Orgo Vocab 1B

krabi's version from 2015-07-16 07:13


Question Answer
Conjugate acidSpecies formed when ⇒ base accepts proton
Conjugate BaseSpecies formed when ⇒ base loses a proton
Core electronsElectrons in filled electrons
Degenerate orbitalsOrbitals have the same energy
Delocalized electronsSlutty Electrons. Electrons that do not belong to a single atom NOR they are not shared in a bond between 2 atoms
DipoleHas a +ve end and -ve END
Dipole momentA measure of the Separation of Charge in a bond/molecule
Double BondComposed of Sigma + Pi bond
Electron affinityThe energy that is given off ⇒ when an atom gets an electron
ElectronegativeDescribes how greedy an electron is and pull electrons towards itself
ElectropositiveHow easily an electron loses an electron
Equilibrium constant(PR) Ratio of ProductsReactants (at equilibrium); ratio of rate constants for forward/reverse rx
Excited State Electronic configurationThe electronic configuration that results - when electron in the ground state ⇒ moved to a higher energy orbital
Formal Charge# of valence - (½ bonding e- + LP)
Free radicalSpecies w/unpaired electron
Ground state electronic configurationDescribe which orbitals the electrons occupy when they are in lowest energy orbitals
Mass numberProtons + Neutrons in atom
NodeA region w/in orbital ⇒ there is 0 probability of finding electron
Non polar covalent bondSHARED Bond formed between 2 atoms; shared equally.
OrbitalSpace around atom that electron should be found
Orbital hybridizationblending/mixing of orbitals
Pauli Exclusion2 electrons can occupy an orbital and have opposite spin
pHlog [H+] (scale that describes acidity)
Pi Bondside to side overlap of P Orbitals.
pKapKa = -log (Ka is the Acid Disassociation constant) Tendency of a compound to lose a proton.
Polar covalent bondwhen electrons are not shared equally (in a bond between 2 atoms)
Proton transfer RxA Rx in which a proton is transferred to an acid (from base)
Free radicalA species with unpaired electron
ResonanceHaving delocalized electrons (electrons in an open relationship)
resonance contributorsStructures with localized electrons that approximate the true structure of a compound with delocalized electrons
Resonance hybridThe actual structure of a compound with delocalized electrons
Sigma BondA bond with symmetrical distribution of electrons about internuclear axis
Single bondA single pair of electrons shared between 2 atoms
Tetrahedral bond angleA 109.5 angle formed by an sp3 hybridized central atom
Tetrahedral carbonA sp3 hybridized carbon; a carbon that forms covalent bonds (using 4 sp3 hybrid orbitals)
Trigonal planar carbonsp2 hybridized carbon
Triple bondOne sigma bond + 2 Pi bonds
Wave equationAn equation that describes the behaviour of each electron
Wave functionA series of solutions of a wave equation