VSEPR Theory and Molecular Geometry Quiz
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Questions and Answers

What are the bond angles in a trigonal bipyramidal geometry?

  • 90° and 120° (correct)
  • 120°
  • 180°
  • 109.5°
  • Which type of intermolecular force is present in all molecules?

  • Hydrogen Bonding
  • London Dispersion (correct)
  • Dipole-Dipole
  • Ionic Bonding
  • What is the primary factor determining the polarity of a molecule?

  • Symmetry of the molecule
  • Electronegativity differences between atoms (correct)
  • Presence of lone pairs on the central atom
  • Molecular mass of the compound
  • Which of the following statements about electrolytes is correct?

    <p>Weak electrolytes partially dissociate in solution.</p> Signup and view all the answers

    Which equation correctly represents the relationship for dilution?

    <p>$M_1 V_1 = M_2 V_2$</p> Signup and view all the answers

    What does the term 'like dissolves like' refer to?

    <p>Polar substances dissolve in polar substances.</p> Signup and view all the answers

    How does adding solvent affect the concentration of a solution?

    <p>It decreases the concentration.</p> Signup and view all the answers

    What is the role of water as a solvent for ionic compounds?

    <p>It helps to separate the ions due to its polar nature.</p> Signup and view all the answers

    What determines the molecular shape of a compound?

    <p>The number of bonds and lone pairs</p> Signup and view all the answers

    How does polarity in molecules typically arise?

    <p>From uneven distribution of dipoles</p> Signup and view all the answers

    What are intramolecular forces primarily responsible for?

    <p>Holding atoms together within a molecule</p> Signup and view all the answers

    Which of the following is a method to prepare a concentrated solution?

    <p>Evaporating the solvent from the solution</p> Signup and view all the answers

    What is the formula used to calculate dilution?

    <p>$M_1 imes V_1 = M_2 imes V_2$</p> Signup and view all the answers

    What is the role of Avogadro's number in solution calculations?

    <p>It converts between moles and particles</p> Signup and view all the answers

    Which intermolecular force is particularly strong in water?

    <p>Hydrogen bonding</p> Signup and view all the answers

    What does molarity measure in a solution?

    <p>The number of moles of solute per liter of solution</p> Signup and view all the answers

    Study Notes

    VSEPR Theory and Molecular Geometry

    • VSEPR theory predicts molecular geometry based on electron repulsion.
    • Common geometries include linear (180°), trigonal planar (120°), tetrahedral (109.5°), trigonal bipyramidal (90°/120°), and octahedral (90°).
    • Use Lewis structures to count bonding and lone pairs around the central atom to determine shape.
    • Examples: Water (bent, 104.5°) and methane (tetrahedral, 109.5°).

    Intermolecular Forces (IMFs) vs. Intramolecular Forces

    • IMFs are forces between molecules (weaker).
    • Types of IMFs: London Dispersion (all molecules), Dipole-Dipole (polar molecules), Hydrogen Bonding (H with N, O, F).
    • Intramolecular forces are bonds within molecules (stronger), such as covalent, ionic, or metallic bonds.

    Polarity of Molecules

    • Polar molecules have asymmetrical electron distribution (asymmetrical dipoles).
    • Nonpolar molecules have symmetrical electron distribution.
    • Dipoles point towards the more electronegative atom.
    • Partial charges are assigned: δ- (partial negative) to the more electronegative atom and δ+ (partial positive) to the less electronegative one.

    Conversions Between Units

    • Use molar mass to convert between grams and moles.
    • Use Avogadro's number (6.022 × 10²³) to convert between moles and particles.

    Formation of a Solution

    • Solvent molecules surround solute particles.
    • For ionic compounds, water (a polar solvent) separates ions.
    • Water's partial negative (O) attracts cations, and partial positive (H) attracts anions.

    Electrolytes and Non-Electrolytes

    • Dilute solutions have low solute concentration; concentrated solutions have high solute concentration.
    • Electrolytes conduct electricity.
      • Strong electrolytes fully dissociate (e.g., NaCl).
      • Weak electrolytes partially dissociate (e.g., CH₃COOH).
    • Non-electrolytes do not dissociate (e.g., sugar).

    Dilution and Concentration Changes

    • Dilution decreases concentration by adding solvent.
    • Concentration increases by removing solvent (e.g., through evaporation).

    Particle Diagrams for Solutions

    • Depict solute (dots/ions) and solvent (molecules).
    • Vary density to represent concentration.
    • Include dissociated ions for electrolytes.

    Dissolution of Solutes

    • "Like dissolves like": Polar solvents dissolve polar solutes; nonpolar solvents dissolve nonpolar solutes.
    • Dissolution depends on particle interactions (e.g., ion-dipole forces in saltwater).

    Additive Volumes

    • Solute and solvent volumes are additive.

    Molarity and Dilution

    • Molarity (M): moles of solute / liters of solution
    • Dilution equation: M₁V₁ = M₂V₂

    Molar Mass

    • The sum of the atomic masses (from the periodic table) of all atoms in a compound.

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    Description

    Test your understanding of VSEPR theory and molecular geometry with this quiz. Explore the shapes of molecules based on electron repulsion, as well as the differences between intermolecular and intramolecular forces. Review examples and key concepts related to molecular polarity.

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