Want this question answered?
At room temperature cyclohexane is a liquid. According to the Wikipedia article on cyclohexane, it's melting point is 6.47 degrees C and it's boiling point is 80.74 degrees C.
The molecule is H3C-CH3. At each C center the bonds are tetrahedral. There is free rotation about the C-C single bond
Solubility in water, 8.7 g/100 ml at 20°C
The H-C bond and each C-Cl bond are covalent bonds.
C-H bond is stronger
No. Cyclohexane does not contain any sufficiently electronegative atoms to promote "hydrogen bond" formation, although cyclohexane of course contains hydrogen atoms bonded to carbon atoms by covalent bonds.
rigid because of the resonance stabilization of the amide (peptide) bond and the C=O (C double bond O) cause the structure to be planar and is therefore incapable of rotation.
At room temperature cyclohexane is a liquid. According to the Wikipedia article on cyclohexane, it's melting point is 6.47 degrees C and it's boiling point is 80.74 degrees C.
It only happens around a c=c as there is no free rotation about the double bond. You need to have 2 of the same atoms/molecules on either side of that double bond. When they are both at the top or both at the bottom it is cis. When they are diagonally accross from each other it is trans. Hope this helps.... sorry if it doesnt make sense it is quite hard to discribe in words
The molecule is H3C-CH3. At each C center the bonds are tetrahedral. There is free rotation about the C-C single bond
Single bond.
Cyclopropane Cyclobutane Cyclopentane Cyclohexane Cycloheptane Cycloalkane
Solubility in water, 8.7 g/100 ml at 20°C
No. In terms of bond strength a C-C bond is stronger than a C-N bond.
It is a covalent bond.
Our local phase rotation is A-B-C. There are many systems that have rotation A-C-B as well. both are correct.
Yes. In CH3Cl, there is one C-Cl bond and three C-H bond.