IMF Flashcards
What factors increase as you move from left to right across the periodic table?
Atomic/Proton number, Atomic mass, Electronegativity, Ionization energy.
Describe the elements on the left of the periodic table.
Because they have low ionization energies, they easily lose electrons and become cations.
Define intramolecular forces.
They hold atoms together within a molecule.
Name the types of intramolecular forces.
Ionic bonds and Covalent bonds, the latter which is sub-typed into Nonpolar, Polar, and Metallic.
Define intermolecular forces.
They are forces that exist between molecules, and are therefore much weaker than intramolecular forces.
Intermolecular forces are electrostatic in nature and include van der Waals forces and hydrogen bonds
Name the types of intermolecular forces.
Dipole-dipole interaction, which is sub-typed into Hydrogen bonding, Ion-dipole interaction, and London dispersion.
When does a dipole-dipole interaction occur?
When a partially negatively charged parts of a molecule interacts with a partially positively charged part of a neighboring molecule.
When does hydrogen bonding occur?
It occurs specifically between an H atom bonded to an O (Oxygen), N (Nitrogen), or F (Fluorine).
When does London dispersion occur?
It occurs between all kinds of molecules, however, they are stronger in molecules with more electrons. They are only temporary on induced dipoles.
Describe the relative strength of dipole-dipole interactions.
Strong.
Describe the strength of hydrogen bonds.
They are the strongest of the dipole-dipole bonds.
Describe the strength of London dispersion forces.
They are the weakest intermolecular force.
Where are ion-dipole bonds evident?
They are evident in solutions because they are the forces that allow polar solvents to dissolve ionic substances.
What is electronegativity?
Electronegativity is the tendency for an atom to attract shared electrons.
What does the octet rule state?
It states that atoms tend to form compounds in ways that give them eight valence electrons and thus the electron configuration of a noble gas.
