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Understanding Molecular Compounds: Naming, Percent Composition, Empirical Formulas, and Reactions

This guide explores the fundamentals of molecular compounds, including naming conventions with prefixes, calculations for percent composition, and determination of empirical formulas. Learn how to calculate the molecular formula from empirical data, balance equations, and identify various types of chemical reactions, such as synthesis, decomposition, and combustion. The document elucidates core concepts like covalent bonds and diatomic molecules, providing a comprehensive overview for students in chemistry. Essential for mastering the basics in molecular chemistry.

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Understanding Molecular Compounds: Naming, Percent Composition, Empirical Formulas, and Reactions

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  1. Test 4 Review • Naming Formulas • Percent composition • Empirical formulas • Balancing Equations • Types of Reactions • Activity Series

  2. Molecular Compounds • A molecule is held together by covalent bonds. • Valence electrons are shared. • Between non-metals i.e. H2O, CO2, O2, NO

  3. Naming molecular compounds • Use prefixes 1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca-

  4. Naming molecular compounds • Use prefixes 1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca-

  5. Percent Composition • Determine the mass percentage of each element in the compound. Mass of elementx 100% mass of compound What is the percent composition of Fe2O3? 2 Fe 2 x 55.8 = 111.6 3 O 3 x 16.0 = 48.0 Formula mass 159.6 %Fe = 111.6/159.6 = 70.0% % O = 48.0/159.6 = 30.0%

  6. Calculating Molecular Formula X (empirical formula) = molecular formula so x = molecular formula mass empirical formula mass

  7. What is the molecular formula of the molecule that has an empirical formula of CH2O and a molar mass of 120.12 g/mol? Empirical formula mass: 12.0 + 2.0 + 16.0 = 30.0 amu X = 120.12 amu = 4 30.0 amu So C4H8O4 is the molecular formula.

  8. Determining empirical formula • Find the empirical formula of a compound that contains 53.7% iron and 46.3% sulfur. • % composition g mass of 100 g sample g moles g mole ratio • 53.7g x 1 mol/55.8g = .962 mol Fe 46.3g x 1 mol/32.1g = 1.44 mol S .962/.962 = 1, 1.44/.962 = 1.5 1:1.5 ratio x 2 = 2:3 ratio Fe2S3

  9. Diatomic Molecules • “Honkle Brif” • H2 • O2 • N2 • Cl2 • Br2 • I2 • F2

  10. Symbols • Yields • Gas (g) • Precipitate • Solid (s) or down arrow • Liquid (l) • Aqueous (aq)

  11. Types of Reactions • Balancing Equations • Synthesis (Combination) • Decomposition • Single Displacement (Replacement) • Double Displacement (Replacement) • Neutralization • Combustion

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