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This video is something you will want to watch from about 2:20 - 9:00, about 7 minutes.
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Stuff from the first half of the year that we need to remember!
Types of Reactions:
Combination Combination reactions, also known as synthesis reactions, involve the combination of two or more substances into a single new substance: A + B ---> AB Many metal oxides, for example, absorb carbon dioxide (CO2) from the air to form carbonates: CaO(s) + CO2(g) ---> CaCO3(s) Decomposition Decomposition reactions represent the reverse of the combination process in that one substance breaks down into two or more substances: AB ---> A + B Water, or H2O, for example, decomposes into its constituent elements when subjected to an electric current: 2 H2O(l) ---> 2 H2(g) + O2(g) Combustion Combustion reactions occur when substances, particularly those containing carbon, burn in the presence of oxygen to produce carbon dioxide and water: CxHy + O2 ---> CO2(g) + H2O(g) Methane, for example, with chemical formula CH4 combusts as: CH4(g) + O2(g) ---> CO2(g) + 2 H2O(g) First 20 elements. >>>>>>>>>>>>>>>
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Single-Replacement
Single-replacement reactions occur when an element replaces one of the elements in a compound: A + BX ---> AX + B where X represents the atom being exchanged. Many metals, for example, react with acids to produce hydrogen and a metal salt: Zn(s) + 2 HCl(aq) ---> ZnCl2(aq) + H2(g) Double-Replacement Double-replacement reactions involve two compounds exchanging elements: AB + CD ---> AD + CB Double-replacement reactions commonly occur when one of the products is not soluble and precipitates out of the reaction solution as a solid: CaCl2(aq) + Na2CO3(aq) ---> CaCO3(s) + 2 NaCl(aq) |
pen_chromatography_lab.pdf | |
File Size: | 69 kb |
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