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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) |
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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 |
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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 |
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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 |
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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 |
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Electrolytes |
Strong Electrolyte 100% dissolves ions Weak Electrolyte partially dissolved |
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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 |
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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 |
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Acid Base reactions |
Identify acid and bases memorize strong acids and bases |
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Gas forming reactions |
Learn to recognize this type of reaction, memorize table |
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Oxidation reduction reactions |
Identify these reactions |
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Chemical reactions in water |
Exchange (metathesis) reactions The anions exchange places between cations A precipitate forms if one of the products in insoluble |
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Writing Equations |
Complete Ionic Equation: Soluble species as ions Net Equations: Molecular equations Total Ionic Equation |
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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 |
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Reactions of Acid and base |
Products: a salt and water HCl (aq) + NaOH (aq) Be able to recognize acid, base reactions |
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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 |
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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 |
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Weak Acids |
Very Important Since Weak acids ionize to such a small extent the molecular species predominates |
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Monoprotic and Polyprotic Acids |
Monoprotic (1 acidic H) HCl, HNO3 Diprotic (2 acidic H's) H2SO4 H2CO3 Triprotic (3 acidic H's) H3PO4 H3C6H5O7 |
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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 |