Nutrients: Nitrogen (N), Sulfur (S), Phosphorus (P), Potassium (K)

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Nutrients: Nitrogen (N), Sulfur (S), Phosphorus (P), Potassium (K)
Essential for all life, their availability (or lack thereof) controls the distribution of flora and fauna

Look into their:

Sources

Pools (sinks)

Fluxes

root uptake
+microbial uptake leaching

solution
solid

Nutrients must be in a specific form – specie - for use by organisms

Soil Organic Matter

Nutrient Cycling: N, S, P, K

(CHONPS)

Minerals

(P, S, K)

Primary Productivity

Leaves & Roots

Decomposition

Heterotrophic respiration

Gas loss

SOM/Minerals
Microbes

leaching of nutrients

plant nutrient uptake

Nutrients: natural & anthropogenic sources (IN) and outputs (OUT)

N₂

fertilizers (chemical, manure, sludge) pesticides gases and particulates to atmosphere

(fossil fuel combustion (coal/oil); cycles; trees)

wet and dry deposition (acid rain, aerosols) plant tissue/residues harvesting root uptake

SOIL

Pools (sinks)

(SOM/clays/oxides)

Fluxes (transformations)

ions and molecules in solution (leaching)
roots (exudates, biomass)

colloidal transport erosion bedrock (1^ry/2^ryminerals in parent material) runoff

The Nitrogen Cycle

Denitrification:

reduction of NO₃to reduced forms of N (N₂) (energyconsuming)

NO₃is the most stable chemical form of N in aerated soil solutions
N₂(g) is prevalent in the air of soil pores

Atmospheric N deposition
Fertilizer additions
Nitrogen evolution (gases)

700 236

(+5)

NO₃

+5 -3

Oxic zone

(+3)

NO₂

(+2)

(+1)

N₂O

(0)

N₂

N-fixation

Suboxic zone

N-mineralization immobilization

NH₃

(-3)

Organic-N

⁺sorption

NH₄

(-3)

(~90% of soil N)

N-fixation: enzyme-

catalyzed reaction (occurs only in living organisms)
Oxidation of N₂does not occur except in a few organisms (N-N triple bond)

Nitrification: NH₃to oxidized

forms of N (NO₂, NO₃)
(energy-releasing)

The Sulfur Cycle

The Sulfur Cycle

Sulfur undergoes dramatic changes in redox cycling
Oxidation states range from +6 to -2

O₂

sorption

Sulfate found in oxidized environments

Oxic zone

SO₄

Suboxic zone

degradation of organic materials
(plant/animal)
A large variety of organic forms of S

reduced organic S

Anoxic zone

(thiol)

S^2-

H₂S
M²⁺+ S^2-= MS
(pptation of metal sulfides)

metal sulfides tend to be “insoluble”
(Hg, Ag, Cd, Cu, Pb, Zn, Fe(II))

In soil, SO₄originates from

• Organic matter mineralization

• Weathering of soil minerals

• Sulfur inputs from atmosphere

The Phosphorus Cycle

P primarily as phosphate (PO₄), with an oxidation state of 5+

Mostly in organic P and inorganic P forms

PO₄is strongly retained by soils but can be transported in colloidal forms

PO₄sorption onto Al and Fe oxides is strong

Phosphate minerals (low solubility):

Al and Fe phosphates (acid mineral soils)
(variscite, AlPO₄.2H₂O )

Ca phosphates (non acid soils)

(hydroxyapatite, Ca₅(PO₄)₃OH )
(strengite, FePO₄.2H₂O )

The Potassium Cycle

Potassium as K⁺with no changes in oxidation state

K⁺flux controlled by CEC & chemical weathering ~ no organisms

Sources: Primary and Secondary Minerals

Recommended publications

Phosphorus and Sulfur Cosmochemistry: Implications for the Origins of Life

Phosphorus and Sulfur Cosmochemistry: Implications for the Origins of Life Item Type text; Electronic Dissertation Authors Pasek, Matthew Adam Publisher The University of Arizona. Rights Copyright © is held by the author. Digital access to this material is made possible by the University Libraries, University of Arizona. Further transmission, reproduction or presentation (such as public display or performance) of protected items is prohibited except with permission of the author. Download date 07/10/2021 06:16:37 Link to Item http://hdl.handle.net/10150/194288 PHOSPHORUS AND SULFUR COSMOCHEMISTRY: IMPLICATIONS FOR THE ORIGINS OF LIFE by Matthew Adam Pasek ________________________ A Dissertation Submitted to the Faculty of the DEPARTMENT OF PLANETARY SCIENCE In Partial Fulfillment of the Requirements For the Degree of DOCTOR OF PHILOSOPHY In the Graduate College UNIVERSITY OF ARIZONA 2 0 0 6 2 THE UNIVERSITY OF ARIZONA GRADUATE COLLEGE As members of the Dissertation Committee, we certify that we have read the dissertation prepared by Matthew Adam Pasek entitled Phosphorus and Sulfur Cosmochemistry: Implications for the Origins of Life and recommend that it be accepted as fulfilling the dissertation requirement for the Degree of Doctor of Philosophy _______________________________________________________________________ Date: 04/11/2006 Dante Lauretta _______________________________________________________________________ Date: 04/11/2006 Timothy Swindle _______________________________________________________________________ Date: 04/11/2006
Phosphorus: from the Stars to Land &

Phosphorus: From the Stars to Land & Sea The MIT Faculty has made this article openly available. Please share how this access benefits you. Your story matters. Citation Cummins, Christopher C. “Phosphorus: From the Stars to Land & Sea.” Daedalus 143, no. 4 (October 2014): 9–20. As Published http://dx.doi.org/10.1162/DAED_a_00301 Publisher MIT Press Version Final published version Citable link http://hdl.handle.net/1721.1/92509 Terms of Use Article is made available in accordance with the publisher's policy and may be subject to US copyright law. Please refer to the publisher's site for terms of use. Phosphorus: From the Stars to Land & Sea Christopher C. Cummins Abstract: The chemistry of the element phosphorus offers a window into the diverse ½eld of inorganic chemistry. Fundamental investigations into some simple molecules containing phosphorus reveal much about the rami½cations of this element’s position in the periodic table and that of its neighbors. Addition - ally, there are many phosphorus compounds of commercial importance, and the industry surrounding this element resides at a crucial nexus of natural resource stewardship, technology, and modern agriculture. Questions about our sources of phosphorus and the applications for which we deploy it raise the provocative issue of the human role in the ongoing depletion of phosphorus deposits, as well as the transfer of phos- phorus from the land into the seas. Inorganic chemistry can be de½ned as “the chem- istry of all the elements of the periodic table,”1 but as such, the ½eld is impossibly broad, encompassing everything from organic chemistry to materials sci- ence and enzymology.
Nitrogen and Phosphorus Fertilization Increases the Uptake of Soil Heavy Metal Pollutants by Plant Community

Nitrogen and phosphorus fertilization increases the uptake of soil heavy metal pollutants by plant community Guangmei Tang Yunnan University Xiaole Zhang Chuxiong Normal University Lanlan Qi Yunnan Normal University Chenjiao Wang Yunnan Normal University Lei Li Yunnan Normal University Jiahang Guo Yunnan Normal University Xiaolin Dou Research Centre for Eco-Environmental Sciences Chinese Academy of Sciences Meng Lu Yunnan University Jingxin Huang ( [email protected] ) Yunnan University https://orcid.org/0000-0001-5641-2731 Research Keywords: soil heavy metals pollution, phytoremediation, nitrogen and phosphorus fertilizer Posted Date: April 19th, 2021 DOI: https://doi.org/10.21203/rs.3.rs-413625/v1 License: This work is licensed under a Creative Commons Attribution 4.0 International License. Read Full License Page 1/20 Abstract Background: Soil heavy metal pollution is widespread around the world. Heavy metal pollutants are easily absorbed by plants and enriched in food chain, which may harm human health, cause the loss of plant, animal and microbial diversity. Plants can generally absorb soil heavy metal pollutants. Compared with hyperaccumulation plants, non-hyperaccumulator plant communities have many advantages in the remediation of heavy metals pollution in soil. However, the amount of heavy metals absorbed could be less, and the biomass would be reduced under heavy metal pollution. The application of nitrogen (N) and phosphorus (P) is inexpensive and convenient, which can increase the resistance of plants to adversity and promote the growth of plants of heavy metal polluted soils. Methods: We designed a comparative greenhouse experiment with heavy metal contaminated soils, and set up four treatments: CK treatment (soil without fertilizer), N treatment (soil with N addition), P treatment (soil with P addition), and N+P treatment (soil with N and P addition).
Chapter 18: the Representative Elements

Chapter 18: The Representative Elements Big Idea: The structure of atoms determines their o Hydrogen properties; o Group 1A consequently, the o Group 2A behavior of elements is o Group 3A related to their o Group 4A location in the o Group 5A periodic table. In general nonmetallic o Group 6A character becomes o Group 7A more pronounced o Group 8A toward the right of the periodic table. 1 The Representative Elements 2 Chapter 18: The Representative Elements The Representative Elements 3 Chapter 18: The Representative Elements Hydrogen Electron configuration is 1s1(similar to the electron configurations of group 1A elements) Classified as a non metal Therefore it doesn’t fit into any group 4 Chapter 18: The Representative Elements Hydrogen Most H is made up of only two particles (an electron and a proton) H is the most abundant element in the universe and accounts for 89% of all atoms Little free H on earth H2 gas is so light that it moves very fast and can escape the Earth’s gravitational pull Need heavier planets to confine H2 5 Chapter 18: The Representative Elements Group 1A The Alkali Metals Electron configuration is ns1(n = period number). Lose their valence e- easily (great reducing agents). Most violently reactive of all the metals. React strongly with H2O(l); the vigor of the reaction increases down the group. The alkali metals are all too easily oxidized to be found in their free state in nature. 6 Chapter 18: The Representative Elements Group 1A Lithium Sodium Strong polarizing power Mined as rock salt Forms bonds with which is a deposit of highly covalent sodium chloride left as character ancient oceans evaporated Used in ceramics, Lubricants, Medicine Extracted using (lithium carbonate electrolysis of molten (treatment for bipolar NaCl (Downs process) disorder)) 7 Chapter 18: The Representative Elements Group 1A Important Group NaCl NaOH NaHCO3 (Baking Soda) - - HCO3 (aq) + HA(aq) A (g) + H2O(l) +CO2(g) The weak acid (HA) must be present in the dough; Some weak acids are sour milk, buttermilk, lemon jucie, or vinegar.
Phosphorus Tips for People with Chronic Kidney Disease (CKD)

Phosphorus Tips for People with Chronic Kidney Disease (CKD) What Is Phosphorus? Phosphorus is a mineral that helps keep your bones healthy. It also helps keep blood vessels and muscles working. Phosphorus is found naturally in foods rich in protein, such as meat, poultry, fish, nuts, beans, and dairy products. Phosphorus is also added to many processed foods. Why Is Phosphorus Important for People with CKD? When you have CKD, phosphorus can build up in your blood, making your bones thin, weak, and more likely to break. It can cause itchy skin, and bone and joint pain. Most people with CKD need to eat foods with less phosphorus than they are used to eating. Your health care provider may talk to you about taking a phosphate binder with meals to lower the amount of phosphorus in your blood. Foods Lower in Phosphorus • Fresh fruits and vegetables • Corn and rice cereals • Rice milk (not enriched) • Light-colored sodas/pop • Breads, pasta, rice • Home-brewed iced tea Foods Higher in Phosphorus • Meat, poultry, fish • Bran cereals and oatmeal • Dairy foods • Colas • Beans, lentils, nuts • Some bottled iced tea 1 Phosphorus How Do I Lower Phosphorus in My Diet? • Know what foods are lower in phosphorus (see page 1). • Eat smaller portions of foods high in protein at meals and for snacks. – Meat, poultry, and fish: A cooked portion should be about 2 to 3 ounces or about the size of a deck of cards. – Dairy foods: Keep your portions to ½ cup of milk or yogurt, or one slice of cheese. – Beans and lentils: Portions should be about ½ cup of cooked beans or lentils.
Phosphorus in the Kidney Disease Diet: Become a Phosphorus Detective

Phosphorus in the Kidney Disease Diet: Become a Phosphorus Detective Carolyn Feibig, MS, RD, LD Transplant Dietitian The George Washington University Hospital Thanks to our speaker! Carolyn Feibig, MS, RD, LD • Kidney Transplant Dietitian at the George Washington University Hospital • Passionate about educating the general public about the importance of early detection of kidney disease and the importance of a healthy diet for kidney health Objectives Managing your phosphorus can be overwhelming! Today we will look at: – what is phosphorus, why it is important – how you can manage your phosphorus with kidney disease/ on dialysis – what can happen if your phosphorus is out of range (high or low) After today you will be a Master Phosphorus Detective – with the skills to find all sources of phosphorus and how to keep your phos in range. Phosphorus • Phosphorus is vital to the production and storage of energy in the human body. It is a main component in ATP (Adenosine Triphosphate). It is widely available in food, and is a important to bone building and health. • About 85% to 90% of total body phosphorus is found in bones and teeth. • Phosphorus is also a component of fats, proteins, and cell membranes. Phosphorus • High levels of phosphorus in your blood are not IMMEDIATELY harmful but can cause SEVERE long term problems. • The recommended range for dialysis patients is 3.0 to 5.5 mg/dL. • The following slides discuss what happens when your phosphorus is high BUT low phos can be cause for immediate concern: – Although rare, a severe drop in serum phosphorus 1.5 mg/dL or below, can cause neuromuscular disturbances, coma and death due to impaired cellular metabolism.
Phosphorus-Element Bond-Forming Reactions

King Hall 04 Thursday, Nov 7, 2019 1:30pm Department of Chemistry Coffee and Cookies provided & 1:15pm Phosphorus-Element Bond-Forming Reactions Professor Christopher Cummins Henry Dreyfus Professor of Chemistry Massachusetts Institute of Technology Department of Chemistry 2019 Chemistry Department King Lecturer Abstract Reactive Intermediates & Group Transfer Reactions. We design and synthesize molecular precursors that can be activated by a stimulus to release a small molecule of interest. The molecular precursors themselves are isolated as crystalline solids; they are typically soluble in common organic solvents and can be weighed out and used as needed. For example, the molecule P2A2 (A = anthracene or C14H10) is a molecular precursor to the diatomic molecule P2. Compounds having the formula RPA serve to transfer the phosphinidene (PR) group either as a freely diffusing species (R = NR’2, singlet phosphinidene) or else by inner sphere mechanisms (R = alkyl, triplet phosphinidene). Using the RPA reagents we are developing reactions analogous to cyclopropanation and aziridination for delivery of the PR group to olefins with the formation of three-membered P-containing rings, phosphiranes. Sustainable Phosphorus Chemistry. The industrial “thermalIN process” by which the raw material phosphate rock is upgraded to white phosphorus is energy intensive and generates CO2. We seek alternative chemical routes to value-added P-chemicals from phosphate starting materials obtained either by the agricultural “wet process” or by phosphorus recovery and recycling from waste streams. Trichlorosilane is a high production volume chemical for its use in the manufacture of silicon for solar panels. We show that trichlorosilane is a reductant for phosphate raw - materials leading to the bis(trichlorosilyl) phosphide anion [P(SiCl3)2] as a versatile intermediate en route to compounds containing P-C bonds.
Role of Silicon in Mediating Phosphorus Imbalance in Plants

plants Review Role of Silicon in Mediating Phosphorus Imbalance in Plants An Yong Hu 1, Shu Nan Xu 1, Dong Ni Qin 1, Wen Li 1 and Xue Qiang Zhao 2,3,* 1 School of Geographical Science, Nantong University, Nantong 226019, China; [email protected] (A.Y.H.); [email protected] (S.N.X.); [email protected] (D.N.Q.); [email protected] (W.L.) 2 State Key Laboratory of Soil and Sustainable Agriculture, Institute of Soil Science, Chinese Academy of Sciences, Nanjing 210008, China 3 University of Chinese Academy of Sciences, Beijing 100049, China * Correspondence: [email protected] Abstract: The soil bioavailability of phosphorus (P) is often low because of its poor solubility, strong sorption and slow diffusion in most soils; however, stress due to excess soil P can occur in greenhouse production systems subjected to high levels of P fertilizer. Silicon (Si) is a beneficial element that can alleviate multiple biotic and abiotic stresses. Although numerous studies have investigated the effects of Si on P nutrition, a comprehensive review has not been published. Accordingly, here we review: (1) the Si uptake, transport and accumulation in various plant species; (2) the roles of phosphate transporters in P acquisition, mobilization, re-utilization and homeostasis; (3) the beneficial role of Si in improving P nutrition under P deficiency; and (4) the regulatory function of Si in decreasing P uptake under excess P. The results of the reviewed studies suggest the important role of Si in mediating P imbalance in plants. We also present a schematic model to explain underlying mechanisms responsible for the beneficial impact of Si on plant adaption to P-imbalance stress.
Nitrogen and Phosphorus in Agricultural Streams

Report on the Environment https://www.epa.gov/roe/ Nitrogen and Phosphorus in Agricultural Streams Nitrogen is a critical nutrient that is generally used and reused by plants within natural ecosystems, with minimal “leakage” into surface or ground water, where nitrogen concentrations remain very low (Vitousek et al., 2002). When nitrogen is applied to the land in amounts greater than can be incorporated into crops or lost to the atmosphere through volatilization or denitrification, however, nitrogen concentrations in streams can increase. The major sources of excess nitrogen in predominantly agricultural watersheds are fertilizer and animal waste; other sources include septic systems and atmospheric deposition. The total nitrogen concentration in streams consists of nitrate, the most common bioavailable form; organic nitrogen, which is generally less available to biota; and nitrite and ammonium compounds, which are typically present at relatively low levels except in highly polluted situations. Excess nitrate is not toxic to aquatic life, but increased nitrogen may result in overgrowth of algae, which can decrease the dissolved oxygen content of the water, thereby harming or killing fish and other aquatic species (U.S. EPA, 2005). Excess nitrogen also can lead to problems in downstream coastal waters, as discussed further in the N and P Loads in Large Rivers indicator. Phosphorus also is an essential nutrient for all life forms, but at high concentrations the most biologically active form of phosphorus (orthophosphate) can cause water quality problems by overstimulating the growth of algae. In addition to being visually unappealing and causing tastes and odors in water supplies, excess algal growth can contribute to the loss of oxygen needed by fish and other animals.
Periodic Table Facts

Periodic Table Facts Compact Periodic Table Table Layout The periodic table is normally presented in a compressed form with Transition Metals the Lanthanides (elements 57-71) and Actinides (elements 89-103) in separate rows below the rest of the table. This is A. Earth Metals Metals Earth A. done to make the table more Lanthanides compact. In the extended table, Actinides shown below, these elements are inserted in their proper position between the Alkaline Earth Metals and the Transition Metals. Extended Periodic Table Transition Metals Lanthanides A. Earth Metals Metals Earth A. Actinides increasing mass How Small Are Atoms? Atoms are very, very small. To similar understand how small atoms are, start properties by looking at a meter stick. A meter can be divided into 1000 smaller lengths called millimeters. Now think of that millimeter and divide it into 1000 smaller lengths called micrometers. Now think of that micrometer and Periodic Trends divide it into 1000 even smaller lengths Dmitri Mendeleëv organized elements called nanometers. One nanometer is in the Periodic Table according to large enough for about 5 carbon their mass and reactive properties. He atoms. recognized that some elements had It would take 7,000,000 (7 million) similar properties, so he placed them carbon atoms stacked on top of each in the same column. He placed the other to be the thickness of a dime. elements from left to right in order of increasing mass. Mendeleëv left It would take 120,000,000 (120 million) spaces in his original table for carbon atoms to cross the face of elements that hadn’t yet been a dime.
Answers STRUCTURES of the PERIOD 3 ELEMENTS

Chemguide – answers STRUCTURES OF THE PERIOD 3 ELEMENTS 1. a) You should have picked out phosphorus, sulphur, chlorine and argon. You could use the diagrams on the Chemguide page you have just read, but you need to be quite good to draw these convincingly without a computer. Instead, use diagrams like these: b) Silicon is the only one with a giant covalent structure – the same as diamond: 2. a) Each of these is an example of metallic bonding. This involves the attraction between a delocalised sea of electrons and the nuclei of the atoms. From sodium to aluminium, the number of electrons delocalised per atom rises from 1 to 3, and so the “sea” is getting more negatively charged. The number of protons in the nucleus is increasing – so more positively charged. The atoms are getting smaller – so the distance between the nuclei and the “sea” is falling. All of these things make the attraction between the nuclei and the “sea” stronger, and more difficult to break. So more heat is needed to turn the metal into a gas. b) All of these molecules are attracted to each other by van der Waals dispersion forces which rely on the number of electrons moving around, and the distance over which they can move. On the whole, bigger molecules have bigger temporary dipoles, and so stronger intermolecular attractions. The biggest molecule is sulphur, S8; next biggest is phosphorus, P4; next is chlorine, Cl2; and the smallest is the single argon atom in the argon molecule. So sulphur has the highest melting and boiling points, phosphorus next, then chlorine and argon.
The Elements.Pdf

A Periodic Table of the Elements at Los Alamos National Laboratory Los Alamos National Laboratory's Chemistry Division Presents Periodic Table of the Elements A Resource for Elementary, Middle School, and High School Students Click an element for more information: Group** Period 1 18 IA VIIIA 1A 8A 1 2 13 14 15 16 17 2 1 H IIA IIIA IVA VA VIAVIIA He 1.008 2A 3A 4A 5A 6A 7A 4.003 3 4 5 6 7 8 9 10 2 Li Be B C N O F Ne 6.941 9.012 10.81 12.01 14.01 16.00 19.00 20.18 11 12 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 3 Na Mg IIIB IVB VB VIB VIIB ------- VIII IB IIB Al Si P S Cl Ar 22.99 24.31 3B 4B 5B 6B 7B ------- 1B 2B 26.98 28.09 30.97 32.07 35.45 39.95 ------- 8 ------- 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 39.10 40.08 44.96 47.88 50.94 52.00 54.94 55.85 58.47 58.69 63.55 65.39 69.72 72.59 74.92 78.96 79.90 83.80 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 5 Rb Sr Y Zr NbMo Tc Ru Rh PdAgCd In Sn Sb Te I Xe 85.47 87.62 88.91 91.22 92.91 95.94 (98) 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 6 Cs Ba La* Hf Ta W Re Os Ir Pt AuHg Tl Pb Bi Po At Rn 132.9 137.3 138.9 178.5 180.9 183.9 186.2 190.2 190.2 195.1 197.0 200.5 204.4 207.2 209.0 (210) (210) (222) 87 88 89 104 105 106 107 108 109 110 111 112 114 116 118 7 Fr Ra Ac~RfDb Sg Bh Hs Mt --- --- --- --- --- --- (223) (226) (227) (257) (260) (263) (262) (265) (266) () () () () () () http://pearl1.lanl.gov/periodic/ (1 of 3) [5/17/2001 4:06:20 PM] A Periodic Table of the Elements at Los Alamos National Laboratory 58 59 60 61 62 63 64 65 66 67 68 69 70 71 Lanthanide Series* Ce Pr NdPmSm Eu Gd TbDyHo Er TmYbLu 140.1 140.9 144.2 (147) 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.0 175.0 90 91 92 93 94 95 96 97 98 99 100 101 102 103 Actinide Series~ Th Pa U Np Pu AmCmBk Cf Es FmMdNo Lr 232.0 (231) (238) (237) (242) (243) (247) (247) (249) (254) (253) (256) (254) (257) ** Groups are noted by 3 notation conventions.