5.3 Flashcards
What is hydrogen bonding?
A strong dipole-dipole interactions between two molecules that each contain an O-H,N-H,F-H
Define dipole-dipole?
Attractive forces between the opposite ends of 2 polar molecules
What is london dispersion forces?
Temporary attraction between other atoms and molecules
Rank the three types of bonds from strongest to weakest
Strongest - Hydrogen bonding
Mid - Dipole-dipole
Weakest - London Dispersion Forces
How do molecules become polar?
Polar molecules must contain a polar covalent bond and asymmetrical ends.
What is delta?
The absolute value difference
What results in a larger partial charge?
A larger electronegativity
How can we determine if the molecule is polar or non-polar?
We draw the dipole movements for the molecule to see if they cancel out and then we also observe the forces.
How can we determine if a molecule will be soluble in water based on its structure?
By looking at the molecule structure and if the ends are hydrophilic or hydrophobic
What type of interactions can polar molecules have?
London Dispersion Forces, Dipole-Dipole and Hydrogen Bonds
Are polar molecule soluble in water? Why?
Yes, the uneven electron density in polar molecules allows them to form hydrogen bonds with the water molecules