1 / 17

Understanding Bond Types and Intermolecular Forces: A Comprehensive Guide

This resource aims to help students predict bond types—polar, nonpolar, and ionic—using electronegativity and periodic table placement. It will explore dispersion forces, dipole-dipole interactions, and hydrogen bonding, along with hands-on exercises. The drill focuses on identifying combinations of bonded and nonbonded electron pairs in bent structures. Key concepts include distinctions among ionic, nonpolar covalent, and polar covalent bonds, as well as various intermolecular forces. This comprehensive overview will enhance comprehension of molecular interactions and polarity.

selah
Télécharger la présentation

Understanding Bond Types and Intermolecular Forces: A Comprehensive Guide

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. Objectives: • To use electronegativity and the location of elements on the periodic table to predict the type of bond (polar, nonpolar, ionic) • To describe dispersion forces, dipole-dipole interaction, and hydrogen bonding

  2. Drill: • Give all the combinations of the number of bonded pairs and nonbonded pairs of electrons for a bent structure.

  3. Homework • Complete Worksheet • Read lab and complete pre-lab questions

  4. Intramolecular Forces The forces of attraction that exist between bonds within a molecule.

  5. Dipole • Charged ends of a molecule • Represented by δ+ or δ- • Slightly positive - δ+ • Slightly negative - δ-

  6. Nonpolar Bond • When two atoms have the same electronegativity. • No dipole is formed

  7. Polar Bond • When the electronegativities of the atoms differ. • The greater the difference the more polar the bond • A dipole may form

  8. Ionic Bonds • Atoms on opposite sides of the table have large differences in electronegativity. • Bonds are highly polar • ΔEN > 1.8

  9. Nonpolar Covalent Bonds • Nonmetallic atoms of the same type have the same electronegativity • Bonds are nonpolar • ΔEN < 0.4

  10. Polar Covalent Bonds • Atoms in between these two extremes have an uneven sharing of electrons • Slightly charged atoms • 1.8 ≥ ΔEN ≥ 0.4

  11. Intermolecular Forces • The attraction between molecules • The stronger the intermolecular forces the more energy it takes to change phases

  12. Types of Intermolecular Forces • Ion • Charged particle • Dipole • Polar molecule • Induced dipole • Non-polar molecule induced into having a temporary dipole

  13. Types of Intermolecular Forces • Strengths of intermolecular forces • Ion – ion (strongest) • Ion – dipole • Dipole - dipole • Dipole – induced dipole • Induced dipole – induced dipole (weakest)

  14. Very special intermolecular force • Hydrogen bonding • An unusually strong dipole-dipole attraction • Between molecules with a hydrogen atom attached to a very electronegative atom • (F or O or N or . . .)

  15. Summary of Types of Intermolecular Forces

  16. Molecular Polarity • Non Polar Molecule • All bonds in the molecule are nonpolar • Dipoles of equal strength but pull in opposite directions, cancel each other out. The net result is an even distribution of bonding electrons around the whole molecules • Often symmetrical in shape

  17. Molecular Polarity • Polar Molecule • There is an uneven distribution of bonding electrons. • Often asymmetrical in shape

More Related