1 / 13

Equations

Equations. Types of Reactions. Four major classes. Synthesis Decomposition Single Replacement Double Replacement. Synthesis. A marriage of two substances (reactants) to form one new substance (product) A + B  AB The reactants can either be elements or compounds.

devika
Télécharger la présentation

Equations

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. Equations Types of Reactions

  2. Four major classes • Synthesis • Decomposition • Single Replacement • Double Replacement

  3. Synthesis • A marriage of two substances (reactants) to form one new substance (product) • A + B  AB • The reactants can either be elements or compounds. • The product is always one compound. • Example: C + O2 CO2

  4. Decomposition • Opposite of synthesis • A divorce of one substance (reactant) to form two or more simpler substances (products) • AB  A + B • The reactant is always one compound. • The products can either be elements or compounds. • Example: 2 HgO  2 Hg + O2

  5. Single Replacement • One element takes the place of another in a compound • The element can replace the first part of a compound, or it can replace the last part of a compound. • A + BC  B + AC (cationic)

  6. Single Replacement, cont • D + BC  C + BD (anionic) • Element + compound  element + compound • 7 elements are diatomic: N2, H2, Cl2, O2, Br2, F2, I2 • Example: Zn + 2 HCl  ZnCl2 + H2

  7. Double Replacement • The positive and negative portions of two compounds switch places. • Compound + compound  compound + compound • AB + CD  AD + CB • Example: HCl + KOH  HOH + KCl

  8. Combustion Reactions • Two types of Combustion Reactions: 1. Complete Combustion CxHy + O2 CO2 + H2O Always involves a hydrocarbon fuel source and oxygen as reactants, and carbon dioxide and water as products. Occurs when oxygen levels are high.

  9. Combustion Reactions • 2. Incomplete Combustion CxHy + O2 CO + H2O Always involves a hydrocarbon fuel source and oxygen as reactants, and carbon monoxide and water as products. Occurs when oxygen levels are insufficient to support combustion.

  10. COMBUSTION: 1. complete CxHy + O2 CO2 + H2O2. incomplete CxHy + O2 CO + H2O • When the reaction description includes the terms combusts, burns, oxidizes, or reacts with air, add oxygen as a reactant. • Determine whether the reaction is complete or incomplete combustion; then write the products. • Balance the carbons. • Balance the hydrogens. • Balance the oxygens.

  11. COMBUSTION: 1. complete CxHy + O2 CO2 + H2O2. incomplete CxHy + O2 CO + H2O • A propane (C3H8)grill is lit on the outside deck. • C3H8 + O2 + H2O

  12. COMBUSTION: 1. complete CxHy + O2 CO2 + H2O2. incomplete CxHy + O2 CO + H2O • A propane (C3H8)grill is lit in a closed garage. • C3H8 + O2 + H2O

  13. COMBUSTION: 1. complete CxHy + O2 CO2 + H2O2. incomplete CxHy + O2 CO + H2O • A butane lighter (C4H10)burns completely. • C4H10 + O2 + H2O

More Related