2.4 Study Guide Flashcards
What are the intermolecular interactions?
London Dispersion, Dipole-Dipole, Hydrogen, Ionic, and Covalent.
Please rank the intermolecular interactions from weakest (1) to strongest (5).
London Dispersion = 1.
Dipole-Dipole = 2.
Hydrogen = 3.
Ionic = 4.
Covalent = 5.
Please describe how a molecule is polar based on its structure.
Electron density is unevenly distributed throughout the molecule, resulting in regions of partial negative charge and regions of partial positive charge.
Please describe how a molecule is nonpolar based on its structure.
There are no positive or negative poles formed in the molecule. They’re all distributed evenly across the molecule. They are generally symmetrical.
Please determine what type of intermolecular attractions a hydrogen molecule will be able to form based on its structure.
Dipole-dipole because of the attractive force between a hydrogen atom covalently bonded to a very electronegative atom such as N, O, or F and another very electronegative atom.
Please state which molecules are soluble in water based on their structure.
Polar molecules. They have dipoles and partial charges. They also usually dissolve in water easily.
What is hydrogen bonding?
Strong dipole-dipol interactions between 2 molecules that each contain an O-H, N-H. F-H bond.
What is london dispersion?
Temporary dipoles. Symmetrical vs. unsymmetrical. Caused by the movement of electrons in a molecule.
What is the dipole-dipole interaction?
2 polar molecules attract to each other by opposite charges. The - end of a molecule will attract the + end of another molecule.
What is considered a special case?
Hydrogen bonding.
Please list the 3 intermolecular bonds/interactions.
London, dipole, and hydrogen.
Please list the 2 intramolecular bonds/interactions.
Ionic and covalent.
