Chemistry Regarding the question of chemical bonds, hello everyone ask a question about chemical bon

The intermolecular forces refer to the van der Waals forces... Hydrogen bonding is a weak interaction between hydrogen atoms and lone pairs of electrons with strong polarity, which is divided into intermolecular hydrogen bonds and intramolecular hydrogen bonds, and the former is between water molecules. The specific definition goes to check the book.,Encyclopedia also has.。。。

The answer to the question is b

Intermolecular forces are always present, but the looser intermolecular forces are weaker, and there is no covalent bond such as H-O between the molecules.

The answer upstairs confused me, I remember that the intermolecular forces defined in high school only refer to the forces between molecules... The various chemical bonds are interatomic or intramolecular... It is recommended that the landlord check the book.。。。

Or ask the teacher. But there is absolutely no such covalent bond as O-H between water molecules...

PS: In my impression, the reason why ice has a regular shape is precisely because of the effect of hydrogen bonding...

Molecular force refers to the interaction between atoms and ions (ionic bonds, covalent bonds, metallic bonds) van der chemical force is generally present between molecules, very small, and related to the molecular potential energy in physics.

Hydrogen bonding is a special chemical bond, inspired by the characteristics of water and ice, and is believed to exist between the molecules of H2O, Hf, NH3. Representation, e.g., o-h · · o-h

Topic a, hydrogen bonding is a type of molecular interaction, and the hydrogen bond between ice and water vapor is broken.

aNitrogen is stable because of the stable structure of nitrogen and nitrogen triple bonds.

bThe boiling point of water is higher than that of hydrogen sulfide because of the presence of hydrogen bonds between water molecules.

c Thermal stability is a chemical property that is related to the chemical bond length as well as the bond energy.

dNitrogen is insoluble in water and is related to molecular polarity, in addition to "similar solubility".

Therefore, choose AC, and the hydrogen bond in item B does not belong to the chemical bond.

A chemical bond is a strong interaction between neighboring atoms within a molecule. Nitrogen, stable in nature, is related to the strength of the chemical bond between two nitrogen atoms in the nitrogen molecule, because it is a triple bond of nitrogen and nitrogen, it is difficult to break, so nitrogen is not easy to undergo chemical reactions. The boiling point of water is higher than that of hydrogen sulfide because of the presence of hydrogen bonds between waters, which are a type of intermolecular force and do not belong to chemical bonds.

Water is not easy to decompose, but hydrogen sulfide is decomposed into water and hydrogen when heated, so it shows that the hydrogen-oxygen bond in the water molecule is more stable than the hydrogen-sulfur bond in the hydrogen sulfide molecule. Nitrogen is insoluble in water because nitrogen is a non-polar molecule, whereas water is a polar molecule. It has nothing to do with chemical bonds.

Chemical bonds are related to chemical changes, and the answer is ABC

1. The essence of chemical bonds is electromagnetic force. The essence of the intermolecular force is also the same as the electromagnetic force.

2. Chemical bond is a general term for the strong interaction force between two or more adjacent atoms (or ions) in the molecule or buried crystal. The force that binds ions or atoms together is known as chemical bonding.

3. Ionic bonds, covalent bonds, and metallic bonds have different origins, and ionic bonds are formed by electron transfer between atoms to form positive and negative ions, which are formed by electrostatic action. The cause of Wang Yan's covalent bond is more complex, Lewis theory believes that covalent bond is formed by the sharing of one or more pairs of electrons between atoms, and other explanations include valence bond theory, valence shell electron mutual exclusion theory, molecular orbital theory and hybrid orbital theory. A metallic bond is a modified covalent bond that is formed by multiple atoms sharing some free-flowing electrons.

Acids are all covalently bonded, and there is no oxygen ion in kclo3, because this is actually an atomic cluster (clo3-), and the oxygen atom does not gain or lose electrons, it is chlorate that gains an electron, and together forms an ion. When there are atomic clusters, the formation of atomic cluster ions is preferred.

The electronic formula of sulfuric acid: the sulfur atom forms two coordination bonds with two oxygen atoms, and two ordinary covalent bonds with the other two oxygen atoms, and these two oxygen atoms form covalent bonds with two hydrogen atoms respectively.

There are two electrons above and two electrons on the bottom. The sulfur atom in the middle forms two coordination bonds with the other two oxygen atoms. Above and below the s. The coordination bond i.e. the shared electron pair is provided by the s alone.

The electronic formula of sodium bicarbonate is also more complex, consisting of sodium ions and bicarbonate ions, and there are also coordination bonds in bicarbonate ions.

There are no requirements for these two e-secondary school stages.

Chemical bond (chemical

bond) refers to the strong mutual attraction between adjacent atoms (or ions) within a molecule or crystal.

For example, in a water molecule, 2 hydrogen atoms and 1 oxygen atom are chemically bonded to form a water molecule. There are 3 limit types of chemical bonds.

i.e. ionic, covalent, and metallic bonds. Ionic bonds are attractions produced by heterosexual charges, such as chlorine and sodium bonded to NaCl. A covalent bond is the attraction of two or more atoms through the common electrons, and a typical covalent bond is formed by two atoms by attracting a pair of bonding electrons.

For example, two hydrogen nuclei attract a pair of electrons at the same time, forming a stable hydrogen molecule. Metallic bonds, on the other hand, are interactions that bind metal atoms together and can be seen as highly delocalized covalent bonds. A chemical bond that is positioned between two atoms is called a localized bond.

A polycentric bond formed by the common electrons of multiple atoms is called a delocalized bond. In addition to this, there are also transition types of chemical bonds: covalent bonds where the bond electrons are biased towards one side are called polar bonds, and chemical bonds that are supplied by one side to form bonds are called coordination bonds.

The limits of both ends of a polar bond are ionic and non-polar bonds, and the limits of both ends of a delocalized bond are a localized bond and a metallic bond.

I don't know how much you have learned chemistry now, but if you know structural chemistry, you can judge by the electronegativity difference of the elements. Polar covalent bonds are formed between the atoms of two elements with an electronegativity difference greater than the electronegativity difference, and an ionic bond is formed when the two elements with an electronegativity difference greater than are combined.

If you don't understand, the easiest way: metal + non-metal is generally an ionic bond; Non-metal + non-metal are generally covalent bonds. Common exceptions: aluminum chloride is a covalent bond, ammonia monohydrate and ammonium salts are ionic bonds.

When hydrogen and metal are combined, it is a negative valence hydrogen ion (of course, an ionic bond); The combination of non-metals is a positive monovalent, covalent bond. Also, what do you mean by "electron"? Is it hydrogen ion [H+]?

Acid molecules (sulfuric acid, hydrochloric acid, etc.) are themselves covalent compounds and do not contain ionic bonds, but in aqueous solution, the covalent bonds are broken, resulting in ionization of hydrogen ions. For the analysis of acid molecules, the covalent bond is used.

Ionic bonds: metals or NH4+ with non-metals.

Covalent bonds: non-metal vs. non-metallic.

Sulfuric acid is both non-metallic, so it forms a covalent bond.

1 mol of silicon contains 1 mol of silicon atoms, in the crystalline silicon structure, each silicon atom is connected to the surrounding four silicon atoms by four covalent bonds, for each bond, belongs to two silicon atoms at the same time, then.

The number of chemical bonds possessed by each silicon atom is 4*1 2=2, so one mole of silicon element contains 2 moles of silicon-silicon bonds.

1mol of silicon dioxide contains 1mol of silicon atoms, and each silicon atom can form four single bonds in the silica structure, so 1mol of silica contains 4mol of oxysilica bonds. (Note: One oxygen atom is shared by two silicon atoms at the same time, so the ratio of the number of silicon atoms to the number of oxygen atoms is 1:.)

The structure of diamond is similar to that of crystalline silicon, so 1 mole of diamond contains 2 moles of carbon-carbon bonds.

The above three species are similar in that the silicon atom or carbon atom is in the center of a tetrahedral composed of four connected atoms.

The law of a bond is a single bond, a double bond, and a triple bond.

The carbon-carbon bond in the benzene ring can be considered to be a superposition of single and double bonds, so the length is between single and double bonds.

Choose a first three build lengths, double bond lengths, single bond lengths, you know.

However, benzene has a co-choke pie bond, which makes the double bond hybridized with the single bond, and the carbon-carbon bond of benzene can be obtained on average, which is greater than the single bond and less than the double bond.

So. Ethane is the largest, benzene is second, ethylene is second, and acetylene is the smallest.

Do you understand.

One nitrogen molecule has 3 nitrogen-nitrogen bonds, one hydrogen molecule has 1 hydrogen-hydrogen bond, and one ammonia molecule has 3 nitrogen-hydrogen bonds.

Chemical bonds bond to release energy, and vice versa.

So (the calculation will do.)

Write the equation first.

3h2+n2==2nh3 △h=

Let nitrogen hydrogen be x

3*Solve x.