Molecular Properties Table Quiz

Molecular Structure Table

• The table displays a list of chemical formulas with their corresponding properties:
  • Number of Valence Electrons
  • Lewis Dot Structure
  • Molecular Geometry
  • Molecular Polarity
  • Intermolecular Forces (IMF's)
• The table includes polyatomic ions with charge (e.g., NO₂⁻)
• The Lewis Dot Structures and Molecular Geometries are handwritten, ensuring accuracy by referring to other sources

Additional Notes

• The total number of valence electrons is calculated by summing the valence electrons of each atom in the molecule.
• Common molecular geometries include bent, linear, trigonal planar, and tetrahedral.
• Molecular polarity is determined by the distribution of electron density within the molecule.
• Intermolecular forces are attractive forces between molecules.
• The table lists common IMFs:
  • Dipole-Dipole Interactions
  • London Dispersion Forces (LDF)
  • Hydrogen Bonding

Molecular Properties of Different Compounds

• The table displays a collection of molecules with their molecular properties, including:
  • Formula
  • Number of Total Valence Electrons
  • Lewis Dot Structure
  • Molecular Geometry
  • Molecular Polarity
  • Intermolecular Forces (IMF's)
• The table focuses on the types of IMF's present in each molecule.
• The Lewis dot structures and geometrical representations are hand drawn, which can be inaccurate.
• The table could be a chemistry assignment or notes on chemical bonding.

Vocabulary

• Double bond: A covalent bond formed by the sharing of two pairs of electrons between two atoms.
• Electronegativity: Measures an atom's ability to attract electrons in a covalent bond.
• Ionic bond: Results from electrostatic attraction between oppositely charged ions.
• Covalent bond: Forms when electrons are shared between two atoms.
• Triple bond: A covalent bond sharing three pairs of electrons between two atoms.
• Polar bond: Occurs when electrons are shared unevenly between two atoms.
• Metallic bond: Forms between metal atoms where electrons are free to move (sea of electrons).
• Lone pair: A pair of electrons not involved in bonding.
• Central atom: Usually carbon, it is the atom at the center of the molecule.
• Intramolecular forces: Attractive forces between atoms within a molecule.
• Intermolecular forces: Attractive forces between molecules.
• Partial charge: Represented by the Greek letter delta (δ), it indicates an uneven distribution of charge within a molecule.

IMFs: Determining IMF Type

• Question 1: F₂ has a lower boiling point than I₂ because F₂ experiences weaker London Dispersion Forces (LDFs) due to its smaller number of electrons.
• Question 2:
  • CH₃OH (methanol) would have the highest boiling point because of its ability to form hydrogen bonds due to the presence of an OH group.
  • Hydrogen bonds are the strongest type of intermolecular force, leading to higher boiling points.
  • CH₃Cl has dipole-dipole forces which are weaker than hydrogen bonds.
  • H₂O also forms hydrogen bonds, but they are less strong than those in methanol.