CHEM 150 -ch9 and 10-

valleystudent84's version from 2015-04-15 13:36


Question Answer
All possible e- geometriesLinear, Trigonal planar, Tetrahedral, Trigonal bipyramidal, Octahedral
(E- geo) Linear = molecular geos and angle0 lone pairs = Linear (180)
(E- geo) Trigonal planar = molecular geo and angle0 lone pairs = Trigonal planar (120). 1 lone pair = bent (<120).
(E- geo) Tetrahedral = molecular geos and angle0 lone pairs = Tetrahedral (109.5). 1 lone pair = Trigonal pyramidal (107). 2 lone pairs = bent (104.5)
(E- geo)Trigonal bipyramidal = molecular geos and angle0 lone pairs = Trigonal bipyramidal (90, 120). 1 lone pair = Seesaw (<90, <120). 2 lone pairs = T shaped (<90, 120). 3 lone pairs = linear (180)
(E- geo) Octahedral = molecular geos and angle0 lone pairs = Octahedral (90). 1 lone pair = Square Pyramidal (<90). 2 lone pairs = Square Planar (90)
Lewis numbers for BI3N = 30. A = 24. S = 6
Exceptions to octet ruleH = 2, He = 2, Li = 2, B = 6, Be = 4
Lewis numbers for SbI5N = 48. A = 40. S = 8
Physical properties of IONIC BONDSHard, brittle rigid - no e- conductivity unless melted/dissolved - High melting pt, high boiling pt
Physical properties of COVALENT BONDSStrong bonding forces, weak inter-molecular forces, strong network covalent solids - poor conductors of e- - low melting/boiling pt
Physical properties of METALLIC POOLINGMalleable, soft or bendable - good conductors of e- - high melting/boiling pt, good conductors of heat.
(DEF) Ionic bondTransfer of e- (has lattice structure)
(DEF) Covalent bondSharing of e-
(DEF) Metallic poolingSharing of delocalized e- between positively charged metal ions.
(DEF) Lattice Energythe energy required to separate a mole of an ionic solid into gaseous ions
(DEF) Lattice or crystal structureatoms or groups of atoms in ordered and symmetrical arrangements which are repeated at regular intervals keeping the same orientation to one another.
Ionic bond trend for lattice energyIon size up = lattice energy down (PT ↑ and ←)
(DEF) Bond OrderThe # of e- pairs being shared between atoms (single bond is BO of 1)
(DEF) Bond energythe measure of bond strength in a chemical bond. (It is the heat required to break one mole of molecules into their individual atoms).
(DEF) Bond length Distance between nuclei (more bonds = smaller bond length)
Strength of bond lengths from largest to smallestTriple > double > single
Equation for Bond energies and it's oppositeΔH = ∑ ΔH(reactant bonds broken) - ∑ ΔH(product bonds formed) _ OPPOSITE = Heat of reaction
(DEF) Cis & polaritySame - Polar
(DEF) Trans & polarityOpposite - Non-polar
Formal charge of elementsAvailable - connected (1 for each single bond)
Formal charge NetFC of each element added up
Net FC MUST = _ of the moleculeCharge
Calculating Fractional Bond OrderTotal shared / amt of groups attached to 1 atom
Calc Fractional BO ClO2-3/2
(DEF) e- densities# of bonds + lone pairs connected to CENTRAL atom
(DEF) Resonance structuresmultiple Lewis Structures that collectively describe a single molecule. (All have FC)

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