Physical science Intermolecular ForcesFor each type of intermolecular force, do the following:•Write the definition in your own words.•Draw a diagram/illustration showing how the force works. (Must be hand-drawn, not digital.)•Give at least two examples of substances or scenarios where it occurs.•Color-code your diagrams for clarity.
Answer (1)
Intermolecular Forces (IMF)1. London Dispersion Forces (LDF)Definition (in my own words):The weakest type of force. It happens when the electrons in an atom or molecule suddenly shift, creating a temporary positive and negative side. This temporary dipole makes nearby molecules shift too, so they attract for a short time.Diagram idea:Draw two neutral circles (atoms or molecules).Shade one side of each molecule slightly darker to show “temporary negative.”On the opposite side, put a “+” sign for temporary positive.Use a dotted line between them to show the weak attraction.Color-code: Use blue for negative side and red for positive side.Examples:Noble gases like Argon (Ar) and Neon (Ne).Nonpolar molecules like CH₄ (methane).2. Dipole-Dipole ForcesDefinition (in my own words):This happens when polar molecules (with permanent positive and negative ends) line up so that the positive side of one is attracted to the negative side of another. Stronger than London dispersion.Diagram idea:Draw two water molecules (H₂O) or two HCl molecules.Label δ+ on the hydrogen or H atom, δ– on the oxygen or Cl atom.Show arrows or dotted lines from δ+ of one molecule to δ– of the other.Color-code: Use blue for δ– (negative) and red for δ+ (positive).Examples:HCl (hydrogen chloride)CH₃Cl (chloromethane)3. Hydrogen BondingDefinition (in my own words):A special type of dipole-dipole force. It happens when hydrogen is bonded to a very electronegative atom (like N, O, or F). The hydrogen becomes strongly δ+, and it forms a strong attraction to another nearby electronegative atom.Diagram idea:Draw two water molecules (H₂O).Show H (δ+) from one water molecule forming a dotted bond with O (δ–) of another.Highlight the hydrogen bond with a dashed or dotted line.Color-code: Red for oxygen (δ–), blue for hydrogen (δ+), dotted green line for hydrogen bond.Examples:Water (H₂O) – gives water high boiling point.NH₃ (ammonia).4. Ion-Dipole ForcesDefinition (in my own words):This happens when an ion (charged particle) attracts the opposite end of a polar molecule. Stronger than dipole-dipole because ions have full charges.Diagram idea:Draw Na⁺ and Cl⁻ ions.Show water molecules (H₂O) surrounding them.Point the δ– oxygen toward Na⁺, and the δ+ hydrogens toward Cl⁻.Color-code: Purple for Na⁺, green for Cl⁻. Red for oxygen, blue for hydrogen.Examples:NaCl dissolving in water.KCl solution in water.✨ Tip for hand-drawing:Use circles for atoms/molecules.Always label δ+ and δ– clearly.Dotted or dashed lines = intermolecular forces.Keep colors consistent: blue (δ–), red (δ+), green (special bonds), purple/green for ions[tex].[/tex]
