2.1.2 Simple Molecular Substances

• Match the characteristic of simple molecular substances with its description:

  Molecular Structure ↔️ Composed of discrete molecules

  Bonding ↔️ Held together by intermolecular forces

  Melting/Boiling Points ↔️ Generally low

  Electrical Conductivity ↔️ Are poor conductors
• Hydrogen bonding is a stronger force between molecules containing hydrogen bonded to nitrogen, oxygen, or fluorine
• Simple molecular substances are held together by intermolecular forces, which are weaker than ionic or metallic bonds
• Simple molecular substances have low melting/boiling points, whereas ionic compounds have high melting/boiling points
• Simple molecular substances are composed of discrete molecules.


  True
• What are the three primary types of intermolecular forces in simple molecular substances?

  London Dispersion, Dipole-Dipole, Hydrogen Bonding
• Dipole-Dipole Forces occur in polar molecules due to uneven sharing of electrons.


  True
• Simple molecular substances are poor electrical conductors because they have no free electrons or ions.


  True
• What is an example of a simple molecular substance with low melting and boiling points?

  Methane (CH₄)
• Water's high polarity and high boiling point make it an excellent solvent and coolant.

  True
• What type of substances are held together by intermolecular forces rather than ionic or metallic bonds?

  Simple molecular substances
• What are the three primary types of intermolecular forces in simple molecular substances?

  London Dispersion Forces, Dipole-Dipole Forces, Hydrogen Bonding
• Which type of intermolecular force is present in all molecules due to temporary fluctuations in electron distribution?

  London Dispersion Forces
• Why do simple molecular substances have low melting and boiling points?

  Weak intermolecular forces
• Match the type of substance with an example:

  Simple Molecular ↔️ Water

  Ionic Compound ↔️ Sodium Chloride

  Metallic Solid ↔️ Copper

  Covalent Network ↔️ Diamond
• Simple molecular substances generally have low melting and boiling points
• Order the intermolecular forces from weakest to strongest.

  1️⃣ London Dispersion Forces

  2️⃣ Dipole-Dipole Forces

  3️⃣ Hydrogen Bonding
• Hydrogen Bonding is a stronger force between molecules containing hydrogen bonded to nitrogen, oxygen, or fluorine
• Simple molecular substances are soluble in non-polar solvents due to the "like dissolves like
• Carbon Dioxide is held together by weak London Dispersion Forces
• Carbon Dioxide is used as a refrigerant and fire suppressant
• Simple molecular substances are composed of discrete molecules held together by intermolecular forces. intermolecular
• London Dispersion Forces are the strongest type of intermolecular force.

  False
• Dipole-Dipole Forces occur in polar molecules due to uneven sharing of electrons.


  True
• Simple molecular substances are soluble in polar solvents due to the "like dissolves like" principle.

  False
• Simple molecular substances are composed of discrete molecules held together by intermolecular forces
• Simple molecular substances are good electrical conductors.

  False
• London Dispersion Forces exist in all molecules due to temporary fluctuations in electron distribution
• Why do simple molecular substances have low melting and boiling points?

  Weak intermolecular forces
• Match the type of substance with its bonding:

  Simple molecular substances ↔️ Intermolecular forces

  Ionic compounds ↔️ Ionic bonds

  Metallic solids ↔️ Metallic bonds

  Covalent networks ↔️ Covalent bonds
• Which intermolecular forces are present in Water (H₂O)?

  Dipole-Dipole and Hydrogen Bonding
• What property of Nitrogen makes it suitable for fertilizer production?

  Inertness at room temperature