium Potassium has five naturally occurring isotopes that include 39K, 40K, 41K, 42K and 43K. Potassium-41 and potassium-39 are the only two stable potassium isotopes and the remaining three are radio active. Potassium-39 accounts for 93% of the total potassium occurring naturally, while the rest is essentially contributed by potassium-41. Radioactive potassium-40 contains a very minute percentage of around 0.012% of potassium that occurs naturally. The table gives the characteristics of the five potassium isotopes (Argonne National Laboratory 1). Table 2: Characteristics of the five Potassium isotopes Physical and Chemical Properties Potassium is a white soft metal that is silvery while cut but oxidises rapidly to form white potassium oxide. Potassium metal has very low density and ranks high amongst the most electropositive and reactive metals. As such it oxidises rapidly in the air and it is supposed to be stored in mineral oils such as kerosene. It reacts vigorously with water in which case it spontaneously catches fire and decomposes with hydrogen evolution. In case, potassium is burnt in presence of oxygen, it produces a violet-coloured flame. Consequently, potassium has a melting point of 336K, a boiling point of 1047K, a density of 862kg/m-3, electron affinity of -43.8(M-M)/kJ mol-1, first ionization energy of 418.8kJ mol-1 and electron configuration of [Ar]4s1 at ground state (Stewart 1). Natural Occurrence of Potassium Potassium metal is the 7th most plentiful metal and creates 2.4% by earth’s crust mass. Majority of potassium containing minerals are slightly soluble and therefore, it is difficult to extract the metal from them. However, certain minerals for instance carnallite, sylvinite as well as sylvite found in potassium salts, and old lakes or seas evaporation depositions can be used to extract potassium. Potassium is also found in small amount in oceans (Stewart 1; Zookeeper 1). Uses of Potassium Potassium is highly used in making fertilizers. Other greatly important salts of potassium include sulphate, cyanide, bromide, chloride and nitrate. Potassium Essentiality in Life Potassium is a non-toxic element that is extensively spread in nature and present in every animal as well as plant tissue and thus, essential to life. However, one of its naturally occurring isotope (Potassium-40) has a mild radioactive characteristics and therefore, it might be one of man’s genetic mutation natural cause (Argonne National Laboratory 2). Sodium Element Sodium is a group one metal in the third period of the periodic table symbolized by Na. It has an atomic number of 11, Relative Atomic Mass of 22.990 and first ionization energy of 495.8kJ mol-1, and with a configuration of (1s2, 2s2, 2p6, 3s1). The sodium atomic structure appears as shown in the diagram below (Doug 1). Figure 4: Sodium atomic structure Valence Sodium has a valence of one with main oxidation state of Na+1 and Na-1 in the liquid of NH3 Isotopes of Sodium Sodium contains three isotopes which include 22Na, 23Na and 24Na. 23Na is a stable element and it’s the only isotope that is occur naturally in nature. 22Na and 24Na are radioactive isotopes with a half-life of 2.602 years and 15 hours respectively. The table below shows important characteristics of the three sodium isotopes. Table 3: Characteristics of the three Sodium isotopes Physical and Chemical Characteristic of Sodium Sodium is a silvery-white, soft metal that is normally preserved in paraffin since it oxidises fast when cut. It is an excessively reactive metal and thus caution should be observed while handling it. Sodium floats on water where it decomposes with hydrogen evolution, forming sodium hydroxide. Depending on the size of the metal uncovered to the water, sodium may not or may ignite spontaneously. It always ignites spontaneously in air at temperature of 115oC and above. It has a melting point of 370.96K, a boiling point of 1156.1K, a density of 971 kg m-3, electron affinity of -21 (M-M-)/kJ mol-1, and an electron configuration of [Ne]3s1 at ground state (Doug 2). Natural Occurrence of Sodium Sodium metal is the 6th most plenty element on earth and consists of 2.6% of the crust of earth. Sodium chloride is its most widespread compound, although, it is also found in several minerals such as sodalite, zeolite and cryolite. Due to its high rate of reactivity, sodium never occurs free in nature. It is extracted commercially through dry melt sodium chloride electrolysis. Industrial and Everyday use of Sodium Sodium metallic is used in esters and sodamide manufacturing as well as in the preparation of particular organic compounds. Additionally, sodium is employed in alloy formation and purifying as well as de-scaling metals. Notably, some sodium-potassium alloys have extensively been used as key agents in heat transfer. Compounds of sodium are essential in a number of industries which include metal, petroleum, textile, soap, glass and paper. In addition, sodium salt contains essential nutritional significance (Doug 1). Essentiality of Sodium in Life Sodium is vital to every animal, an aspect that has been in recognition since prehistoric eras. Although it is regarded as non-toxic, excessive use of salt in the diet has under specific circumstances been connected to high blood pressure. Works Cited Pierson, Hugh O. Handbook of carbon, graphite, diamond and fullerenes. Properties, processing, and applications. New Jersey: Noyes publications, 1993. Print. Argonne National Laboratory, EVS. “Potassium-40.” Human health fact sheet, August 2005. 1-2. Web. 1 Aug. 2012. . Stewart, Doug. "Potassium." Chemicool Periodic Table. Chemicool.com. 26 Feb. 2012. Web. 8 Feb. 2012. . Zookeeper. “Element #19: Potassium (K).” 08 Dec. 2012. Web. 1 Aug. 2012. . Doug, Stewart. "Sodium." Chemicool Periodic Table. Chemicool.com. 05 Mar. 2012. Web. 8 Feb. 2012. . Tiecke, T.G. Properties of Potassium. Waals-Zeeman Institute, University of Amsterdam. 2010. 1-14. Web. 1 Aug. 2012. . Read More

14C on the other hand contains a long half-life and therefore it has important applications especially in carbon dating. Below are atomic structures of the three most useful isotopes of carbon (Pierson 19). Figure 2: Atomic structures of the three most useful Carbon Isotopes Natural Occurrence of Carbon Element The carbon element is distributed extensively in nature. In the crust of earth, it is found in 180ppm ratio with the greatest percentage being in form of compounds. Majority of carbon’s naturally occurring compounds are crucial in production of carbon-based synthetic materials as well as various for instant anthracite and bituminous, hydrocarbons complexes such as asphalt, tar, and petroleum and gaseous hydrocarbons such as methane.

It is worth noting that natural diamond and carbon polymorphs are the only ones found in form of a mineral on earth (Ibid, 3). Industrial and Everyday Use Of Carbon Products that are derived from carbon element are commonly found in everyday life facets and they are for instance chimney grimy soot and jewellery box diamond (Pierson 17). Furthermore, broad application of carbon element are as outlined below, Natural graphite for shoe polish and lubricants Black carbon reinforcement vital to all automobile tires Black carbon and black lamp contained in every printing ink Black acetylene in conductive rubber Bone chars and vegetable to purify and decolorize sugar as well as other food Activated charcoal for catalytic and gas purification Essentiality of Carbon in Life Other than the above uses, Carbon is utilized by plants during photosynthesis in the form of Carbon Dioxide gas.

This ensures that there is life continuation on earth. Potassium Element Potassium element is a group one metal in the fourth period of periodic table. It is represented by the symbol K with its Atomic Number being 19 (Z=19) whereas the Relative Atomic Mass is 39.098. Electronic configuration of Potassium is of the form ‘1s2, 2s2, 2p6, 3s2, 3p6, 3d1’ and in the figure below, the atomic structure is illustrated (Tiecke 1). Figure 3: Potassium atomic structure Valence Potassium has a valence of one with an oxidization state of K+1 which is the main one and another of K-1 in NH3 liquid.

Isotopes of Potassium Potassium has five naturally occurring isotopes that include 39K, 40K, 41K, 42K and 43K. Potassium-41 and potassium-39 are the only two stable potassium isotopes and the remaining three are radio active. Potassium-39 accounts for 93% of the total potassium occurring naturally, while the rest is essentially contributed by potassium-41. Radioactive potassium-40 contains a very minute percentage of around 0.012% of potassium that occurs naturally. The table gives the characteristics of the five potassium isotopes (Argonne National Laboratory 1).

Table 2: Characteristics of the five Potassium isotopes Physical and Chemical Properties Potassium is a white soft metal that is silvery while cut but oxidises rapidly to form white potassium oxide. Potassium metal has very low density and ranks high amongst the most electropositive and reactive metals. As such it oxidises rapidly in the air and it is supposed to be stored in mineral oils such as kerosene. It reacts vigorously with water in which case it spontaneously catches fire and decomposes with hydrogen evolution.

In case, potassium is burnt in presence of oxygen, it produces a violet-coloured flame. Consequently, potassium has a melting point of 336K, a boiling point of 1047K, a density of 862kg/m-3, electron affinity of -43.8(M-M)/kJ mol-1, first ionization energy of 418.8kJ mol-1 and electron configuration of [Ar]4s1 at ground state (Stewart 1). Natural Occurrence of Potassium Potassium metal is the 7th most plentiful metal and creates 2.4% by earth’s crust mass. Majority of potassium containing minerals are slightly soluble and therefore, it is difficult to extract the metal from them.

However, certain minerals for instance carnallite, sylvinite as well as sylvite found in potassium salts, and old lakes or seas evaporation depositions can be used to extract potassium.

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