IB Bonding cont. Flashcards
(IB) VBT
1 electron from each atom form a covalent bond
2 electron total within the “bond orbital”
(IB) higher overlap of orbitals
stronger bond
(IB) HYBRIDIZATION
atomic orbitals to form bond orbitals
(IB) hybrid orbitals are only form in
bonding (shape is still a probability function
(IB) hybrid orbitals uses energy from
intermediate energy between s and p (even d)
(IB) linear would have which hybridization
sp
(IB) trig. planar would have which hybridization
sp2
(IB) tetrahedral would have which hybridization
sp3
(IB) sp3 hybridization
electron domain geometry has a central atoms that is sp3 hybridized
(IB) sigma bonds location
centre of electron density in along the internuclear axis
(IB) SIGMA BOND
covalent bond
end-to-end ocerlap of bond orbitals
(IB) sp2 hybridization
molecules with 3 centres of electron density
(IB) PI BOND
2 lobes of electron density above and below the internuclears axis side-by-side overlap of 2 unhybridized p orbitals
(IB) what does pi bond do
restricts bond rotation, gives rigidity to the molecule
(IB) double bond has how many bonds
1 sigma and 1 pi
(IB) triple bond has how many bonds
1 sigma and 2 pi
(IB) sp hyrbidization
centre atom has linear electron domain geomertry
(IB) localized pi bond
pi bond between 2 atoms
(IB) DELOCALIZED
pi bond spread between 3+ atoms
3+ atoms each have an unhyrbridized p orbital
(IB) bond order
of bond/# of bond sites
(IB) HYBRID STRUCTURE
show each resonance structure combined
double bond = dashed line
(IB) Metallic bonding
found in pure metals and alloys (mix of metals)
(IB) electrostatic attractions in metallic bonding
between lattice of cations and delocalized electrons
(IB) how is metallic bonding different than covalent
shows delocalized electrons, moving freely throughout the piece of metal
(IB) does metallic bonding have angles
no bond alges, non-directional, the electrons aren’t trapped in any bond
