1 / 8

Metallic Bonds and Properties

Metallic Bonds and Properties. Metallic Bonds. is a chemical bond resulting from the attraction between positive ions and surrounding mobile e-. Metallic bonds- electrons are free to move throughout the material. Metals. Hybridization -The Blending of Orbitals.

grayjennifer
Télécharger la présentation

Metallic Bonds and Properties

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. Metallic Bonds and Properties

  2. Metallic Bonds • is a chemical bond resulting from the attraction between positive ions and surrounding mobile e-.

  3. Metallic bonds- electrons are free to move throughout the material. Metals

  4. Hybridization-The Blending of Orbitals. • Dipole- is created by equal but opposite charges that are separated by a short distance. • Dipole-DipoleAttractions-Attraction between oppositely charged regions of neighboring molecules. • Hydrogen Bonding- Bonding between hydrogen and more electronegative neighboring atoms such as oxygen and nitrogen. Hydrogen bonding in Kevlar, a strong polymer used in bullet-proof vests. • London DispersionForces-The temporary separations of charge that lead to the London force attractions are what attract one nonpolar molecule to its neighbors. London forces increase with the size of the molecules.

  5. Molecular StructuresandVSEPR theory

  6. VSEPR Theory- “Valence- shell, electron-pair repulsion” • states that repulsion between the sets of valence-level electrons surrounding an atom cause these sets to be oriented as far apart as possible.

  7. Determining VSEPR • Determine the VSEPR for H2O • Draw the Lewis Dot • Draw the Structural Formula • Label the central atom as A • Label any atoms attached to the center atom as B • Label any paired electrons on the central atom that are not used in the bond as E H-O-H E2 B B A VSEPR AB2E2 Shape Bent (look on chart)

  8. VSEPR Chart

More Related