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4.2 Synthesis and Decomposition Reactions
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Synthesis Reactions Involves smaller atoms or molecules combining to form a larger molecule Two or more reactants combine to make one product element + element → compound Synthesis reactions of non-metals create molecular compounds Synthesis reactions can involve compounds coming together compound + compound → new compound
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General Equation
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Synthesis Reactions involving Hydrogen
Usually forms a molecular compound
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Example Ex. 1) Hydrogen + oxygen → water
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Synthesis Reactions Involving Other Reactions
Can be more difficult to predict In these cases, the only way to identify the reaction products is by conducting chemical tests.
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Examples Sodium + chlorine → sodium chloride
3 )Copper + Oxygen → copper (ll) oxide
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Synthesis Involving Compounds
This is an important reaction that impacts aquatic ecosystems.
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Decomposition Reaction
Opposite to synthesis Involves a large molecule splitting to form smaller molecules or elements One reactant breaks apart into two or more products The general equation for a decomposition reaction is: compound → element + element
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Examples! 1) Water → Hydrogen + Oxygen
2) Triiodine mononitride→ Nitrogen + Iodine
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