1 / 15

Lecture 4.1 – Intermolecular Forces and the Dissolving Process

Lecture 4.1 – Intermolecular Forces and the Dissolving Process. Today ’ s Learning Targets. LT 4.1 – I can discuss how ionic solids dissolve due to the random molecular motion of the water molecules.

asha
Download Presentation

Lecture 4.1 – Intermolecular Forces and the Dissolving Process

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Lecture 4.1 – Intermolecular Forces and the Dissolving Process

  2. Today’s Learning Targets • LT 4.1 – I can discuss how ionic solids dissolve due to the random molecular motion of the water molecules. • LT 4.2 – I can identify a compound as containing hydrogen bonding, dipole – dipole forces, and Van der Waals forces. • LT 4.3 – I can compare and contrast various intermolecular forces and relate them to the dissolving process of a solid.

  3. What are intermolecular forces?

  4. I. Intermolecular Forces • Intermolecular forces are forces that attract molecules to one another. • The three main types of intermolecular forces are: (1) Hydrogen Bonding (2) Dipole-Dipole Forces (3) Dispersion Force (also known as Van der Waals Forces)

  5. Pulls electrons towards itself because it has a higher electronegativity H F δ- δ+ Partial negative charge H F This is what a dipole looks like

  6. III. Dipole-Dipole Forces • Dipole-dipole forcesrefer to the attraction between molecules that have a permanent dipole.

  7. What Dipole-Dipoles Look Like Partial negative attracted to the partial positive

  8. III. Dispersion Forces • Some molecules have an induced dipole. • Dispersion forcesare the intermolecular forces resulting from the uneven distribution of electrons and the creation of temporary dipoles. • Weakest intermolecular force

  9. But, when two H2 molecules are put next to one another, a dipole is induced because electrons rearrange themselves There is no electronegativity difference between two hydrogens, so they are non-polar and do not have a dipole

  10. What the Heck?

  11. IV. Hydrogen Bonding • Hydrogen bondingis the attraction of one molecule that contains hydrogen to another molecule. • When hydrogen is bound to N, O, or F, there is a large difference in electronegativity • Creates a partial positive and negative charge • The partial positive charge on hydrogen is attracted to N, O, or F of another molecule.

  12. Hydrogen bond between H and O

  13. V. Intermolecular Forces and Phase of Substance • The degree of intermolecular forces determines the phase of a substance. Least intermolecular forces Most intermolecular forces

  14. Summarize

More Related