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Acids and Bases - Coggle Diagram
Acids and Bases
Types of acids
Binary acids
An acid that contains hydrogen and a highly electronegative element such as fluorine(ex: HF, HBr, HCl, HI
Oxyacids
A acid that contains three elements; usually hydrogen, oxygen and a nonmetal
Ionizable acids
Polyprotic acids
Acids that contain more than one ionizable hydrogen ion(ex: Methane, Acetic acid, Phosphoric acid)
Monoprotic acids
An acid that can only donate one proton/hydrogen ion per molecule(ex: HCl, HNO3, HPO4)
Only hydrogens that are highly polar can be ionizable,meaning their bonded to a highly electronegative element
After each ionization, the strength of the acid gets weaker since the polarity of the bonds decreases
Common Industrial Acids
Phosphoric Acid: Essential for plants and animals; mostly used for manufacturing fertilizers; used as a flavoring agent in beverages
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Nitric Acid: Stains proteins yellow; used for making explosives; a volatile, unstable liquid so dissolving it in water makes it more stable
Acetic Acid: Can form crystals in a cold room; used in manufacturing plastics; raw material in food production supplements
Sulfuric acid: used in large quantities in petroleum; essential for production of metals; automobile batteries; can be used to remove water from gases making it a great dehydrating agent
Acid/Base Definitions
Arrhenius
Arrhenius Acid: A compound that increases the number of hydrogen ions in the solution forms a hydronium ion(H3O)
Arrhenius acids are compounds with ionizable hydrogens; their water solutions are aqueous acids which are all electrolytes
Water molecules attract the hydrogens from the acids since they are polar, which is why the stronger polarity = > ionizable
Arrhenius Base: A substance that increases the number of hydroxide(OH-) ions present in the solution
BrØnsted-Lowry
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In a reaction, the proton is transferred from the acid to the base from reactant to product
Lewis
Lewis Acids accepts an electron pair to form a covalent bond; based on the bonding structure; don't contain any hydrogen at all; are the broadest of the three definitions
Any substance that can accept electron pairs are lewis acids including hydrogen protons or elements such as silver; can apply to substances in any phase
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Lewis Acid-base reaction: The formation of one or more covalent bonds between an electron pair donor and acceptor
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