All the reactions are assumed to take place in water unless otherwise stated, so things that completely disassociate in water should be written as ions.

• A pure metal or a metal hydride in water will produce a base and hydrogen gas.
• A metal oxide in water will produce a base.
• A nonmetal oxide in water will produce an acid.

Electrolytes: a salt that conducts electricity once it is in solution--according to Arthur.

• any ionic solid that dissolves in solution because it dissociates into its ions
  • the free ions allow conductivity in the solution
    
• any insoluble ionic solid = nonelectrolyte

concentrated/dilute: describe molarity
strong/ weak: describe intermolecular strength (fully disassociates/ does not)

Strong acids and bases fully dissociate into their ions--strong electrolytes
Weak acids and bases do not fully dissociate -- weak electrolytes

salt- description for any ionic compound whose cation comes from a base and whose anion comes from an acid.

Reaction Types
Precipitation- formation of insoluble compound
acid- base; neutralization- formation of a salt and water; proton transfer
gas- forming- evolution of a water- insoluble gas (CO2)
Oxidation- reduction- electron tranfer
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Titrations

• Titration = use of an acid or base of known concentration to determine the concentration of the unknown solution
• Standard solution = a solution of which an exact concentration is known
• Equivalence point--when moles of acid is equal to moles of base. At the equivalence point, the pH is dependent on whether you use strong or weak acids and bases. [ H+ ] = [ OH- ]
• Endpoint--The point at which you end the titration. Usually it is when the indicator changes colors. Ideally, that is as close to the equivalence point as possible.

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Oxidation-Reduction Reactions

• When a substance accepts electrons, it is said to be reduced beceause there is a reduction in the positive charge on an atom of the substance. (This substance is the oxidizing agent)
• When a substance loses electrons, it is said to be oxidized because the positive charge on an atom of the substance increases. (This substance is the reducing agent)

Cheesy Ways to Remember:

• OIL RIG (oxidation is loss, reduction is gain)
• LEO the lion goes GER (losing electrons oxidation, gaining electrons reduction)
• OLÉ (oxidation losing electrons)

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Oxidation Numbers RULES

1. Each atom in a pure element has an oxidation number of zero.
2. For monatomic ions, the oxidation number is equal to the charge on the ion.
3. Fluorine always has an oxidation number of -1 in compounds with all other elements.
4. Cl, Br, and I always have oxidation numbers of -1 in compounds with all other elements.
5. The oxidation number of H is +1 and of O is -2 in most compounds.
6. The algebraic sum of the oxidation numbers for the atoms in an neutral compounds must be zero; in a polyatomic ion, the sum must be equal to the ion charge.

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Net Ionic Equations:

• Substances that dissociate extensively should be written as ions
• Leave out spectator ions ( any molecules that are not changed in the reaction)
• Make sure the net ionic equation has the same charge and same mass on each side, if they don't then balance.

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Standardization- using a known concentration of a substance to calculate an unknown concentration
Primary standard- typically a solid acid that does not react with the environment therefore, its concentration
does not chance. It is used to determine an unknown concentration and to then standardize the unknown solution
Secondary standard- standard that is found by a primary standard, once standardized it can be used to calculate
the concentration of a new unknown.



M or Molarity (Concentration) = amount of solute (mol)/ volume of solution (L)