Are chemical bonds caused by strong interactions?

The strong interaction is the force acting between hadrons, and is the strongest of the four known fundamental forces between the universes, and the second shortest range (in the range of about 10 (-15) 10 (-10) m). The earliest studied strong interaction is the nuclear force between nucleons (protons or neutrons), which is the interaction that causes nucleons to combine into atomic nuclei.

The essence of chemical bonding is that the electrons around the atom are redistributed in space before and after bonding, and this distribution reduces the energy of the energy system.

All chemical reactions are essentially changes in the state of motion of the outermost electrons of an atom; The energy absorbed or released in a chemical reaction is called chemical energy, and the first of chemical energy is the result of a change in the motion state of the outermost electrons of an atom and a change in the energy level of the atom in a chemical reaction."

The two things are different, the chemical bond is a matter of electrons outside the nucleus, and the strong interaction is a matter of the nucleus, which does not belong to the scope of chemical research.

There are three types of chemical bond formation: ionic bond, covalent bond, and metallic bond. The ionic bond is the attraction between the cation and the anion due to the posito-negative charge, which is only due to the attraction caused by physical factors, and does not belong to the strong interaction. Covalent bonding is the sharing of electrons to bring each atom to a stable state, which is the interaction between electrons and the entire nucleus, and does not belong to strong interactions.

Metallic bonds are interactions between free electrons and metal cations, which also belong to the category of positive and negative attraction, and are not strong interactions.

The polarity of the <> chemical bond is determined by the difference in electronegativity of the atoms. In chemical bonds, the greater the difference in electronegativity between atoms, the stronger the polarity of the chemical bonds. Chemical bonds with strong polarity are generally more stable and harder to break than less polar ones.

To determine the polarity of a chemical bond, the following methods can be used:

Contrast the electronegativity of atoms: The more electronegative the atom, the more likely it is to form a polar chemical bond. The electronegativity of an atom can be compared using ortho-ion electronegativity (Pauling Scale) or density functional theory (DFT) indicators.

Calculate polarizability: Polarizability is a measure of how unevenly the electron density is distributed in a chemical bond. The greater the polarizability, the stronger the polarity of the chemical bond.

Calculate the dipole moment: The dipole moment refers to the rotation of the electron density in a chemical bond. The greater the dipole moment, the stronger the polarity of the chemical bond.

Calculate the electrotransfer rate: The electrotransfer rate refers to the degree to which electrons are transferred in a chemical bond. The greater the rate of electrotransfer, the more polar the chemical bond will be.

In chemistry problems, in addition to the thermal motion energy of the molecule inside the substance (that is, the simplified definition of internal energy in middle school physics, which should be strictly called thermodynamic energy), the internal energy also includes the interaction energy between atoms inside the molecule (which is not the same concept as chemical bond energy). The interaction energy between the atoms inside the molecule includes the gravitational potential energy between the electron and the nucleus, the repulsive potential energy between the electron and the electron, the repulsive potential energy between the nucleus and the nucleus (the above potential energy belongs to the electric potential energy), and the kinetic energy of the electron (excluding the kinetic energy of the nucleus, the kinetic energy of the nucleus has been included in the kinetic energy of the molecule). The sum of the above four energies constitutes the interaction energy between the atoms in the molecule, which is a negative value (such a molecule is a stable molecule), and its absolute value is the energy expended to break the molecule into isolated atoms, which is the chemical bond energy (for polyatomic molecules, it is the sum of the bond energies of all the chemical bonds in the molecule).

Therefore, at a certain temperature and pressure (thermodynamic energy is a fixed value under this condition), the greater the chemical bond energy of the molecules in the substance, the smaller the internal energy of the substance, and the more stable it can be.

In short, in a chemical problem (without considering the energy inside the nucleus), the internal energy is the sum of the thermodynamic energy and the energy of the interaction between the atoms within all molecules. where the interatomic interaction energy is the negative value of the chemical bond energy.

If you have any questions, you are welcome to ask further.

It doesn't matter, one is the energy required to crack the molecular bonds, and the other is related to the vibration of the molecule itself and the potential energy between the molecules.

Summary. Kiss No, a chemical-organic reaction with a broken double bond is not necessarily an addition reaction.

Kiss No, a chemical-organic reaction with a broken double bond is not necessarily an addition reaction.

The cleavage of double bonds can be achieved through a variety of mechanisms, including addition, elimination, rearrangement, redox, etc. Among them, the addition reaction is the most common type of double bond cleavage reaction, that is, one or more atomic groups are attached to both sides of the Shenhu double bond.

The chemical properties and structures of the reactive and generating species formed by the cleavage of double bonds can be complex, and there are a variety of possible reaction pathways and substrate characteristics.

Then this reaction is a bonus or a replacement.

Kiss This is a substitution reaction.

Doesn't it break the unsaturated bonds.

Yes, but he is the substitute response.

Are you sure. Yes dear.

Is it that as long as a small molecule comes down, whether there is a broken double bond or not, it is a substitution reaction?

No, whether or not a small molecule substance undergoes a substitution reaction depends on the reaction modification and reaction conditions involved in the chemical reaction. In many cases, small molecule substances come down to the substitution reaction, but in some cases, they can also participate in the addition of erection reactions, elimination reactions, rearrangement reactions, and other types of reactions. Whether the double bond is broken or not, Tong Jianda will also affect the judgment of the reaction type in some cases.

Chemical bonds can affect the physical properties of substances, such as the melting and boiling point of ionic crystals and atomic crystals, which depends on the strength of ionic and covalent bonds. It can also affect the chemical properties of the substance, as you said, the greater the bond energy, the more stable the substance. Chemical bonds can also explain the thermal effects of chemical reactions, bond breakage to absorb heat, and bond release to form a bond.

Chemical bond energy refers to the energy required to break a chemical bond, so the higher the bond energy, the more stable the substance and the smaller the energy.

The shorter the chemical bond, the higher the energy and melting point.

First, determine whether the chemical bond is broken during the reaction or the chemical bond is broken during the physical change.

If it is a chemical reaction, it is necessary to judge what chemical bonds are broken based on the specific type of reaction and the change of the substances in the reaction. However, in general, ionic compounds are broken by ionic bonds, and the covalent bonds that may be contained in them are discussed separately. Whereas, covalent compounds are covalent bonds that are broken, and as for what covalent bonds are broken, you need to look at the reaction specifically.

If it is a physical change, such as melting or dissolving, etc. It depends on the type of crystal.

In the case of ionic crystals, it is the ionic bonds that are broken.

In the case of molecular crystals, the intermolecular forces are broken and the covalent bonds are not broken.

If it is an atomic crystal, it is generally not discussed.

Chemical bonds are divided into ionic and covalent bonds.

A chemical reaction must occur to break the covalent bonds.

There are several cases of breaking ionic bonds:1A chemical reaction occurs2The electrolyte is soluble in water3Melting the electrolyte keeps the electrolyte in a molten state.

Strictly speaking, Shihu is not.

Chemical bonds include: ionic bonds.

Covalent bond. Metallic bonds.

They exist separately.

Ionic compounds.

Covalent compounds.

Elemental metals. Middle.

NaCl (most salts, except aluminium chloride.

All are ionic compounds.

HCl (most non-metallic compounds and aluminum chloride) are covalently compounded.

Chemical bonds exist between atoms, intermolecular forces.

Present between molecules (e.g. carbon dioxide.

Between molecules, chlorine.

There are only two forces between molecules:

Intermolecular forces. And. Hydrogen bond.

The common ones are: intermolecular staring force: halogen elemental gas (chlorochlorobromoiodine) hydrogen bond: water. Ammonia molecule.

Chemical bonds. Definition: Intense between adjacent molecules.

Interaction forces.

This is called a chemical bond.

Intermolecular forces.

It does not belong to chemical bonds, mainly including hydrogen bonds, van der Waals force, etc., which are molecules and.

Intermolecular sedan school Zen interaction.

The strength of the force, which is much less strong than the chemical bond, bond energy.

It is also much lower than the chemical bond.

The carbon-carbon double bond must be additional, and the carbon-oxygen double bond can be added with hydrogen in aldehydes and ketones; The carbon-oxygen double bonds in the carboxyl and ester groups cannot be added with hydrogen under normal conditions.