Name: PowerPoint Presentation
Uploaded: 2023-05-15
Duration: 2 min 56 s
Description: “Exploring Phosphorus: The Element of Life”. Author: Yarima Leyva Chemistry Department The College of St. Scholastica.

“Exploring Phosphorus: The Element of Life”. Author: Yarima Leyva Chemistry Department The College of St. Scholastica. 

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“Exploring Phosphorus: The Element of Life”

Author: Yarima Leyva  Chemistry Department The College of St. Scholastica

Abstract This poster provides a comprehensive analysis of the non-metallic element phosphorus, emphasizing its importance in biological and industrial processes. It examines the element's electronic and nuclear structure, its oxidation states, and physical properties such as density, ionization energy, ionic radii, electron affinity, and electronegativity. The poster also explores phosphorus's role in various chemical reactions, including purification, isolation, Oxidation–Reduction, and, coordination chemistry, and its use in creating compounds like phosphoric acid and phosphine. Finally, it proposes a novel application for phosphorus in advanced energy storage systems, leveraging its unique electrochemical properties to contribute to sustainable energy solutions.

White phosphorus          Red Phosphorus            Black Phosphorus

Introduction:  Phosphorus is a non-metallic chemical element with the symbol P and atomic number 15. It's a crucial element for life, playing a key role in the structure of DNA, energy storage and transfer, and other biological processes. It is also used extensively in various industrial applications. Electronic and Nuclear Structure:  Phosphorus has 15 electrons, arranged in the electron configuration [Ne] 3s² 3p³. This structure indicates that phosphorus has five valence electrons, which explains its ability to form covalent compounds by sharing these electrons. The nucleus of phosphorus contains 15 protons and, typically, 16 neutrons in its most common isotope, phosphorus-31.

Oxidation States:  Phosphorus exhibits several oxidation states, the most common being +5, +3, and -3. The +5 oxidation state corresponds to the use of all five valence electrons in bonding, while the -3 state corresponds to the addition of three electrons to achieve a full outer shell. Physical Properties: Density: 1.82 g/cm³ Ionization Energy: 1st - 10.49 eV Ionic Radius: 212 pm (for the -3 ion) Electron Affinity: 0.746 eV Electronegativity (Pauling scale): 2.19

References: Atkins, P., & de Paula, J. (2010). Physical Chemistry (9th ed.). Oxford University Press.  Emsley, J. (2001). Nature's Building Blocks: An A-Z Guide to the Elements. Oxford University Press.  Gray, T. W.; Mann, N.   The Elements: A Visual Exploration of Every Known Atom in the Universe ; Black Dog & Leventhal Publishers,   2009.    Greenwood, N. N., & Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann.  Housecroft , C. E., & Sharpe, A. G. (2012). Inorganic Chemistry (4th ed.). Pearson.  Winter, M. (2023). Phosphorus.  WebElements . Retrieved from  www.webelements.com/phosphorus .

Chemical Reactions:  Phosphorus is involved in many chemical reactions due to its reactivity. Purification and Isolation:  Elemental phosphorus is produced from phosphate rock through a series of chemical reactions involving the use of sulfuric acid, silica, and carbon. Oxidation-Reduction Properties:  Phosphorus can undergo redox reactions, typically being oxidized from its elemental form to form compounds like phosphoric acid. Coordination Chemistry:  Phosphorus can form a variety of coordination compounds, particularly with transition metals. Synthesis and Application of Interesting Compounds:  Phosphorus forms many compounds with wide-ranging applications. Phosphoric Acid:  Used in fertilizers, detergents, and food additives. Phosphine:  Used in the semiconductor industry and for fumigation.

Allotropes: The diversity among phosphorus allotropes showcases the versatility of phosphorus as an element. From the highly reactive white phosphorus to the stable, semi-conducting black phosphorus, with red phosphorus as an intermediate, phosphorus has a wide range of applications in various fields. This depth of understanding underscores the element's potential for future technological advancements.

Chart or Image T his rare violet phosphorus is considered a mixture of red and black phosphorus.

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Atomic
Number
Symbol
Name
Electronic
Configuration
Electron
15
30.9737
Atomic
Weight
Crystal Structure
body-centred
cubic (bcc)
Phosphorus
1s2 2s2 2P6 3s2 3P3
Nucleus
Proton = 15
Neutron —15

Phosphorus , an element with unique properties, is essential to a multitude of biological and industrial processes. Biologically, it's a fundamental component of life, present in nucleic acids, ATP, phospholipids, and in bones and teeth as calcium phosphate. Industrially, it's a key player in the production of fertilizers, detergents, cleaning products, and is used in water treatment, flame retardants, steel production, and specialty glass and ceramics creation. Phosphorus' diverse applications highlight its crucial role in sustaining life and driving technological progress.

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 References: Atkins, P., & de Paula, J. (2010). Physical Chemistry (9th ed.). Oxford University Press.  Emsley, J. (2001). Nature's Building Blocks: An A-Z Guide to the Elements. Oxford University Press.  Gray, T. W.; Mann, N.   The Elements: A Visual Exploration of Every Known Atom in the Universe ; Black Dog & Leventhal Publishers,   2009.    Greenwood, N. N., & Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann.  Housecroft , C. E., & Sharpe, A. G. (2012). Inorganic Chemistry (4th ed.). Pearson.  Winter, M. (2023). Phosphorus.  WebElements . Retrieved from  www.webelements.com/phosphorus . 

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