Taco sauce penny cleaner
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This document discusses copper oxidation and how copper turns green through exposure to oxygen in the air. It explains that copper oxide forms on pennies and turns them green over time. The document also discusses how hydrochloric acid, formed from a mixture of vinegar and salt, can be used to clean oxidized pennies and surfaces by removing the copper oxide layer. Finally, it notes that hydrochloric acid has cleaning applications in buildings like hospitals by removing messes and debris.
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Chemical reactions of Metal for Class 10th CBSE
Metals react with oxygen in the air to form metal oxides. For example, magnesium reacts with oxygen to form magnesium oxide. Some metals like sodium and potassium react vigorously with air and must be stored in oil. Most metal oxides react with both acids and bases. For example, aluminum oxide reacts with hydrochloric acid to form aluminum chloride and water. Metals also react with acids, producing salts and hydrogen gas. Lighter metals like sodium and potassium react quickly, while heavier metals like magnesium, aluminum, and zinc react more slowly.
Ions to know
Thomas Edison conducted over 10,000 experiments to develop a successful battery and around 100 experiments to create an effective light bulb. Through perseverance and many trials, he was able to make significant contributions to electrical technology and innovation through hard work and repeated testing of ideas.
Silicon Presentation
Silicon has an atomic number of 14, atomic mass of 28.085, and symbol Si. It has a melting point of 1410°C and boiling point of 3265°C. Silicon is commonly found in computers, cars, cosmetics, and foods. It is the second most abundant element on Earth, making up over 80% of the crust, and is found in many common minerals like granite and clay.
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This document discusses acid reactions with metals, metal carbonates, and metal hydrogen carbonates. It explains that acids react with metals to produce salts and hydrogen gas. Acids react with metal carbonates to produce salts, water, and carbon dioxide gas. Acids react similarly with metal hydrogen carbonates, producing salts, water, and carbon dioxide gas. Examples of these types of acid reactions are provided, along with the balanced chemical equations. The document is intended for a year 9 chemistry class and includes instructions for an upcoming worksheet and game activity based on the students' performance.
22 ions to know for quiz
Thomas Edison worked very hard through many experiments to develop successful inventions. He conducted over 100 experiments to create a working light bulb with the right combination of metals and gases. He also did around 10,000 experiments to develop a battery that could effectively provide electric current.
REACTION OF METALS WITH ACID
Metals have several key properties including high thermal and electrical conductivity, sonority, high melting points, ductility, and malleability. When metals react with acids, bubbles of hydrogen gas are produced along with salts of the metal. For example, zinc reacts with hydrochloric acid to form zinc chloride and hydrogen gas. Different metals react to varying degrees with acids, with magnesium reacting vigorously and copper not reacting at all.
Chemical reaction between metals and water/acid
- Lighter metals like sodium, potassium, and calcium react vigorously with acids, while heavier metals like magnesium, aluminum, zinc, and lead react more slowly.
- Dilute acids are weaker as they are mixed with water, while concentrated acids are strong and pure.
- Most reactions of metals with dilute acids are single replacement reactions where the metal replaces hydrogen in the acid, producing hydrogen gas.
- Reactions of metals with concentrated acids can involve both single replacement and decomposition reactions.
- Lighter metals like sodium react vigorously with cold water, producing hydroxides and hydrogen gas, while their reaction with steam produces metal oxides and hydrogen gas.
Cobalt Assignment
Cobalt has been used for centuries in ceramics, pottery glazes, dyes and glassware. It was first isolated as an element in 1735. Cobalt is commonly used today in magnets, MRI machines, batteries and paints due to its strong magnetic properties. Cobalt is generally found in ores combined with arsenic, oxygen or sulfur and extracted as a byproduct during the refining of other ores.
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Chemical reactions of Metal for Class 10th CBSE
Metals react with oxygen in the air to form metal oxides. For example, magnesium reacts with oxygen to form magnesium oxide. Some metals like sodium and potassium react vigorously with air and must be stored in oil. Most metal oxides react with both acids and bases. For example, aluminum oxide reacts with hydrochloric acid to form aluminum chloride and water. Metals also react with acids, producing salts and hydrogen gas. Lighter metals like sodium and potassium react quickly, while heavier metals like magnesium, aluminum, and zinc react more slowly.
Ions to know
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Silicon has an atomic number of 14, atomic mass of 28.085, and symbol Si. It has a melting point of 1410°C and boiling point of 3265°C. Silicon is commonly found in computers, cars, cosmetics, and foods. It is the second most abundant element on Earth, making up over 80% of the crust, and is found in many common minerals like granite and clay.
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This document discusses acid reactions with metals, metal carbonates, and metal hydrogen carbonates. It explains that acids react with metals to produce salts and hydrogen gas. Acids react with metal carbonates to produce salts, water, and carbon dioxide gas. Acids react similarly with metal hydrogen carbonates, producing salts, water, and carbon dioxide gas. Examples of these types of acid reactions are provided, along with the balanced chemical equations. The document is intended for a year 9 chemistry class and includes instructions for an upcoming worksheet and game activity based on the students' performance.
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Chemical reaction between metals and water/acid
- Lighter metals like sodium, potassium, and calcium react vigorously with acids, while heavier metals like magnesium, aluminum, zinc, and lead react more slowly.
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- Reactions of metals with concentrated acids can involve both single replacement and decomposition reactions.
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The document discusses the reaction of various metals with acids. When metals like magnesium, aluminum, zinc, and iron react with hydrochloric acid, they produce bubbles of hydrogen gas. Copper does not react with dilute hydrochloric acid and produces no bubbles. Unlike reactions with hydrochloric acid, reactions of metals with nitric acid do not produce hydrogen gas. Aluminum also does not react with nitric acid due to the formation of a protective layer of aluminum oxide.
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Metals react with oxygen in the air to form metal oxides. For example, magnesium burns with an intense light when heated in air, forming magnesium oxide. Other metals like copper and aluminum also form oxides when heated in air. The reactivity of different metals with oxygen varies, with sodium and potassium being the most reactive and catching fire in open air. Less reactive metals like iron do not burn but will react when sprinkled as filings in a flame. Some metal oxides like aluminum oxide are amphoteric, reacting with both acids and bases.
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All the carbonates in this Group undergo thermal decomposition to give the metal oxide and carbon dioxide gas. Thermal decomposition is the term given to splitting up a compound by heating it.
All of these carbonates are white solids, and the oxides that are produced are also white solids.
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References
Tindale, Ritchie et al, 2014, Chemistry for CSEC 2nd Edition, Nelson Thornes. p156-159
Electron Transfer in Redox Reactions Todayhttps://www.sewanhakaschools.org
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Metals are usually found as metal oxides or sulfides in ores. To extract the metal, the ore undergoes a reduction reaction where a reducing agent removes the oxygen. Common reducing agents include carbon, carbon monoxide, and hydrogen. Extraction of iron uses carbon in a blast furnace, while aluminum requires an electrolysis process due to its high reactivity. Recycling scrap metals provides environmental and economic benefits by reducing waste and saving energy compared to extracting from ores.
Metal extraction slides
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- Iron rusts in the presence of oxygen and water to form iron(III) oxide. Rusting can be prevented by barriers like paint, grease, or sacrificial protection using more reactive metals like zinc.
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Nitrogen is a colorless, odorless non-metal gas that was discovered in 1772 by Daniel Rutherford. It has 7 protons, 7 electrons, 7 neutrons, and an atomic number of 7. Nitrogen is used in many common products like lightbulbs, refrigeration devices, and in manufacturing stainless steel. It is also used as a power source for paintball guns.
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The document summarizes the contact process for manufacturing sulfuric acid. It involves three main stages:
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3) Sulfur trioxide is absorbed into oleum and diluted with water to produce sulfuric acid.
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The document provides instructions for classifying elements and compounds and performing chemistry experiments. Students are asked to classify substances as elements or compounds and write the number of atoms in each. They are also given directions for experiments involving iron filings, sulfur, and hydrochloric acid to observe chemical reactions and changes in magnetic properties. The experiments aim to demonstrate the formation of new substances through chemical reactions.
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This document provides information about acid-base chemistry including definitions of terms like acids, bases, indicators, and saponification. It asks the reader to name carboxylic acids, give scientific reasons for uses of sodium bicarbonate and baking powder, and answer questions about how acids and bases react, the uses of various substances like bleaching powder and washing soda, and properties of substances like salt. It also asks about indicators, the pH scale, water of crystallization, and asks the reader to explain several chemical scenarios.
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This document summarizes key questions and answers from a YouTube chemistry lesson on nitric acid and its reactions with metals and other compounds.
The lesson covers the preparation of nitric acid, its reactions with copper and sulfur, and the identification and equations for reactions of nitric acid with compounds like copper carbonate, lead nitrate, potassium nitrate, and ammonium nitrate. Key reactions include the decomposition of nitric acid and metal nitrates like copper nitrate and lead nitrate when heated. Equations are provided for the oxidation of sulfur and copper by concentrated nitric acid.
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Copper to copper labs better stronger faster
1) Copper was one of the first metals isolated due to its ease of separation from ores as early as 4500 BC.
2) This experiment transforms copper metal through a series of reactions including metathesis, decomposition, displacement, and oxidation-reduction into copper compounds and back to copper metal.
3) The series of reactions begins and ends with copper metal and involves the use of nitric acid, sodium hydroxide, sulfuric acid, and zinc.
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hi guys,i have been getting useful materials for my students teaching, the least i can do for thanking all of you is by uploading this file on acids,bases and salts
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Metals
This is a summary of the topic "metals" in the GCE O levels subject: Chemistry. Students taking either the combined science (chemistry/physics) or pure chemistry will find this useful. These slides are prepared according to the learning outcomes required by the examinations board.
Cobalt
- Cobalt compounds have been used to color glass and ceramics for millennia, dating back to ancient Egypt and China.
- Swedish chemist Georg Brandt discovered cobalt as a new element in 1735 and showed that cobalt compounds were responsible for the blue color in glass.
- Cobalt occurs naturally in combination with other elements like sulfur and arsenic in minerals, but is most often obtained as a byproduct of copper and nickel mining.
acids bases and salts for class 10 pdf download
Numerous acids and bases are naturally present in our surroundings. Citric acid is abundant in fruits such as oranges and lemons, tartaric acid is found in tamarind, malic acid is present in apples, and lactic acid is a component of milk and dairy products. Additionally, hydrochloric acid naturally occurs in gastric juices.
Similarly, various bases are also naturally occurring, including lime water. In our daily lives, we frequently use these acids for various purposes. For instance, acetic acid, commonly known as vinegar, is a staple in the kitchen. Boric acid is utilized in laundry, while baking soda finds its way into cooking, and washing soda is employed for cleaning. The diverse applications of these acids and bases showcase their significance in our everyday activities.
For more information, visit. www.vavaclasses.com
Acids,bases and salts
This document provides information about acids, bases, salts, and the pH scale. It defines acids as substances that release hydrogen ions in solution, bases as substances that release hydroxide ions in solution, and salts as ionic compounds composed of metallic and nonmetallic ions. Key properties of acids, bases, and salts are described such as how they affect litmus paper and their uses. Methods of preparing acids, bases, and salts are also summarized. Finally, the pH scale is defined as a measure of the hydrogen ion concentration in solutions.
Chemistry experiments
1. Dilute hydrochloric acid was used to react with various substances including copper oxide, iron nails, magnesium strips, and egg shells. These reactions all produced observable changes and gaseous products like hydrogen and carbon dioxide.
2. The acid reacted with the copper oxide on a coin, removing the layer to expose bare copper. Reactions with iron nails removed rust and bubbles formed, while magnesium vigorously reacted with bubbles. Egg shells reacted to produce carbon dioxide bubbles.
3. Additional details are provided about the chemical reactions, products, and observations for each substance tested with the hydrochloric acid.
Metallurgy
Metallurgy is the process of extracting pure metals from their ores. Ores contain unwanted impurities and the required metal. The process involves both physical and chemical steps to separate the metal from impurities. One such process is the Parke's process for extracting silver, which involves heating an alloy of lead and silver to melt it, mixing it with molten zinc where the silver dissolves and separates from the lead due to different solubilities. Ellingham diagrams graphically show the thermodynamic stability of metal oxides and their variation with temperature, indicating the spontaneity of oxidation reactions. Iron is extracted from its ore, haematite, using a blast furnace where coke and limestone are added and hot
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1. The document describes different types of chemical reactions including synthesis, decomposition, single displacement, double displacement, combustion, acid-base, and neutralization reactions.
2. Metals react with oxygen to form metal oxides which are bases. Non-metals react with oxygen to form non-metal oxides which are acids.
3. Acid-base reactions involve acids and bases reacting to form salts and water in a neutralization reaction.
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This document discusses acids, bases, and salts. It defines acids as substances that produce hydrogen ions (H+) in aqueous solution, making them sour and able to turn litmus red. Bases are defined as substances that produce hydroxide ions (OH-) in solution, making them soapy and able to turn litmus blue. Salts are formed by the reaction of acids and bases and can be acidic, basic, or neutral depending on the reactants. Common natural and synthetic acid-base indicators are also described. The document then discusses the properties and reactions of acids, bases, and salts and how pH is used to measure acidity. Finally, several industrial chemicals derived from sodium chloride (common salt) are summarized, including
3. qualitative analysis
Qualitative analysis is used to identify the cations and anions present in an unknown chemical substance. Cations such as sodium, calcium, and ammonium can be identified using sodium hydroxide and ammonia solutions. Anions like chloride, nitrate, and sulfate can be identified through chemical tests involving silver nitrate, sodium hydroxide with aluminum foil, and barium chloride solutions respectively. These tests produce characteristic precipitates or gas emissions to reveal the ions present. Dilute nitric acid is first added to remove any interfering carbonate ions.
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The document discusses chemical reactions and provides examples to illustrate different types of chemical reactions:
1) Combination reactions involve reactants combining to form a single product, like burning of coal or formation of water.
2) Decomposition reactions involve a single reactant breaking down into simpler products, like heating ferrous sulfate crystals.
3) Displacement reactions involve one element displacing another from a compound, like an iron nail causing copper ions to displace from copper sulfate solution.
4) Precipitation reactions form an insoluble product or precipitate, like mixing sodium sulfate and barium chloride solutions.
5) Oxidation-reduction reactions involve transfer of electrons leading to oxidation and reduction of reactants.
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Taco sauce penny cleaner
- 2. copper Oxide The rust on a penny is formed when oxygen in the air reacts with the copper to form copper oxide (Science 1). When this rust turns green, it becomes copper carbonate (Science 2).
- 3. ue of Libe rtyLady Liberty is made out of copper. Over time the copper has turned green through the chemical process of copper oxidation.
- 4. Copper, Copper Everywhere! Copper fixtures are used in building materials, like in HVAC units, plumbing, and electrical wires as well as for decorative touches like gutters, and copper pans.
- 5. Presto! •When you place an oxidized penny into taco sauce, the penny becomes shiny again!
- 6. What’s in that sauce? The two ingredients in taco sauce that work together to clean a penny are vinegar and salt. When combined they create a mild hydrochloric acid.
- 7. Hydrochloric Acid The chemistry behind the vinegar salt cleaner is the compound Hydrochloric acid (HCl). A vinegar and salt mixture creates a weak HCL (Schcm 1). The equation that explains this is: “HC2H3O2 + NaCl HCl + NaCH3O2”. The vinegar formula, HC2H3O2, added to the formula for salt, NaCl, makes hydrochloric acid plus sodium acetate (Blindt 1).
- 8. Use HCl at home! Combine equal parts of vinegar and salt, then scrub away: Clean bathrooms, like around the toilet and sink In the kitchen it can be used for cleaning the counter, stove, refrigerator, etc…
- 9. HCl in the community… Hydrochloric Acid is also used in hospitals and nursing homes to clean up messes in the building ( National 2).
- 10. Work Cited Hints and Tips. Schsm, n.d. Web. 28 Apr. 2013. http://www.schsm.org/html/ hints_and_tips.html National Pollutant Inventory. N.p., n.d. Web. 11 Apr. 2013. http://www.nip.gov.au/substance/hydrochloric-acid/ Science.yourdictionary.com. Love To Know, 1996-2013. Web. 11 Apr. 2013. http://Science.yourdictionary.com/articles/why-does-copper- oxidize.html. Shiny Pennies. Jessica Blindt, n.d. Web. 28 Apr. 2013. http://www.elmhurst.edu/~chm/demos/ShinyPennies.html Steve Spangler Science. Steve Spangler, n.d. Web. 28 Apr. 2013. htt://www.stevespanglerscience.com/experiment/the- cleaning-power-of-taco-sauce-bright.html