Copper Sulfate - Integrative Project Chemistry 1B

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COPPER SULFATE

• Hugo Adrian Fernandez Cordero 1B

History of Copper Sulfate

It was discovered in the year 400 B.C. by the Greek civilization

During the Middle Ages and the Renaissance in Europe, copper sulfate continued to be valued in the textile industry and in the preservation of food and wine. In the 19th century, it was used as a pesticide and fungicide in agriculture, particularly in viticulture, where it helped combat phylloxera.

Middle Ages:

History of the compound

Copper sulfate, known as "vitriol," was used by alchemists in practices related to the transmutation of metals and in dyeing textiles. Its blue color made it valuable in art and decoration. In the 19th century, it became popular in agriculture with the creation of the "Bordeaux mixture" (copper sulfate and lime) to combat diseases in crops, especially in vineyards. Currently, copper sulfate has applications in agriculture (fungicides), industry (electroplating, water treatment), and education (crystallization experiments).

Copper sulfate was already used in the ancient civilizations of Egypt, Greece, and Rome. In Egypt, artisans used it in paints and dyes, while the Greeks and Romans employed it to treat diseases and in water purification processes.

Antiquity:

Modern Age:

Summary of its evolution:

Antiquity: Use in dyes, medicine, and water purification. Middle Ages: Popular among alchemists and in textiles. Modern Age: Development of Bordeaux mixture in agriculture. Contemporary Era: Wide industrial, scientific, and agricultural applications.

Contemporary Era:

OXYGEN, COPPER, SULFUR

What is it made of?

Formula: Cu2SO4

Oxygen: An essential gas for respiration; forms compounds such as water and carbon dioxide.

Copper: A conductive metal, used in electricity and alloys; resistant to corrosion.

Copper sulfate, cuprous sulfate, or dicopper sulfate is an insoluble blue salt, formed by the sulfate anion and the copper cation in its oxidation state.

Sulfur: A non-metallic element; important in proteins and fertilizers; forms compounds such as sulfuric acid.

OXYGEN COPPER SULFUR

Atoms in copper sulfate:

Copper is a metallic element. It is found in rocks, soil, water, and air. Copper is an essential nutrient for humans and is present in many foods. It is also vital for animals and plants.

It is located in the periodic table within the group of nonmetals. Its color is yellow and it is quite abundant in volcanic areas of the Earth.

Oxygen is present in the air with concentrations of 21%. It is found in a gaseous phase with no odor, color, or taste. It is a highly reactive substance that reacts with almost all elements.

Quantum numbers of copper sulfate

Configuración electrónica:

Graphical electron configuration

1s²: ↑↓ 2s²: ↑↓ 2p⁶: ↑↓ ↑↓ ↑↓ 3s²: ↑↓ 3p⁶: ↑↓ ↑↓ ↑↓ 3d⁹: ↑↓ ↑↓ ↑↓ ↑↓ ↑

Cu (Copper): 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s¹

Ion Cu²⁺: Electron in the 3d orbital: n = 3 l = 2 mₗ = -2, -1, 0, +1, or +2 mₛ = +1/2 or -1/2 Ion SO₄²⁻: Electron in the 3p orbital (sulfur): n = 3 l = 1 mₗ = -1, 0, or +1 mₛ = +1/2 or -1/2 Electron in the 2p orbital (oxygen): n = 2 l = 1 mₗ = -1, 0, or +1 mₛ = +1/2 or -1/2

S (Sulfur): 1s² 2s² 2p⁶ 3s² 3p⁴

1s²: ↑↓ 2s²: ↑↓ 2p⁶: ↑↓ ↑↓ ↑↓ 3s²: ↑↓ 3p⁴: ↑↓ ↑ ↑

O (Oxygen): 1s² 2s² 2p⁴

1s²: ↑↓ 2s²: ↑↓ 2p⁴: ↑↓ ↑↓ ↑ ↑

Lewis structure of CuSO₄:

Paracelso (1493-1541)

M. Faraday (1791-1867)

August Wilhelm (1818-1892)

Contributions: He was a prominent German chemist known for his research in organic chemistry and for being one of the founders of modern organic chemistry.

Contributions: Faraday was a physicist and chemist whose research in electromagnetism and electrochemistry revolutionized science.

Contributions: Paracelsus was a Swiss physician, alchemist, and philosopher who revolutionized medicine and chemistry of his time.

His focus on the use of chemical substances and his insistence on experimentation and observation helped lay the foundation for the development of modern chemistry.

He discovered electrochemistry, Faraday's law, and conducted pioneering research on electric and magnetic fields.

He studied nitrogen compounds and developed methods for the synthesis of dyes and other chemical compounds.Relevant work: He made significant contributions to the understanding of the chemistry of metals, including copper. He helped expand knowledge about the properties and applications of metal compounds.

Who discover it?

In the context of copper sulfate, Faraday investigated electrochemical reactions in aqueous solutions, including those involving copper salts such as copper sulfate.

Relevance to copper sulfate: Although he did not directly study copper sulfate, Paracelsus worked with copper compounds and other minerals, which contributed to the evolution of knowledge about chemical compounds and their applications.

When was it discovered?

History of the compound

His work on electrolysis helped understand how copper sulfate can be decomposed into its components by passing an electric current through it.

Sulfur

Oxygen

En el año 1777 Antoine Lavoisier un quimico y fisico lo clasifico como un elemento químico. El azufre tiene muchos minerales en común.

Oxygen was discovered by Joseph Priestley in 1774. Its chemical symbol is O, with an atomic number of 8. It is an essential gas for respiration and forms water with hydrogen.

Discovery

Cupper

Copper does not have a specific discoverer or a defined year of discovery, as its use dates back to prehistory. The earliest uses of copper date back to around 9000 BC in the area of Anatolia (modern-day Turkey).

It gets its name from Lars Frederik Nilson, who worked with it in 1879.

Extra Information

Cupper - Cu

Oxygen-O

Everyday use: Coins, kitchen utensils, jewelry. In industry: It is used in motors, electronic systems, and electrical systems. Copper extraction: In surface and underground mining.

Everyday use: For breathing. Technological use: Oxygen therapy, medical equipment. In industry: Used in welding and cutting, steel production, water treatment. Oxygen extraction: Fractional distillation method. Membrane separation.

Sulfur-S

Everyday use: Found in cell phones, computers, and household appliances. Technological use: Computers and mobile devices. Automation and robotics. Extraction of Sulfur: Mining extraction. Fracturing process. Purification. Manufacturing of products.

Where is it located?

Soils and water bodies

In small quantities, copper sulfate may be present in soils or water, especially in areas near mines or industries that use this compound. It may also be found in agricultural areas where it is used for pest control.

Commercial gardening products

It is found in commercial products such as fungicides and pesticides that you can buy in gardening or agricultural stores. These products contain copper sulfate as an active ingredient.

Mining

In the mineral flotation process, copper sulfate is used to separate useful minerals, such as copper, from impurities. It is essential for obtaining valuable metals.

In electronics, sulfate is used for the manufacture of printed circuit boards or PCBs, used in processes for coating with a copper layer that conducts electricity.

Uses in specific products

In construction as an additive for the manufacture of concrete and mortar, which increases its useful life and its resistance to sulfates present in soils.

Use in the synthesis of other copper compounds and in the manufacture of dyes.

In production of herbicides for weeds, fungicides to treat fungal diseases in plants, fertilizers for copper deficiencies in agricultural soils.

Control algae and cyanobacteria growth which helps to improve water quality.

State of matter

State of Matter: Copper sulfate is commonly found in solid crystal form, especially as pentahydrate: CuSO4 ⋅ 5H2O.

Solubility: Very soluble in water (25 g in 100 mL of water at 20 °C). Density: Density of anhydrous copper sulfate: approximately 3.6 g/cm³. Density of copper sulfate pentahydrate: approximately 2.2 g/cm³.

Melting point: Copper sulfate (anhydrous): 650 °C.Copper sulfate pentahydrate: 30 °C (dehydrated). Boiling point: t has no defined boiling point, as it decomposes before reaching a boiling temperature. Color: Copper (II) sulfate is bright blue in its hydrated form.Odor:It has no odor.

Toxicity

Copper sulfate is a potent oxidizing agent and, depending on the amount ingested, can cause damage to the human body. The effects of poisoning are seen in red blood cells, gastrointestinal system, kidneys and cardiovascular system.

Health risks

Symptoms of exposure

Sulfate may cause headache, nausea, vomiting, diarrhea and abdominal pain. Also skin allergy and possible liver and kidney damage.

- Fire prevention

Rules for its use

The product is not flammable.

- Special exposure risks

May generate toxic gas.

- Special protective equipment for firefighters

Firefighters should wear appropriate protective equipment and self-contained breathing apparatus with face mask.

- Precautions to protect the environment

Prevent a significant quantity of the product from coming into contact with water bodies or pipes. In case of occurrence, immediately inform the competent authorities.

- Storage

Store the product in sealed containers away from moisture and sunlight.

Personal protection:

Respirator with particulate filter adapted to the concentration of the substance in air, protective suit, protective gloves and goggles with integral frame. DO NOT allow this chemical to enter the environment.

Preventive measures

REACTIVITY WITH OTHER COMPOUNDS

Cupric sulfate reacts with MAGENSIUM to produce hydrogen gas, which is flammable, explosive and reacts with ACETYLENE to form shock-sensitive copper acetylides. Cupric sulfate can ignite HYDROXYLAMINE.

El sulfato de cobre tiene enlaces metal-oxígeno con un carácter covalente significativo. Copper(II) sulfate, also known as cupric sulfate, is an inorganic compound with the chemical formula CuSO4(H2O)x. Its properties are:

• It is a crystalline solid.

• The most common form is copper(II) sulfate pentahydrate, which is bright blue and triclinic.

• The anhydrous form is white or pale gray-white and has a rhombic structure.

• It is characterized by rapid temperature changes when more water is added.

• It is hygroscopic.

• It is strongly irritating to living organisms.

• It is not biodegradable.

LINK TYPES

The chemical stability of copper sulfate depends on the conditions under which it is stored and its type:

• Copper sulfate pentahydrate.

• It is stable under normal storage conditions, but it loses water slowly at 30°C and decomposes completely at 250°C and above.

• Copper (I) sulfate.

• It is stable in dry air at room temperature, but decomposes rapidly in the presence of moisture or when heated.

• Copper (II) sulfate is not reactive under normal ambient conditions. However, it reacts with magnesium to produce hydrogen gas, with acetylene to form copper acetylides and can ignite hydroxylamine.

CHEMICAL STABILITY

OXIDATION AND REDUCTION POTENTIAL

Copper (II) sulfate (CuSO4) is an inorganic compound that forms in the second degree of oxidation. Copper (II) sulfate: Oxidation state: +2F Formula: CuSO4 Properties: Odorless crystalline powder, absorbs water, dissolves in methanol, does not dissolve in ethanol. Applications: Agricultural fungicide, algaecide, molluscicide, animal feed additive, preservative, glue and paint additive. Hazards: Extremely hazardous, toxic and non-biodegradable substance. Copper(I) sulfate (Cu2SO4) is a blue insoluble salt, which is formed when copper is in the +1 oxidation state. This oxidation state is not very stable, so copper (I) sulfate is much less common than copper (II) sulfate.

PRODUCTION AND EXTRACTION METHOD

This compound occurs naturally in large quantities, as it is a chemical compound formed through industrial processes or specific chemical reactions.

The production process of copper sulfate pentahydrate from copper scrap basically consists of seven stages: reception and selection of the scrap, reaction, crystallization, draining, drying, sifting and milling, weighing and bagging.

Agriculture: Used as a fungicide to protect crops from fungal diseases such as downy mildew on grapevines and black spot on citrus. It is also used as a component of manures and fertilizers, and as a herbicide to control invasive aquatic plants and algae in potted plants. Industry: It is used in metallurgy for galvanic baths, in the production of copper printed circuits and in the production of copper cathodes. Medicine: Used in blood tests to detect anemia. Household: Used as a disinfectant to clean equipment and surfaces in agricultural and livestock facilities. Printing: It is added to binding pastes and adhesives to protect the paper from insect attack. Construction: It is used as an additive for concrete to provide disinfectant properties and water resistance. Glass and ceramic production: It is used as a coloring ingredient. Fireworks: It is used to give them their blue color.

USE IN INDUSTRY, AGRICULTURE, MEDICINE AND THE HOME

Effects on the environment

The presence of copper in soils decreases the biomass and bacterial metabolic activity causing a lower yield of the biogeochemical processes in which bacteria participate. This leads to a loss of fertility of agricultural soils and damage to the ecosystem.

Biogradability or accumulation

Copper (II) sulfate pentahydrate decomposes before melting, gradually losing its water molecules at 63 °C, 109 °C and finally at 200 °C. Dehydration occurs by decomposition of the tetraaquacopper (2+) residue, forming a diaguacopper (2+) residue. Finally, at 650 °C, it decomposes into copper (II) oxide (CuO) and sulfur trioxide (SO3).

To remove copper, place a Superflock Plus flocculant cartridge in the skimmer. Let the circulation run uninterruptedly for at least 24 hours, until the water becomes clear again.

Avoid contact with skin, eyes and clothing. Do not breathe vapors/aerosols. Keep product away from drains, surface and ground water. Retain and dispose of contaminated wash water.

Prevention and control measures

Cupric sulfate may cause headache, nausea, vomiting, diarrhea and abdominal pain. Cupric sulfate may cause a skin allergy. Cupric sulfate may affect the liver and kidney.

Specific method Weigh the copper sulfate, dissolve it in 3/4 parts of water and complete the total volume with the rest of purified water. Store at temperature below 30 ºC and protect from light.

EXTRA IMAGES

Chemical representation

Adrian

In conclusion, Copper Sulfate is a very ancient compound that is still used today, discovered by the Greek civilization. Its functions range goes from medicine to agriculture. With its characteristic blue color coming from the water particles in its structure.

Conclusions

https://www.omega-air.es/noticias/noticias/aplicaciones-del-oxigeno#:~:text=El%20ox%C3%ADgeno%20est%C3%A1%20presente%20en,elementos%2C%20excepto%20los%20gases%20inertes.

https://www.atsdr.cdc.gov/es/toxfaqs/es_tfacts132.html#:~:text=El%20cobre%20(Cu)%20es%20un,los%20animales%20y%20las%20plantas.

https://www.zinsa.com/es/derivados-de-cobre/sulfato-de-cobre

Copper life cycle - international copper association. (n.d.). Retrieved September 10, 2024, from https://internationalcopper.org/es/sustainable-copper/about-copper/copper-life-cycle/

Rodríguez, H. (2022, May 14). Oxígeno (O): Propiedades químicas del elemento de la tabla periódica. National geographic. https://www.nationalgeographic.com.es/ciencia/propiedades-oxigeno-o_18219

Rodríguez, H. (2022a, May 14). Azufre (S). Propiedades químicas del Azufre de la tabla periódica. National geographic. https://www.nationalgeographic.com.es/ciencia/propiedades-azufre-s_18220

https://mexico.pochteca.net/usos-del-sulfato-de-cobre-en-las-industrias/

Bibliographies

Bibliographies

Royal Society of Chemistry. (n.d.). Copper(II) sulfate. Retrieved October 14, 2024, from https://www.rsc.org/periodic-table/element/29/copper National Center for Biotechnology Information. (n.d.). Copper sulfate. In PubChem compound summary. Retrieved October 14, 2024, from https://pubchem.ncbi.nlm.nih.gov/compound/Copper-sulfate Royal Society of Chemistry. (n.d.). Copper(II) sulfate. In ChemSpider. Retrieved October 14, 2024, from http://www.chemspider.com/Chemical-Structure.24813.html Baird, R. (2015). The use of copper(II) sulfate in education: A critical review. Journal of Chemical Education, 92(10), 1640-1644. https://doi.org/10.1021/acs.jchemed.5b00127 Alvaro, E. (n.d.). Copper sulfate: Environmental impact and uses. In ScienceDirect. Retrieved October 14, 2024, from https://www.sciencedirect.com/topics/earth-and-planetary-sciences/copper-sulfate American Chemical Society. (n.d.). The science of copper sulfate. Retrieved October 14, 2024, from https://www.acs.org/content/acs/en/education/whatischemistry/chemical-society/copper-sulfate.html Wikipedia contributors. (2024, October 14). Copper(II) sulfate. Wikipedia, The Free Encyclopedia. Retrieved October 14, 2024, from https://es.wikipedia.org/wiki/Sulfato_de_cobre https://www.google.com/search?sca_esv=04a744430a52c168&rlz=1C1EJFC_enMX916MX917&q=medidas+de+prevencion+y+control+del+sulfato+de+cobre&source=lnms&fbs=AEQNm0CbCVgAZ5mWEJDg6aoPVcBgWizR0-0aFOH11Sb5tlNhd7L9QFlHbGCCw2CV3tLpo-Edf3PZjBOdqq5j9Bo9oYv4OpEg-GZ1AvBfuuoWF_KsKSWEhkd39XWuNVQ6gR_WgQVn7U3vWSxfRzUadrMOc_5yPZ84XtBnKKaCKgsq53S6zd4_6wmMfrRAO2db4_dOu60L3WmlOl6C_9zydQunba62MPcRpg&sa=X&ved=2ahUKEwj2zIWcuI-JAxXBL9AFHbgvH6cQ0pQJegQIERAB&biw=1920&bih=953&dpr=1