What is the type of hybridization of oxygen in carbon oxygen double bond, what is the type of hybrid

The type of hybrid oxygen in the carbon-oxygen double bond is sp2 hybridization.

Because oxygen contains 6 electrons, two of which are lone pairs, must occupy two orbitals of the sp2 hybrid orbital. One orbital and carbon form a sigma bond, and one more p-electron and carbon's p-electron form a bond.

I think that when talking about atomic orbital hybridization, it only makes sense within a molecule or group, and it doesn't make sense for a bond. For example, for the CoCl2 molecule, the C in the carbon-oxygen double bond is the sp2 hybridization.

Diatomic molecules do not discuss hybridization. Oxygen is the element oxygen.

Formed as a elemental substance, the chemical formula O2, its chemical properties.

It is relatively reactive and can react with oxygen with most elements.

Oxygen is a colorless and odorless gas, and it is the most common elemental morphomorphic fissure of oxygen. Melting point , boiling point 183 . Not easily soluble in water, about 30ml of oxygen is dissolved in 1L of water. In the air, oxygen accounts for about 21%. Liquid oxygen.

for sky blue. Oxygenation is a blue crystal.

Discover History: Priestley.

Inspired by the discovery of CO2 from Blake's calcined limestone, a convex lens was utilized.

Gathering sunlight causes some substances to burn or separate to release gases and conduct research. On August 1, 1774, Priestley finally succeeded in producing oxygen, which became a significant event in the history of chemistry.

His experiment was very simple, put mercury oxide in a place filled with sparrow letter this swift silver.

Then, the glass bottle is poured into the mercury tank, the glass bottle is completely filled with mercury, the air is all excreted, and the mercury oxide floats on top. He then used a convex lens to concentrate the sun's rays and shine them on the mercury oxide, which heated it.

The above content reference: Encyclopedia - Oxygen.

Atomization.

Although the O atom is connected with 2 H atoms, the O atom also has 2 lone electron pairs, which also participate in the hybrid orbital of the O atom.

Therefore, it is sp3 hybridization, because the repulsion of the H-O bond by the two lone electron pairs is used for bucket resistance, so the bond angle is smaller than that of the sp3 hybridization, so it is unequal sp3 hybridization.

The delayed formula for judging the hybrid type of the molecular structure is: k=m+n: where the value of n is n in abn, and the number of atoms bound to the central atom m=(e-nd) 2m:

The number of lone electron pairs (refers to unbonded electrons) e: the number of valence electrons of the central atom (the number of valence electrons is the number of outermost electrons.

n: the number of atoms bound to the central atom, d: the maximum number of electrons that can be received by the atom bound to the central atom (the atom bound to the central atom refers to the h atom, and the outermost difference is 1 electron full, where d = 1). Due to hydrogen peroxide.

The central atom of is the oxygen atom.

So e is 6, n is 2, d is 1, then k=2+(6-2*1) 2=4. When k=4, the hybrid type is sp3 hybridization.

To correct a point, the carbon that is not a double bond is sp2 hybrid, but a carbon that is a carbon-oxygen double bond is sp2 hybrid.

The reason why sp2 hybridization is that the orbital of the carbon atom is explained as sp2 hybridization can explain its physicochemical properties, such as double bond properties, so it is considered sp2 hybridization.

It should be noted here that the hybrid orbital theory is a theory that explains atomic orbitals, whether it is sp or sp2 hybridization, not because it is sp or sp2 but because it is more reasonable to explain sp or sp2 hybridization, so it is sp2 hybridization.

For example, methane, methane has a tetrahedral structure, so it is obviously not appropriate to use sp hybridization to explain the atomic orbital of the carbon atom (linear structure), and it is not appropriate to use sp2 (triangular structure), but it is reasonable to explain it with sp3 hybrid orbital, so the carbon atom of methane is sp3 hybrid.

What kind of hybridization method is, the key is which hybridization method is more reasonable to explain its structure.

1.How many ways are there to hybridize carbon? What are the characteristics of each?

There are three hybrid ways of carbon: sp, sp2, and sp3. They each have the following characteristics:

Sp hybridization: Sp hybridization refers to the mixing of two hybrid orbitals with one 2S orbital and one 2p orbital in a carbon atom. This hybrid pattern is often found in tri-bonded compounds, such as olefins and alkynes.

The shape of the electron cloud on the sp hybrid carbon atom is linear, i.e., a straight line.

Sp2 hybridization: Sp2 hybridization refers to the mixing of one 2S orbital and two 2P orbitals in the carbon atom to form three hybrid orbitals. This hybrid mode is commonly found in double-bonded compounds, such as olefins.

The shape of the electron cloud on the sp2 hybrid carbon atom is a planar triangle.

Sp3 hybridization: Sp3 hybridization refers to the mixing of one 2S orbital and three 2P orbitals in the carbon atom to form four hybrid orbitals. This hybrid mode is commonly found in single-stop rebonding compounds, such as alkanes.

The electron cloud on the sp3 hybrid carbon atom is tetrahedral in shape.

2.How many types of simple hunger breaks of covalent bonds?

There are two ways to break covalent bonds, homofiguration and heterocleavage. Homolysis produces free radicals, and the reaction with the participation of free radicals is called a free radical reaction. As a result of heterocleavage, positive and negative ions are produced. The reaction carried out by the covalent bond heterocleavage to produce positive and negative ions is called ionic reaction type.

1) There are 3 ways to hybridize carbon! It is characterized by sp3 -- the shape of the mold quietly into a tetrahedron; sp2 --- coplanar; SP--- collinear!

2) There are 2 kinds of fractures of the covalent bond of the slag, the pie bond is easy to break, and the sigma bond is relatively strong!

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The type of hybridization of the carbon atom of carbon dioxanetetradinegative is that the two oxygen atoms of the carbon dioxide CO2 in the molecule form a double bond while the carbon atom does not form any bond, so the hybrid type of the carbon atom is sp orbital hybrid. Specifically, this is because one s orbital and two p orbitals of the carbon atom are mixed to form three sp hybrid orbitals. <>

Hybrid type of carbon atom with carbon dioxanetetradiminus.

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The hybrid type of carbon atom of carbon distate exatriation tetradi-negative is that the carbon dioxide CO2 forms a double bond between two oxygen mode atoms in the molecule, while the carbon atom does not form any bond, so the hybrid type of carbon atom is sp orbital hybridization. Specifically, this is because one s orbital and two p orbitals of the carbon atom are mixed to form three sp hybrid orbitals. <>

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The answer is sp2. Explained in COC, 0In the 2H2O molecule, the carbon atom is surrounded by two oxygen atoms, forming two carbon-oxygen double bonds.

Each carbon atom needs to form four bonds, so its hybrid type should be sp2 hybridization, that is, one s orbital and two p orbitals of the carbon atom are mixed to form three sp2 hybrid orbitals, and two p orbitals formed by two oxygen atoms and one unhybridized p orbital form three carbon-oxygen double bonds. <>

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Why. Kiss, unraveling the god stool release in coc,0.In the 2H2O molecule, the carbon atom is surrounded by two oxygen atoms, forming two carbon-oxygen double blind and noisy bonds. Since each carbon atom needs to form four bonds, its hybrid type should be sp2 hybridized <>

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The carbon atom in the carbon-carbon triple bond is sp hybridized, forming 2 sp hybrid orbitals and 2 unhybridized p orbitals.

The carbon-carbon triple bond contains sp-sp to form a titit bond, and two unhybridized p orbitals to form a p-p bond. The carbon-carbon triple bond is made up of one bond and two bonds together.

The C-H bond contained in acetylene is another sp hybrid orbital of each carbon atom and the S orbital of the hydrogen atom forming the bond. The carbon-carbon triple bond becomes a carbon-carbon double bond (type E) under the reduction of lithium aluminum hydride.

Chemical characteristics of carbon-carbon triple bonds:

When the triple bond carbon is connected with hydrogen, the carbon-hydrogen bond is more polar, easy to crack, and releases protons, so the acidity of terminal alkynes is stronger than that of terminal alkenes and alkanes. Under the action of commonly used catalysts palladium, platinum or nickel, it is added with H2 to form alkanes.

The carbon-carbon triple bond contains two bonds, which can be added with two molecules of hydrohalic acid. Mercury salts are often used as catalysts for addition to water. For example, the addition of acetylene to water occurs in an aqueous solution of 10% sulfuric acid and 5% mercuric sulfate. <>