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Chemical Reactions

This text provides an overview of four fundamental types of chemical reactions: synthesis, decomposition, single replacement, and double replacement. Key examples include the synthesis of magnesium nitride from magnesium and nitrogen, the decomposition of titanium(III) oxide into titanium and oxygen, and the single replacement reaction where lithium replaces potassium in a solution. The text also highlights a double replacement reaction involving barium chloride and rubidium hydroxide, emphasizing the importance of reference tables for reaction determination.

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Chemical Reactions

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  1. Chemical Reactions By: Ni

  2. Synthesis Magnesium + Nitrogen form into Magnesium Nitride Mg(S) + N2(g)

  3. Synthesis Magnesium + Nitrogen form into Magnesium Nitride 3Mg(S) + N2(g)Mg3N2(S) In synthesis 2 or more reactants make one larger product

  4. Decomposition Titanium(III) Oxide decomposes into Titanium metal and Oxygen Ti2O3(S)

  5. Decomposition Titanium(III) Oxide decomposes into Titanium metal and Oxygen 2Ti2O3(S) 4Ti(S) + 3O2(g) One reactant becomes two or more products.

  6. Single Replacement Lithium replaced the potassium in solution, the potassium is bumped out as a solid. The bromide is the spectator ion. Li(S) + KBr(AQ)

  7. Single Replacement Lithium replaced the potassium in the solution, the potassium is bumped out as a solid. The bromide is the spectator ionbecause it isn’t directly involved in the reaction. Li(S) + KBr(AQ)LiBr(AQ) + K(S) Always use table J to determine if this reaction happened.

  8. Double Replacement Barium Chloride and Rubidium Hydroxide BaCI2 + 2RbOH

  9. Double Replacement Barium Chloride and Rubidium Hydroxide BaCl2(AQ) + 2RbOH(AQ)Ba(OH)2(S) +2RbCl(AQ) Always use table F to determine if this reaction happened.

  10. Closure Those are the 4 types of chemical reactions which we studied already. -Synthesis -Decomposition -Single Replacement -Double Replacement

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