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principles of chemistry 1, final exam study guide all summarized

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Course
Principles of chemistry 1 (1211)

Institution
Abraham Baldwin Agricultural College

principles of chemistry 1, summarized document for the final exam, be aware this is notes all put together more simply.

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Final exam study guide
Chapter 4: chemical reactions, stoichiometry

Types of Chemical Reactions

Reaction type description
Combination Two or more reactants combine to form one product. A
reaction + B → AB.
Decomposition One reactant breaks down into two or more products.
reaction AB → A + B
Single One element replaces another in a compound.
displacement Example: AB + X → XB + A.
Double Two compounds exchange ions. Example: AB + XY →
displacement AY + XB.
Acid-base A reaction between an acid and a base to produce salt
and water. Example: HCl + NaOH → NaCl + H₂O.

Key Compounds
 Acids: Compounds that produce H⁺ ions in water. Examples: HCl, H₂SO₄.
 Bases: Compounds that produce OH⁻ ions in water. Examples: NaOH, Ba (OH)₂.
 Salts: Compounds formed from the neutralization reaction of an acid and a
base. Examples: NaCl, K₂SO₄.
 Molecular Compounds: Compounds formed by covalent bonds between
nonmetals. Examples: CH₄ (methane), C₂H₅OH (ethanol).

Key Concepts in Solutions
 Solvent: The substance in which a solute is dissolved, typically water in
aqueous solutions.
 Solute: The substance that is dissolved in a solvent. Examples: salts, sugars.
 Solution: A homogeneous mixture of solute and solvent.

,  Strong Electrolytes: Compounds that dissociate completely in water, such as
strong acids and bases.
 Weak Electrolytes: Compounds that partially dissociate in water, such as weak
acids and bases.
Equation type description
Complete A balanced chemical equation showing all reactants and
reaction products.
ionic A representation of a chemical reaction showing the
ions involved.
Net ionic An equation that shows only the ions that participate in
the reaction, omitting spectator ions.
Facts to Memorize
 Strong acids: HCl, HNO3, H2SO4, HI, HClO4
 Strong bases: NaOH, KOH, Ba (OH)2, Ca (OH)2
 Oxidation number of elements in their elemental state is 0.
 Common strong electrolytes: NaCl, K2SO4, Mg (NO3)2
 Common weak electrolytes: HF, H2CO3, NH3
 Solubility rules for ionic compounds in water.

Cause Effect
Combination of H₂ and Formation of water (H₂O)
O₂
Decomposition of H₂O Production of H₂ and O₂ gases
Acid reacts with base Formation of salt and water (neutralization)
Oxidation of Zn by Zn is oxidized and Cu²+ is reduced,
Cu²+ demonstrating electron transfer.

Calculation type description

molarity To find molarity, convert grams of solute to moles
using molar mass, then divide by the volume of
solution in liters.
dilution Use the formula M₁V₁ = M₂V₂ to find the
concentration after dilution.
Stoichiometry in Use balanced chemical equations to determine
reactions the molar relationships between reactants and
products for calculations involving mass and
volume.
Key Practice Problems

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