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21 Cards in this Set
- Front
- Back
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-n describes the ____ of an orbital
-l describes the ____ of an orbital -m describes the number of ____ orbitals an element possesses choices: shape size atomic |
size
shape atomic |
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the n level describes the energy level (1, 2, 3,...)
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measure of size
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the smaller the n number...
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the smaller the energy level...
the closer it is to nucleus |
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s orbital
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spherical
symmetrical centered on the nucleus |
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p orbital
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composed of two lobes
symmetrically about nucleus contain a node |
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node
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an area where the probability of finding an electron is zero
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d orbital
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4 symmetrical lobes
2 nodes |
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when two atomic orbitals combine, they form a ____ orbital
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molecular
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if the signs of the wave functions are the same for the molecular orbital, they form a bond/non-bond orbital
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lower energy = bond
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if the signs of the wave functions are different for the molecular orbital, they form a bond/non-bond orbital
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higher energy = non-bond
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sigma bond
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head to head or tail to tail overlap
single bond accommodate 2 electrons |
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pi bond
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when two p orbitals line up in parallel (8 8); electron clouds overlap
-2 bonds form; double bond sigma and pi bond |
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triple bond
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2 pi bonds and a sigma bond
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double/triple bonds both ____ rotation
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hinder
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pi bonds ____ a sigma bond
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require
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pi bonds are ____ than sigma bonds in comparison, but strength is additive(strength of pi bond and sigma bond of the double bond) so therefore double/triple bonds are ____ overall
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weaker
stronger -breaking single bond requires more energy than a pi bond... |
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the more bonds between molecules, the ____ the distance between them
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shorter
1>2>3 (bond length) |
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sp3
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3p orbitals
1s orbital forms a tetrahedran if no electron pairs |
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s character and sp3, sp2, and sp....
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sp3 < sp2 < sp < s
25%<33.3%<50%<100% |
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sp2
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120degree angles
planar alkenes |
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sp
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triple and single bond
180degree angle |
