Organic Chem Unit 1 (VOCABULARY) Flashcards
Orbital
mathematical descriptions that chemists use to explain and predict the properties of atoms and molecules
Heisenberg Uncertainty Principals
never define exactly where the electron is; nevertheless, we can find the electron densities-the probability of finding the electron in a particular part of the orbital
Pauli Exclusion Principle
each orbital can hold a max of 2 electrons, provided the spins are paired
Aufbau Principle
how to build up the electron configuration of an atom’s ground state
Hund’s Rule
2 or more orbitals of the same energy, electrons go into different orbitals rather than pair up in the same orbital
Octet Rule
atoms transfer or share electrons in such a way as to attain a filled shell of electron
Ionic bond
transfer of 1 electron gives each atom 2 electrons
Covalent Bond
electrons are shared
Lewis Structure
visualize bonding in covalent molecules
Non-bonding electrons
valence electrons that are not shared between 2 atoms = lone pairs
Formal Charge
number of valence electrons - number of non-bonding - 1/2 total number of electrons shared in bonds
Molecular Dipole Moment
dipole moment of the molecule taken as a whole
Intermolecular Forces
the force that mediates interaction between molecules, including the electromagnetic forces of attraction between atoms and other types of neighboring particles.
Dipole - Dipole
2 negative ends or positive ends approach each other, they repel, but may turn themselves in a more stable positive negative orientation
London Dispersion
arise from temporary dipole moments
