Differences
This shows you the differences between two versions of the page.
| Both sides previous revisionPrevious revisionNext revision | Previous revision | ||
| ap_chem:intermolecular_forces [2020/10/13 02:07] – epix | ap_chem:intermolecular_forces [2020/11/16 05:37] (current) – add s to shorthand epix | ||
|---|---|---|---|
| Line 1: | Line 1: | ||
| - | ====== Intermolecular Forces (IMF) ====== | + | ====== Intermolecular Forces (IMFs) ====== |
| Forces of attraction between molecules. Sometimes called an interparticle force. They are caused by attractions from opposing charges in a molecule. | Forces of attraction between molecules. Sometimes called an interparticle force. They are caused by attractions from opposing charges in a molecule. | ||
| ===== Main Types ===== | ===== Main Types ===== | ||
| Line 7: | Line 7: | ||
| Polarizability is used to determine the strength of LDFs for any given covalently bonded molecule. As the likelihood of dipole formation increases with the amount of electrons, the general trend of polarizability follows the size (and thus amount of electrons) of any given atom. A general rule of thumb would be the atom with the larger atomic number will have the higher polarizability and thus stronger LDFs. | Polarizability is used to determine the strength of LDFs for any given covalently bonded molecule. As the likelihood of dipole formation increases with the amount of electrons, the general trend of polarizability follows the size (and thus amount of electrons) of any given atom. A general rule of thumb would be the atom with the larger atomic number will have the higher polarizability and thus stronger LDFs. | ||
| ==== Dipole-Dipole Attractions ==== | ==== Dipole-Dipole Attractions ==== | ||
| - | Dipole-Dipole attractions are what allow polar molecules to attract one another. As the partial charges of polar molecules are relatively consistent, they are stronger than LDFs which rely on temporary dipoles. Also, this means that orientation matters for Dipole-Dipole Attractions. The difference of electronegativity determines the strength of the attractions (higher is better.) | + | Dipole-Dipole attractions are what allow polar molecules to attract one another. As the partial charges of polar molecules are relatively consistent, they are stronger than LDFs which rely on temporary dipoles. Also, this means that orientation matters for Dipole-Dipole Attractions. The difference of electronegativity determines |
| ==== Hydrogen Bonds ==== | ==== Hydrogen Bonds ==== | ||
| - | Hydrogen bonds are a unique type of Dipole-Dipole Attraction that is categorized by two molecules with a Hydrogen bonded to either a Florine, Oxygen, or Nitrogen atom that is also unpaired. Hydrogen bonds are not Hydrogen atoms covalently bonded with another atom, it is an IMF. They are extremely strong | + | Hydrogen bonds are a unique type of Dipole-Dipole Attraction that is categorized by two molecules with a Hydrogen bonded to either a Florine, Oxygen, or Nitrogen atom with one being unpaired. Hydrogen bonds are not Hydrogen atoms covalently bonded with another atom, it is an IMF. They are extremely strong |
| + | ==== Ion-Dipole Forces ==== | ||
| + | Attractions between ions and polar molecules. Strength of attraction depends on Coulomb' | ||
| + | ==== Dipole-Induced Dipole Interactions ==== | ||
| + | Attractions between a polar and nonpolar molecule. The strength increases with the dipole magnitude of the polar molecule and the polarizability of the nonpolar molecule. | ||
