1 / 13

Warm Up:

Warm Up:. Why do chemical equations need to be balanced? Balance the following equation: __PbCl 2 + __ AgNO 3 __ Pb (NO 3 ) + __ AgCl. Types of Chemical Reactions. Learning Target: To be able to identify the different type of reactions when looking at skeletal equations.

rosalba-frank
Télécharger la présentation

Warm Up:

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Warm Up: • Why do chemical equations need to be balanced? • Balance the following equation: __PbCl2 + __ AgNO3 __Pb(NO3) + __ AgCl

  2. Types of Chemical Reactions Learning Target: To be able to identify the different type of reactions when looking at skeletal equations

  3. Types of Reactions: • There are 5 types of Reactions: • Synthesis • Decomposition • Single-replacement • Double-replacement • Combustion

  4. Synthesis: A chemical rxn in which 2 or more substances (A + B) react to produce a single product (AB) A + B ⇒ AB Na(s) + Cl2(g) ⇒ NaCl(s) SO2(g) + O2(g) ⇒ SO3(g)

  5. Decomposition: A rxn in which a single compound (AB) breaks down into 2 or more new substances (A + B…) AB ⇒ A + B NH4NO3(s) ⇒ N2O(g) + H2O(g) Na3N(s) ⇒ Na(s) + N2(g)

  6. Single Replacement: A rxn in which the atoms of one element replace the atoms of another element in a compound A + BX ⇒ AX + B Li(s) + H2O(l) ⇒ LiOH(aq) + H2(g) Cu(s) + AgNO3(aq) ⇒ Ag(s) + Cu(NO3)2

  7. Double Replacement: a rxn which involves an exchange of ions between 2 compounds AX + BY ⇒ AY + BX *Either the metals change places or the nonmetals change places but not both!!! Ca(OH)2(aq) + HCl(aq) ⇒ CaCl2(aq) + H2O(l) *Typically occurs in aqueous solutions (in water) NaOH(aq) + CuCl2(aq) ⇒ NaCl(aq) + Cu(OH)2(s) *Precipitate: Is when a solid forms from a solution

  8. 3 Types of Double Replacement: • Formation of a precipitate • Formation of H2O • Formation of a product which decomposes into a gas

  9. Double-Replacement: Formation of a precipitate • Solubility Rules: • Some compounds will dissolve in water (soluble) • Some will NOT dissolve in water (insoluble/ not soluble) • If during a double-replacement rxn is formed, it will fall out of the solution as a solid, which is called a percipitant.

  10. Double-Replacement: Formation of H2O • These occur between Acids and Bases • Acids ALWAYS start with _________ • Bases are compounds that end with hydroxides (OH-) • One product will be H2O and one will be an ionic compound salt HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) *Some people consider this a separate rxn altogether

  11. Combustion: a rxn in which O2 can combine with a substance to release energy • Ex: Fire, Burning, Magnesium Stripe, etc. C(s) + O2(g) ⇒ CO2(g) CH4(g) + O2(g) ⇒ CO2(g) + H2O(l) *In most cases, the products will be H2O and CO2

  12. Activity Series: Single Replacement Rxn • Active metals will replace less active metals in reactions. Pt(s) + Zn2O (aq) → NR Fe(s)  +  CuSO4(aq)  →    FeSO4(aq)  +  Cu(s) Na(s) + SnCO3(aq) → Na2CO3(aq) + Sn(s)

  13. Practice Problems: Complete these in your notes and see how many you get right! • C2H6(g) + O2(g) → H2O(g) +CO2(g) • Br2(l) + LiI(s) → LiBr + I2(s) • Fe(s) + H2O(l) →Fe3O4(s) + H2(g) • MgCO3(s) → MgO(s) + CO2(g) • P4(s) + O2(g) → P4O10(s) • KNO3(s) → KNO2(s) + O2(g) • KOH + H3PO4 →K3PO4 + H2O • Na(s) + O2(g) →Na2O(s) • O2(g) + C6H12O6(g) → H2O(g) + CO2(g)

More Related