A carbon carbon bond can be rotated, which means that the carbon carbon bond has the characteristics

It should be written in parentheses

It is a Greek alphabet pronounced si ge ma (the first sound is pronounced according to the English pinyin rules, and the last two sounds are pronounced according to the Chinese pinyin rules).

The meaning of bond is carbon-carbon single bond. So strictly speaking, it is also correct to write "single" or "carbon carbon single" in parentheses.

Reason. A carbon-carbon single bond, also known as a bond, is formed by the overlapping of two carbon atom hybrid orbitals head-to-head on the electron region. See ** for the appearance of the hybrid orbitals of carbon atoms.

As you can see, the hybrid orbital has a rotation axis from start to finish. Therefore, the rotation of the atoms according to this axis has no effect on the orbital itself, so even if the orbital becomes a chemical bond and connects with other carbon atoms, because the rotation of the atom has no effect on the orbit itself, it is not limited by bonding.

If the chemical bond is not a hybrid orbital bond, then it is generally not possible to rotate.

In secondary school, it is possible to rotate a single key, so fill in the brackets.

Only carbon-carbon single bonds can rotate.

A single key can be rotated. The double key cannot be rotated.

Hydroxyl oxygen and hydrogen must be coplanar (because the two are collinear), but this plane is said to be with the benzene ring.

The plane in which it is located (i.e., hydroxyl oxygen and carbonyl group.

in the plane) does not have to be the same plane. What you want to convey should be:

Why hydroxyhydrogen is not necessarily coplanar with benzene ring.

To put it simply, because hydroxyl oxygen is sp hybridized, and the O-H bond can be rotated. Since it is sp hybridization, then hydroxyl oxygen is located in tetrahedron.

, while hydroxyl hydrogen is located at one of the vertices of the tetrahedron, while the benzene ring is located in the planeIt is just a plane that passes through the center of the tetrahedron to the line where the other vertex is located. Geometrically, it is clear that hydroxyhydrogen is not necessarily on this plane. Unless this plane passes through a straight line where hydroxyl oxygen and hydroxyhydrogen are located.

Since it can be rotated, then the hydroxyl hydrogen will have the O-H bond as the axis of rotation, and the hydroxyl oxygen as the center of rotation, in the whole bodyThree-dimensional spaceMake a rotation. Then, in the process of rotation, it is possible to rotate the straight line where the hydroxyl oxygen and hydroxyhydrogen are located to the plane where the benzene ring is located.

It can be 1-phenyl-1-cyclohexene, 2-phenyl-1-cyclohexene, 3-phenyl-1-cyclohexene.

Carbon-carbon triple bonds are more stable than carbon-carbon double bonds, so why are carbon-carbon triple bonds more likely to break than carbon-carbon double bonds?

Hello dear. I can provide you with the following references; Although carbon-carbon triple bonds are more stable than carbon-carbon double bonds, the reason why carbon-carbon triple bonds are more likely to break than carbon-carbon finger-sensitive double bonds is because of their bond energy. The bond energy of a carbon-carbon triple bond is higher than that of a carbon-carbon double bond, which means that more energy is required to break the carbon-carbon triple bond.

However, since the carbon-carbon triple bond has a higher spring-only bond energy, the energy released at the time of fracture is also greater, which makes the carbon-carbon triple bond cleavage more likely to occur. In addition, the length of the carbon-carbon triple bond is also shorter than the carbon-carbon double bond, which makes it easier to break. Therefore, while carbon-carbon triple bonds are more stable than carbon-carbon double bonds, in some cases, carbon-carbon triple bonds are still more likely to break than carbon-carbon double bonds.

You see, I've marked you with three red dots on the diagram, and these three red dots are in a straight line.

The benzene ring on the left has 6 Cs, plus the carbon in the two methyl groups is 8, plus the three red dots, isn't it 11.

Answer: The left-hand of a chiral carbon molecule cannot become right-handed by rotating its bonds.

Explanation: Chiral molecule refers to the phenomenon of the presence of enantiomers in the molecule, and the same is true for chiral carbon molecules. Chiral carbon molecules have two structures, left-handed and right-handed, and their three-dimensional configurations are asymmetrical.

Therefore, the left-handed and right-handed hands of the chiral carbon molecule cannot be disturbed into each other's structures by rotating its bonds. This is because rotational carbon-carbon single bonds or carbon-hydrogen single bonds can only change the relative position of atoms in the molecule, not their configuration. Therefore, the satire-bridge left-handed chiral carbon molecule can only be left-handed, and the right-handed chiral carbon molecule can only be right-handed.

Expansion: The enantiomers of chiral molecules have the same chemical properties, but their biological and pharmacological properties can be very different. This is because the biological and pharmacological properties of chiral molecules are related to their interaction with molecules in living organisms, whereas for enantiomers of chiral molecules, their interactions with molecules in living organisms may change due to differences in stereoconfiguration.

Therefore, the study of enantiomers of chiral molecules is of great significance for drug discovery and Lao Li Meng Medicine.

Yes, a left-handed carbon molecule can be implicitly bonded by rotating its bond to become right-handed. This is because the bonds of carbon atoms can rotate and their bonds can be converted between left-handed and right-handed ones. This conversion can be achieved through a process called "carbon bond rotation".

Carbon bond rotation is a chemical reaction that can invoke the bond of a carbon atom from left rotation to right rotation or vice versa. The process of carbon bond rotation requires a substance called a "carbon bond spinner" which helps the bonds of carbon atoms to rotate from left to right. Carbon bond spinner can be an organic and a companion or an inorganic substance, both of which can help the bond of the carbon atom to rotate from left to right.

Carbon bond spinners can be achieved by a reaction called the "carbon bond rotation reaction", which causes the bonds of carbon atoms to rotate from left to right.

A single bond is a key.

A double bond is a key and a key.

A triple bond is a bond and two bonds (plain terms).

Bonds are hard to break.

Whereas the key is more easily broken (unstable.

susceptible to attack by electrophiles such as halogens).

The addition reaction only destroys the bonds in the double and triple bonds, but not the bonds, so the double and triple bonds are more active than the single bonds.

Whereas, double bonds, triple bonds eventually become single bonds by addition.

To break a single bond, it takes means such as high temperature (which requires a lot of energy).

by molecular orbital theory.

Three keys are not simply one key and two keys.

The electrons in those two bonds can form a new molecular orbital which reduces their own electric potential energy.

More stable. This makes the electrons in the triple bond less susceptible to attack by electrophiles (compared to double bonds), so it is not.

The triple bond has two keys.

It's like a double key.

More lively, so livelyness is.

Double Bond, Triple Bond, Single Bond.

Butane rotates carbon-carbon single bonds, observed every 60°, and when rotated 360°, how many different conformations can be obtained? That.

Butane is a four-carbon straight-chain alkane that has a variety of conformations due to its presence of four different substituents. Specifically, the rotational carbon-carbon single bond of butane can produce different conformations, including: cis and trans conformations.

In cis conformation, two substituents are on the same side of the adjacent carbon atoms, whereas in the trans conformation, these two substituents are on the opposite side of the adjacent carbon atoms. For butane, a single rotation can produce two different conformations of the circle (cis and trans). So, when rotated 360°, you can get 6 different conformations, because every 60° you produce two different conformations, so 360° can get 6 different conformations.

Carbon-carbon double bond: A covalent bond formed by two carbon atoms combining by two pairs of shared electrons.

Carbon-carbon triple bond is a covalent bond formed by two carbon atoms combining three pairs of shared electron pairs.

Carbon-carbon double bonds and carbon-carbon triple bonds are two common forms of compounds, both of which are unsaturated bonds that are prone to electrophilic reactions, cleavage and the formation of new shared electron pairs. Stability is relative, and it is not absolute. In the benzene ring carbon chain, it is generally considered to be composed of carbon-carbon single bonds and carbon-carbon double bonds alternately connected, and the carbon bonds are relatively stable.

Hello, I am glad to serve you and give you the following answers: Answer: The bond energy of carbon-carbon single bond is greater than that of oxy-oxygen single bond is that the carbon atom is buried and has a larger atomic radius than the oxygen atom, so the bond length of the carbon-carbon single bond is longer than that of the oxygen-oxygen single bond.

Solution: 1. Understand the concept of atomic radius: atomic radius refers to the radius of the electron cloud around the nucleus, which can contain ants to measure the size of atoms.

2. Understand the formation process of carbon-carbon and oxygen-oxygen single bonds: the formation process of carbon-carbon single bonds is that carbon-carbon single bonds can be formed due to the large atomic radius of carbon atoms; The formation process of oxygen-oxygen single bond is that only oxygen-oxygen single bond can be formed due to the small atomic radius of the buried atom in the oxygen tank. 3. Understand the bond energy of carbon-carbon and oxygen-oxygen single bonds

The bond energy of a carbon-carbon single bond is greater than that of an oxygen-oxygen single bond because the atomic radius of a carbon atom is larger than that of an oxygen atom, so the bond length of a carbon-carbon single bond is longer than that of an oxygen-oxygen single bond, thus the bond energy of a carbon-carbon single bond is greater than that of an oxygen-oxygen single bond.