Quiz 4 Flashcards
3 Types of Hybridization and their angles
sp^3: 109.5 degrees (4 electron regions)
sp^2: 120 degrees (3 electron regions)
sp: 180 degrees (2 electron regions)
Polar Molecule
-soluble in water
-greater than 0.5 difference in electronegativiy
-has asymmetry so is NOT symmetrical as such bond dipole movement won’t cancel out
-has dipoles
2 types of covalent bonds
sigma and pi bonds
Formal Charge
hypothetical charge an atom would have if it shared its electrons equally
-minimum formal charged structures are favored
FC = (# valence e-) - [# unshared e- + 1/2(# of bonding e-)]
- sum will be 0 in a neutral atom, and in ion will match ionic charge
Bond Length
-distance between two nuclei
as it increases bond order decrease as well as bond enthalpy
Bond Order
of e- pair bonds connecting two atoms (can be fractional)
as bond order increases bond strength increases and bond length decreases
- as more bonding electrons means stronger attraction between two nuclei so a shorter distance
Bond Energy
energy required to break a chemical bond (endothermic)
VSEPR
valence shell electron pair repulsion theory
-shape of molecule determined by charge repulsion between valence shell electron pairs of central atom
Hybridization:
-process where we combine atomic orbitals to produce hybrid atomic orbitals
-bonds form because it brings stability to atoms
-bonds occur when singly-occupied orbitals overlap
-atoms rearrange to allow bonding
-explained by Valence Bond Theory
Pi bonds
-formed by sideways overlap of parallel p-orbital
-e- density lies above and below plane of bonding axis
- pi bonds use unhybridized p orbitals
sigma bonds
-formed from head on atomic orbital overlap
-e- density lies between nuclei of 2 atoms
-sigma bonds often use hybrid orbitals
AX6E0
Octahedral, Octahedral, 90 and 180 degrees
AX5E1
Octahedral, square pyramidal, 90 and 180 degrees
AX4E2
octahedral, square planar, 90 and 180 degrees
AX5E0
Trigonal Bipyramidal, Trigonal bipyramidal, 90,120, 180 degrees
