Cyclopropane ( C 3 H 6 ) has the shape of a triangle in which a C atom is bonded to two H atoms and two other C atoms at each corner. Cubane ( C 8 H 8 ) has the shape of a cube in which a C atom is bonded to one H atom and three other C atoms at each comer. (a) Draw Lewis structures of these molecules. (b) Compare the CCC angles in these molecules with those predicted for an s p 3 − hybridized C atom. (c) Would you expect these molecules to be easy to make?
Cyclopropane ( C 3 H 6 ) has the shape of a triangle in which a C atom is bonded to two H atoms and two other C atoms at each corner. Cubane ( C 8 H 8 ) has the shape of a cube in which a C atom is bonded to one H atom and three other C atoms at each comer. (a) Draw Lewis structures of these molecules. (b) Compare the CCC angles in these molecules with those predicted for an s p 3 − hybridized C atom. (c) Would you expect these molecules to be easy to make?
Solution Summary: The author explains that the Lewis structures of cyclopropane and cubane are to be drawn and their bond angles with a mathrmsp3 hybridized carbon atom
Cyclopropane
(
C
3
H
6
)
has the shape of a triangle in which a C atom is bonded to two H atoms and two other C atoms at each corner. Cubane
(
C
8
H
8
)
has the shape of a cube in which a C atom is bonded to one H atom and three other C atoms at each comer. (a) Draw Lewis structures of these molecules. (b) Compare the CCC angles in these molecules with those predicted for an
s
p
3
−
hybridized C atom. (c) Would you expect these molecules to be easy to make?
2(a) Provide the Lewis structures for both CH3OH and C2H3Cl. 2(b) What is the largest bond angle among all the bond angles in CH3OH and C2H3Cl? Listthe three atoms making this largest bond angle, and estimate the value of the angle.2(c) What intermolecular forces are present(i) between CH3OH molecules?(ii) between C2H3Cl molecules?
Butadiene, C4H6, is a planar molecule that has the followingcarbon–carbon bond lengths:
(a) Predict the bond angles around each of the carbon atoms and sketch the molecule. (b) From left to right, what is the hybridization of each carbon atom in butadiene? (c) The middle C—C bond length in butadiene (1.48 Å) is a little shorter than the average C—C single bond length (1.54 Å). Does this imply that the middle C—C bond in butadiene is weaker or stronger than the average C—C single bond? (d) Based on your answer for part (c), discuss what additional aspects of bonding in butadiene might support the shorter middle C—C bond.
Consider the reaction BF3 + NH3 -> F3B-NH3
(a) Describe the changes in hybridization of the B and N atoms as a result of this reaction.
(b) Describe the shapes of all the reactant molecules with their bond angles.
(c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms.
(d) What is the name of the bond between B and N.
(e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product molecule.
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