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4U Chemistry

Stuctures and Properties

QuestionAnswer
principal quantum number n, describes the size of the orbital (see the coefficient number in front of orbital type)
magnetic quantum number m sub l; describes magnetic orientation of a sub-orbital
orbital-shape quantum number l=0 (s orbital); 1 (p orbital); ; 2 (d orbital); ; 3 (f orbital)
spin quantum number m sub s; describes the electron spin; either +1/2 or -1/2
Hund's Rule maximum 2 electrons per orbital but these electrons must have opposite spins. Electrons fill orbitals singly before pairing up
atomic orbital region in space around a nucleus where an electron has a high probability of being found
aufbau filling order assigning electrons to orbitals, starting with the lowest energy orbitals (1s)
ionization energy energy required to remove an electron (F has highest)
electron affinity energy released when an electron is added (F has highest)
metallic bonding metal cations held together by attraction to delocalized electrons
network covalent bonding covalent network solid is a continuous network of covalently bonded atoms that spans the entirety of the material; very strong bond
ionic bonding attraction between fully charged ions of opposite charge (metal + nonmetal ions); strong bond
ion-dipole force intermolecular attraction between a fully charged ion and a dipole with an opposite partial charge; strongest IMF
London dispersion forces as electrons disperse in an atom or compound, there may be a momentary uneven distribution of electrons. This creates a momentary dipole that has weak attractive forces.
intermolecular force force of attraction BETWEEN separate atoms or molecules; has great influence on the physical properties of that substance.
intramolecular force force of attraction WITHIN an atom or compound (eg. metallic, ionic, covalent or network force)
Pauli exclusion principle no two electrons in the same atom can have identical values for all four of their quantum numbers.
hybridization blending of orbital energies so that sigma bonds can form. This creates half-filled orbitals which will overlap the orbital of the next atom
sp hybridization occurs in molecules with two regions of electron density
sp2 hybridization occurs in molecules with 3 regions of electron density
sp3 hybridization occurs in molecules with 4 regions of electron density
sp3d hybridization occurs in molecules with 5 regions of electron density
sp3d2 hybridization occurs in molecules with 6 regions of electron density
Isomers Molecules that have the same molecular formula but different structure (shape).
Created by: jcepella
 



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