imf_chart1

imf_chart1 - nonpolar molecules Polar Molecules Molecules...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Weakest ------------------------------------------------------------------------------------------------------------------------- Strongest London Disperson Forces Dipole-Dipole Interactions Hydrogen Bonding Metallic Bonding Ionic Bonding Covalent Bonding (as Intermolecular Force!) Definition Attraction b/w temporary dipoles due to random e- motion Attraction b/w the permanent dipole in polar molecules Special kind of dipole-dipole interaction that involves an H attached to a very electronegative atom Metal cations held together by delocalized electron “sea” Ions held together by electrostatic attraction Atoms held together in the bulk solid by a network of covalent bonds Occurs in Everything! Especially important for
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: nonpolar molecules Polar Molecules Molecules containing X-H bond where X =O, N or F Metals Ionic compounds Covalent Network solids Examples N 2 , benzene,C 6 H 6 gasoline, C 8 H 18 Formaldehyde CH 2 O, NH 3, H 2 O HF NH 3 CH 3 OH R-COOH Na, Cu, Fe, Mn NaCl, MgCl 2 Silicates: (glass, quartz, ceramics) Carbon: diamond, graphite Increases with Molar mass; surface area of molecule; polarizability (number of electrons) Dipole moment (Dependent on difference in electronegativity) # of X-H bonds; electronegativity of X Smaller atomic size means greater strength. (Coulombs Law) Charge of ions; small ion size (Coulombs Law) Greater hybridization= greater strength. Graphite sp 2 Compared to diamond sp 3...
View Full Document

{[ snackBarMessage ]}

Ask a homework question - tutors are online