Notes
Slide Show
Outline
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Unit 4 – Conservation of Mass and Stoichiometry
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Ions
  • Cation:  A positive ion
  • Mg2+, NH4+
  • Anion:  A negative ion
  • Cl-, SO42-
  • Ionic Bonding:  Force of attraction between oppositely charged ions.
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Predicting Ionic Charges
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Predicting Ionic Charges
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Predicting Ionic Charges
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Predicting Ionic Charges
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Predicting Ionic Charges
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Predicting Ionic Charges
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Predicting Ionic Charges
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Predicting Ionic Charges
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Predicting Ionic Charges
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Predicting Ionic Charges
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Writing Ionic Compound Formulas
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Writing Ionic Compound Formulas
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Writing Ionic Compound Formulas
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Writing Ionic Compound Formulas
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Writing Ionic Compound Formulas
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Writing Ionic Compound Formulas
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Writing Ionic Compound Formulas
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Naming Ionic Compounds
  • 1.  Cation first, then anion
  • 2.  Monatomic cation = name of the element
  • Ca2+ = calcium ion
  • 3.  Monatomic anion   =   root  +  -ide
  • Cl-  =  chloride
  • CaCl2  =  calcium chloride
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Naming Ionic Compounds
(continued)
  • - some metal forms more than one cation
  • - use Roman numeral in name
  • PbCl2
  • Pb2+ is cation
  • PbCl2  =  lead(II) chloride
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Naming Binary Compounds
  • - Compounds between two nonmetals
  • - First element in the formula is named first.
  • - Second element is named as if it were an anion.
  • - Use prefixes
  • - Only use mono on second element -
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Calculating Formula Mass
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Calculating Percentage Composition
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Formulas
  •  molecular formula  =  (empirical formula)n [n = integer]
  •  molecular formula  =  C6H6  =  (CH)6
  •  empirical formula  =  CH
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Formulas (continued)
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Formulas (continued)
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Empirical Formula Determination
  • Base calculation on 100 grams of compound.
  • Determine moles of each element in 100 grams of compound.
  • Divide each value of moles by the smallest of the values.
  • Multiply each number by an integer to obtain all whole numbers.
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Empirical Formula Determination
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Empirical Formula Determination
(part 2)
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Empirical Formula Determination
(part 3)
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Finding the Molecular Formula
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Finding the Molecular Formula
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Finding the Molecular Formula
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Combination (Synthesis) Reactions
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Decomposition Reactions
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Single Replacement Reactions
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The Activity Series of the Metals
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The Activity Series of the Halogens
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Double Replacement Reactions
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Combustion Reactions
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Stoichiometry
  •   Stoichiometry - The study of quantities of materials consumed and produced in chemical reactions.
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Review: Atomic Masses
  • Elements occur in nature as mixtures of isotopes
  • Carbon  = 98.89% 12C
  •   1.11% 13C
  • <0.01% 14C
  • Carbon’s atomic mass = 12.01 amu
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Review: The Mole
  •  The number equal to the number of carbon atoms in exactly 12 grams of pure 12C.
  •  1 mole of anything = 6.022 ´ 1023 units of that thing
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The Mole
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Using Compound Masses
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Review: Molar Mass
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Review: Chemical Equations
  • Chemical change involves a reorganization of
  • the atoms in one or more substances.
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Mole Relations
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Calculating Masses of Reactants and Products
  • Balance the equation.
  • Convert mass to moles.
  • Set up mole ratios.
  • Use mole ratios to calculate moles of desired substituent.
  • Convert moles to grams, if necessary.
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Working a Stoichiometry Problem
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Working a Stoichiometry Problem
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Standard Molar Volume
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Gas Stoichiometry #1
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Gas Stoichiometry #2
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Gas Stoichiometry #3
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Gas Stoichiometry #4
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Limiting Reactant
  •   The limiting reactant is the reactant
  •   that is consumed first, limiting the amounts of products formed.
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Limiting Reagents - Combustion
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Solving a Stoichiometry Problem
  • Balance the equation.
  • Convert masses to moles.
  • Determine which reactant is limiting.
  • Use moles of limiting reactant and mole ratios to find moles of desired product.
  • Convert from moles to grams.