| Terms |
Definitions |
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120 and 90
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degree of trigonal bipyramidal
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as you move down a family
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the electron affinity decreases
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metallic bond differences
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alkali < transition
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bond length
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the average distance between the nuclei held together by the bond
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Azimuthal (secondary) Quantum number
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the value of l determines orbital shape. The value of n places limits on l, its max value is (n-1).
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non-polar bond
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the electron density at both ends of the bond is the same because the electrons are equally attracted to both nuclei. No lone pairs, ligands are =.
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0-0.2
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values of non-polar electronegativity
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intramolecular bonds
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forces between bonded atoms in a molecule or complex ion - Ionic bonds
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Ionic Bond
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the attraction between + and - ions in an ionic compound
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As you move across a period
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the atomic radius decreases
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Principal Quantum Number
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a positive whole # specifiying energy level of an atomic orbital and its relative size.
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Intermolecular bonds
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forces between two non-bonded atoms or molecules - hydrogen bonds, d-d bonds, VDW
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180
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degree of linear shape
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104.5
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degree of angular
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Atomic Radius
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the distance from the nucleus to the outermost energy level
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angular
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sp3 two lone pairs
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120
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degree of trigonal planar shape
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Spin Quantum Number
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only two possible values, +1/2 or -1/2.
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Magnetic Quantum number
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integer with values ranging from -l to +1.
l=0 then m= -1,0,1
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trigonal pyramidal
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sp3 one lone pair
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octahedral
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sp3d2 non-polar
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hydrogen bonds
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stronger than d-d or VDW but less than 1/10th the strength of intramolecular bonds, strongest when aligned in a straight line
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As you move down a family
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the Ionization Energy decreases
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coordinate covalent bond
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when one atom supplies both of the electrons that are shared in a covalent bond
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Lattice energy
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amount of energy required per mole to separate the ions from their lattice positions
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tetrahedral
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sp3 non-polar
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Electron Affinity
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tendency of an atom to attract an electron
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Resonance
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when the bonding in some molecules and ions cannot be adequately described by a single LEDD
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Hund's Rule
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the lowest energy state for an atom has the max # of unpaired electrons allowed by the Pauli Exclusion principle in a given energy sublevel.
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trigonal bipyramidal
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sp3d non-polar
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0.2-1.7
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values of polar electronegativity
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ionic differences
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radius -- F= Kq1q2/r2
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single/double/triple bond
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a covalent bond in which 1/2/3 pairs of electrons are shared between two atoms
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square planar
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sp3d2 two lone pairs
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trigonal planar
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sp2 3 bonding
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Ionic compounds
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form when elements with low ionization energies react with elements with high electron affinities
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Quantum mechanical model of the atom
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describes atoms as having certain allowed quantities of energy because of the wave-like properties of their electrons.
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Valence Shell Electron Pair Repulsion Theory
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VSEPR stands for...
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Ionic radius
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Distance from the center of an ion's nucleus to its outermost electron
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angular
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sp2 one lone pair
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Ionization Energy
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the amount of energy required to remove the most loosely held electron from a neutral gaseous atom
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as you move across a period
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the electron affinity increases
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Non-polar differences
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Van Der Waals
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seesaw
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sp3d one lone pair
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Polar Bond
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the effect of unequal attractions for the bonding electrons is an unbalanced distribution of electron density within the bond
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Dipole-Dipole bonds
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force of attraction exerted by the molecular dipoles (polar molecules) for one another.the larger the dipole moment (greater difference in E.N) the greater the d-d attractive forces b/w molecules
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>1.7
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values of ionic negativity
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Pauli Exclusion Principle
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only two electrons of opposite spin can occupy an orbital
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VSEPR Theory
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based on the idea that valence shell electron pairs, negatively charged, stay as far apart from each other as possible, so that the repulsions between them are at a minimum
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Polar differences
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d-d, hydrogen bonds
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As you move across a period
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the Ionization Energy increases
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covalent bond
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a chemical bond in which electrons are shared between two atoms
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linear
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sp3d three lone pairs
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As you move down a family
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the atomic radius increases
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exothermic
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releases energy
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109.5
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degree of tetrahedral shape
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linear
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sp2 2 bonding
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square pyramidal
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sp3d2 one lone pair
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Van Der Waals
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instantaneous forces of attraction between fluctuating dipoles in non-polar molecules
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t-shaped
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sp3d two lone pairs
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endothermic
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requires energy
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bond energy
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the amount of energy released when the bond is formed (or amount of energy needed to break the bond)
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hybridization
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the mixing of two or more pure atomic orbitals to form to or more hybrid atomic orbitals that are identical
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