Lesson 2 Flashcards
A type of chemical bond that is formed when electrons are shared equally between two atoms.
Non-polar covalent bond
A German physicist who later worked in the United States proposed that temporary fluctuations in the electron distributions within atoms and nonpolar molecules could result in the formation of short-lived instantaneous dipole moments.
Fritz London
Attraction results from temporary dipole moments induced in ordinary nonpolar molecules.
London Dispersion Forces/Van Der Waals Forces
Present between all molecules, whether they are polar or non-polar.
London Dispersion Forces/Van Der Waals Forces
Electrons are equally distributed and constantly revolve.
Neutral atom
Weak Forces, temporary intermolecular forces.
London Dispersion Forces/Van Der Waals Forces
Attractive forces between polar molecules. The partial negative side of one molecule is attracted to the partial positive side of another molecule.
Dipole-Dipole Forces
The larger the dipole moment, the stronger the attraction.
Coulomb’s Law
The electrons are unevenly distributed because some elements are more electronegative than others.
Polar molecules
It is a polarized molecule having partially positive and negative poles.
Dipole
It is not a chemical bond. It only exists in polar covalent bonds.
Dipole-Dipole Force
It is a special type of dipole-dipole interaction between the hydrogen atom in a polar bond, such as N‒H, O‒H, or F‒H, and an electronegative O, N, or F atom (F,O,N). This bond is particularly strong between water molecules.
Hydrogen Bond
It is not a chemical bond rather it is weaker than a covalent bond 20 times but stronger than a dipole-dipole force 10 times.
Hydrogen Bond
Attractive force that occurs between an ion and a polar molecule.
Ion-Dipole Force
It is an atom or group that holds an electrical charge.
Ion
