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

Hybridization-The Blending of Orbitals.Hybridization-The Blending of Orbitals. Dipole- is created by equal but opposite charges that are separated by a short distance. Dipole-Dipole AttractionsDipole-Dipole Attractions-Attraction between oppositely charged regions of neighboring molecules. Hydrogen Bonding-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 Dispersion Forces- 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.London Dispersion Forces- 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.

Molecular Structures and VSEPR theory

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.

Determining VSEPR Determine the VSEPR for H 2 O 1.Draw the Lewis Dot 2.Draw the Structural Formula 3.Label the central atom as A 4.Label any atoms attached to the center atom as B 5.Label any paired electrons on the central atom that are not used in the bond as E H-O-H A BB E2E2 VSEPR AB 2 E 2 Shape Bent (look on chart)

VSEPR Chart VSEPRSHAPE AB or AB 2 Linear AB 2 EBent AB 3 Trigonal-Planar AB 4 Tetrahedral AB 3 ETrigonal-Pyramidal AB 2 E 2 Bent AB 5 Trigonal-Bipyramidal AB 6 Octahedral