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20 Cards in this Set

  • Front
  • Back

Lavoisier

Law of conservation of matter


Matter can not be created nor destroyed in a reaction


Matter cannot be created nor destroyed in a reaction


P4 (s) + Cl2 (g)--> PCl3 (l)


P4 (s) + (6) Cl2 (g)--> (4) PCl3 (l)

Chemical Equations

The reactants and products in a reaction


The the numbers in the front are called


stoichiometric coefficients


Stoichiometry: Relationship between amounts of reactant and products

Balancing Equations

Write unbalanced equation with correct formulas


Pentane burns in presence of oxygen to produce gaseous carbon dioxide and water


Adjust coefficients to get equal number of each atom


-Begins with most complex substances


Balance elements that appear only once


on each side first


Balance polyatomic ions as a group


Balance free elements last


Reduce coefficients to smallest whole numbers

Notes on balancing equations

Formulas must be right or equation is meaningless


Subscripts cannot be changed


Treat polyatomic ions as units


Some reactions are reversible


Some reactions form a lot of product or a little bit of product

Reactions in Aqueous Solution

Solvent: aqueous --->water


Ionic compounds dissolve in water to produce ions!


Solutions with ions called electrolytes


Strong electrolytes -solute 100% dissociates into ions


Weak electrolytes - more molecules than ions

Electrolytes



Strong Electrolyte 100% dissolves ions


Weak Electrolyte partially dissolved

Conductivity

No ions:


Nonelectrolyte


Dissolves in water, but no ions to conduct electricity




Few ions and Lots of Ions:


Based on how many ions are produced in the solution

Precipitate Reactions

A table know how to use it


A "driving force" is the formation of an insoluble solid called a precipitate


Precipitates are determined from the solubility rules


A reaction where an insoluble solid (precipitate) forms and falls out of a solution



Acid Base reactions

Identify acid and bases


memorize strong acids and bases

Gas forming reactions

Learn to recognize this type of reaction, memorize table

Oxidation reduction reactions

Identify these reactions

Chemical reactions in water

Exchange (metathesis) reactions


The anions exchange places between cations


A precipitate forms if one of the products in insoluble

Writing Equations

Complete Ionic Equation:


Soluble species as ions




Net Equations:


Molecular equations


Total Ionic Equation

Acids and bases

Arrhenius Definition:


An acid is any substance that increases the H+ (aq) concentration when dissolved in water




A base is any substance that increase the OH- (aq) concentration in an aqueous solution

Reactions of Acid and base

Products: a salt and water


HCl (aq) + NaOH (aq)


Be able to recognize acid, base reactions



What is the definition of a strong acid

A strong acid completely dissociates into its ions


A weak acid does not completely ionize in solution

Acid Base and Strength

Strong Acids: Dissociate completely in water




HCl, HBr, HI, HNO3, HClO4, H2SO4




Weak acids: partially dissociate in water


Most Acids are weak. All other soluble acids HF, acetic acid (CH3COOH) HNO2.




Strong Bases: Dissociate completely in water


NaOH, KOH, Ba(OH)2




Weak bases: partially dissociate in water


NH3, many others

Weak Acids

Very Important


Since Weak acids ionize to such a small extent the molecular species predominates

Monoprotic and Polyprotic Acids

Monoprotic (1 acidic H)


HCl, HNO3




Diprotic (2 acidic H's)


H2SO4


H2CO3




Triprotic (3 acidic H's)


H3PO4


H3C6H5O7



Acids and Bases

Bronsted-Lowery definitions:


An acid is any substance that donates H+ (aq)


[A proton] to another species in an aqueous solution.




A base is any substances that accepts an H+ (aq)


[a proton] in an aqueous solution.




All strong acids completely transfer H+ at equilibria


A weak acid does not completely transfer protons (H+)


A weak base does not completely accept protons