Term
In acetylene, each carbon atom is bonded to __________ other atoms, and there are no nonbonding valence electrons.
Each carbon atom needs two hybrid orbitals to form the __________ bond framework.
Hybridization of the __________ orbital with one __________ orbital gives two hybrid orbitals, directed 180 degrees apart, for each carbon atom.
Overlap of these __________ hybrid orbitals with each other and with the hydrogen __________ orbitals gives the sigma bond framework. |
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Definition
1) Two
2) Sigma
3) s
4) p
5) sp
6) s |
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Term
In acetylene, two __________ bonds result from overlap of the two remaining unhybridized __________ orbitals on each carbon atom.
These orbitals overlap at right angles to each other, forming one __________ bond with electron density above and below the C-C __________ bond, and the other with electron density in front and in back of the __________ bond. |
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Definition
1) Pi
2) p
3) Pi
4) Sigma
5) Sigma |
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Term
| The carbon-carbon bond length in __________ is 1.20 angstroms, and each carbon-hydrogen bond is 1.06 angstroms; both bonds are __________ than the corresponding bonds in ethane and ethene. |
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Definition
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Term
The triple bond in acetylene is relatively short because of the attractive overlap of __________ bonding pairs of electrons and the high __________ __________ of the sp hybrid orbitals.
The sp hybrid orbitals are about __________-__________ s character (as opposed to __________-__________ s character of sp2 hybrids and _________-__________ s character of sp3 hybrids), using more of the closer, tightly held __________ orbital.
The sp hybrid orbitals also account for the slightly (shorter/longer) C-H bonds in acetylene compared with ethylene. |
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Definition
1) Three
2) s character
3) One-half
4) One-third
5) One-fourth
6) S
7) Shorter |
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