1.5 Hybrid Orbitals Flashcards
what creates stronger bonds in orbitals
the better overlap between the orbitals the stronger the bond
what do bond involve
the sharing of spin-paired electrons
in organic chem what is the most common valence orbitals available
S and P
what is hybridization
it is a simple theory that can help explain why geometry can be linear, trigonal plainer, or tetrahedral
what is hybridization orbitals
S and P orbitals overlapping
if we have a carbon (valence e is 2S2, 2P2) and hybridization occurs what happens to the configuration
it becomes sp3 this means one s + 3p (25% s and 75% p) and all _ _ _ _s get filled with electrons and moved to the same heights. and we call this atom 3 P hybridized
if we combine 2s orbitals with the 2p, 2p, 2p orbitals we get…
four sp3 orbitals distributed in a tetrahedral
how many lobes do SP3 orbitals have
the combination of the s and the p orbitals cause it to has 2 lobes like p orbitals but one is smaller then the other
what kind of hybridization can pi bonding be explained
by sp2 hybridization
if a atom is sp2-hybridized how many orbitals does it have and what are they made from
it has 3 orbitals made from one s and two p orbitals
what is the precent compisition of sp2-hybridized orbitals
they are 33.3% s and 66.6% p
what has more energy sp3 or sp2
sp3
explain how the electrons fill when there is a sp2 hybridization
there is sp2 _ _ _ with one arrow (these are hybridized
and there is a 2p _ with a arrow (this is not hybridized)
in a sp2 hybridization are all orbitals hybridized
no there is one unhybridized p orbital
what kind of bonds does sp2-hybridized allow for
the formation of double bonds if 2 p orbitals each with electron are on atoms connected by a sigma bond
if we combine the 2s orbitals with the 2px, 2py we get…
three sp2 orbitals (and keep 2pz)
for the sp2 hybridization what do the orbitals look like
the three sp2 have two lobes (one bigger, one smaller) and they are distributed in a trigonal planer
the un hybridized p orbital does not change (2 same sized lobes)
what is they hybridization of methane (CH4)
sp3
what is the hybridization of ethylene (C2H4)
sp2
in ethylene (C2H4) explain how the structure creates double bonds
there is 2 tetrahedral shape of hybridized sp2 carbon orbitals and they over lap creating a sigma bond
there is 2 un hybridized p bonds that hover electrons causing pi bonds
these two bonds create double bonding
if we combine the 2s orbital and the 2px orbital we get…
two sp orbitals (and keep the 2py and 2pz)
describe the shape of a sp orbital
the two sp hybrids would have two lobes one bigger then the other
the un hybridized 2py and 2pz will have two same sized lobes
what are the anges between the new sp hybridized orbitals
they are 180 degrees so the geometry is linear
list the charictrisitc of an orbital with 2 groups
-it (can/has?) have a triple bond
-its linear
-it is sp hybridized
-2=1+1
