2.5/2.6 Key Words Flashcards
Electron configuration
Arrangement of electrons in shells, sub-shells and orbitals
Electronic energy level
Energy of electrons in a specific electron shell and sub-shell
Principle quantum number
Overall energy of orbital, increasing with distance from nucleus
Sub-shell
Collection of atomic orbitals in a main electron shell
Atomic orbital
Region of electron density with different shapes, contain 2 electrons w/ opposite spin
s-orbital
Spherical shaped atomic orbital with lowest energy of all orbitals (in a main energy level)
p-orbital
Dumbbell-shaped atomic orbital with second lowest energy of all orbitals (in a main energy level) 3 p-orbitals on x,y and z planes in space - 6 electrons
d-orbital
5 variations holding 10 electrons
f-orbital
7 variations holding 14 electrons
Ionic bonding
Strong electrostatic attraction between oppositely charged ions
Covalent bonding
Strong electrostatic attraction between shared pairs of electrons and the positive nuclei of the bonded atoms
Dot and cross diagrams
Diagrams to show electron transfer or sharing in bonding
Dative/coordinate covalent bonding
Covalent bond where both of the shared pair of electrons are donated to by one of the bonding atoms (NH4)
Electron-pair repulsion theory
Electron pairs repel as far apart as possible
bonded-pair/bonded-pair < lone-pair/bonded-pair < lone-pair/lone-pair - strength of repulsion (lone pairs closer to nucleus than bonded pairs
Bond angle tetrahedral
109.5 degrees
Bond angle trigonal planar
120 degrees
Bond angle pyramidal
107 degrees
Bond angle linear
180 degrees
Bond angle non-linear/bent
104.5 degrees
Bond angle octahedral
90 degrees
Bond angle trigonal bipyramidal
90 degrees from vertical and 120 degrees around
Permanent dipole - Permanent dipole
Attraction between two molecules where atoms have high electronegativity difference, opposite delta-charges attract. 2 polar molecules
Permanent dipole - Induced dipole
Attraction of shared pair(s) of electrons in a non-polar molecule by a polar molecule due to delta-charges repelling the shared pair of electrons. Polar and non-polar molecule.
Instantaneous dipole - Induced dipole (London forces)
Movement of electrons in orbitals, potential for high concentration on one side of molecule, creates instantaneous dipole, induces dipole in nearby molecule due to delta-charges. All molecules. Weakest intermolecular force
Hydrogen bond
Molecules where N, O & F bond with hydrogen, many lone pairs of electrons, area of high electron density creates a delta charge which can attract other permanent dipoles. Strongest intermolecular force
