chemical reactions n.
Download
Skip this Video
Loading SlideShow in 5 Seconds..
Chemical Reactions PowerPoint Presentation
Download Presentation
Chemical Reactions

Loading in 2 Seconds...

play fullscreen
1 / 24

Chemical Reactions - PowerPoint PPT Presentation


  • 83 Views
  • Uploaded on

Chemical Reactions. Objectives. 1) Write and balance equations 2) Identifying the types of reactions. Reactants and Products. Gallium + Sulfuric acid → Gallium Sulfate + Hydrogen Reactants- left side of the arrow -starting materials Products-right side of the arrow

loader
I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
capcha
Download Presentation

PowerPoint Slideshow about 'Chemical Reactions' - ivrit


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.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
objectives
Objectives
  • 1) Write and balance equations
  • 2) Identifying the types of reactions
reactants and products
Reactants and Products

Gallium + Sulfuric acid → Gallium Sulfate + Hydrogen

  • Reactants- left side of the arrow

-starting materials

  • Products-right side of the arrow

-the substance made, produced

  • The number of atoms on the reactant side must equal the number of atoms on the product side.
balancing
Balancing

Rules:

  • 1) Write the correct chemical formula for the reactants and the products.
  • 2) Adjust the coefficients (the numbers that appear in front of the formulas) only and evenly.
  • 3) Never change the subscripts (the small numbers in a formula)
  • 4) When counting atoms, multiply the coefficients by the subscript for each element.
  • 5) There are seven elements, that when left alone, exist as diatomic molecules.

Br2 I2 N2 Cl2 H2 O2 F2

balancing example
Balancing Example
  • Ga + H2SO4 → Ga2(SO4)3 + H2

Balanced:

2Ga + 3H2SO4 → Ga2(SO4)3 + 3H2

identifying reactions
Identifying Reactions
  • The five types of reactions:

-Synthesis or Combination

-Single Replacement

-Double Replacement

-Combustion

-Decomposition (6 types)

synthesis
Synthesis
  • element + element → compound
  • Occurs when two or more elements are combined to form a new substance
  • Also called Combination

A + B AB

synthesis or combination
Synthesis or Combination
  • Example:

2 Na + Cl2 → 2NaCl

Jayhawk says: Here’s an example of synthesis:

+ = Rivalry

single replacement
Single Replacement
  • Occurs when one element displaces another in a compound.
  • A + BC → B + AC

element + compound → element + compound

single replacement1
Single Replacement

Example:

Na + LiCl → NaCl + Li

Listen up ,class, it’s time for an example.

double replacement
Double Replacement
  • Occurs when the positive and negative ions of the two reactants are interchanged
  • AB + CD → AD + CB
  • compound + compound→compound +compound
  • Never put two metals together
double replacement1
Double Replacement

Example:

2NaCl + Li2O → Na2O + 2LiCl

Did you know? Double replacement is also referred to as metathesis.

combustion
Combustion
  • Hydrocarbon + O2 → H2O + CO2
combustion1
Combustion

Example:

C4H8 + O2 →H2O + CO2

decomposition
Decomposition
  • Occurs when energy in the form of heat, light, electricity, or mechanical shock is supplied. A compound may decompose to form simpler compounds and/or elements.
  • compound → 2 or more substances

AB A + B

decomposition1
Decomposition
  • There are 6 different types of decomposition

Did you know? You might also know decomposition by analysis.

electrical decomposition
Electrical Decomposition

AB → A + B

2NaCl → 2Na + Cl2

decomposition oxy acid
Decomposition: Oxy-Acid

Oxy-Acid → Water + Nonmetal Oxide

H2SO4 → H2O + SO3

Examples:

HNO3

H3PO4

HClO2

decomposition metallic hydroxide
Decomposition: Metallic Hydroxide

Metallic Hydroxide → Metal Oxide + Water

2LiOH → Li2O + H2O

Fe(OH)2 → FeO + H2O

decomposition metallic carbonate
Decomposition: Metallic Carbonate

Metallic Carbonate → Metal Oxide +Carbon Dioxide

MgCO3 → MgO + CO2

Fe2(CO3)2 → Fe2O3 + 3CO2

decomposition metallic chlorate
Decomposition: Metallic Chlorate

Metallic Chlorate → Metal Chloride + Oxygen

2LiClO2 → 2LiCl + 3O2

Ca(ClO3)2 → CaCl2 + 3O2

decomposition metallic oxide
Decomposition: Metallic Oxide

Metallic Oxide → Metal + Oxygen

2Li2O → 4Li + O2

2BaO → 2Ba + O2