Intermolecular Forces Flashcards
What does VSEPR stand for?
Valence Shell Electron Pair Repulsion Theory
What does the repulsion of electron pairs determine?
Determines the shape of the molecule as electron pairs will be as far from one another
What are the Intermolecular Forces?
London Dispersion, Dipole-Dipole Forces, Hydrogen Bonds
Bent
2 bonds, lone pairs
Linear
2 bonds, no lone pairs
Trigonal planar
3 bonds, no lone pairs
Trigonal pyramidal
3 bonds, lone pairs
tetrahedral
4 bonds, no lone pairs
Intermolecular Forces:
Exist between individual molecules of a compound
Holds a compound together in a liquid, solid, or gas phase relatively weak
Diople-Diople forces
Polar molecules
Attraction force between the positive dipole of one molecule and the negative dipole of another
Act in many directions between multiple polar molecules at the same time
Liquid
London Dispersion forces
Weakest, but in all compounds
The attraction between protons (in the nucleus) of one atom to elections in another
Gas
What does the state of matter depend on?
The strength of the intermolecular forces
Strong IMF = Solid
Weak IMF = Gas
Hydrogen Bonds
The strongest, type of dipole force
Occurs when molecules have a covalent bond only between H-O, H-N, H-F
The attractive force between the proton in a Hydrogen atom and a very high electronegative atom creates a strong dipole effect
Polar Molecules
Partial positive and partial negative neds, causing a dipole
The molecule is polar when the atoms in the molecule are asymmetrical and have greatly different electronegativities
Different atoms surrounding the central atom
What electronegativity are metal atoms?
low, partially positive end
