The more acidic it is, the more stable HF HCl HBr HI is

It's the other way around. HF HCL HBR HI From left to right: less stable and more acidic, so for hydrohalic acids, the stronger the acidity the more unstable, and the weaker the acidity the more stable (for dilute acids only).

Hi is the strongest acid in hydrohalic acid, which has strong reducing properties, but is extremely unstable and easily decomposed into hydrogen and iodine.

HBR is unstable, strongly acidic and reducing, and similar in nature to hydrochloric acid. It can corrode most metals.

HCL is a common acid, one of the three strong acids (nitric acid, sulfuric acid, hydrochloric acid), but the acidity is slightly weaker than hydrobromic acid and stable. It is an important chemical raw material, and is commonly used in laboratories to produce carbon dioxide and dilute acid.

Dilute HF is a weak acid and is very stable. Although HF is a weak acid, it can corrode glass, so it is usually packed in plastic bottles. (Concentrated hydrofluoric acid is also a strong acid due to disproportionation.) ）

No, the stronger the elemental oxidation, the more stable the hydride formed by combining with hydrogen.

It depends on the non-metallic properties, for example, if the non-metallic is stronger, the more stable the gaseous hydride is, rather than the stronger the acidic and more stable, so the F2 and H2 mixture** The product is the most stable, because F is the most non-metallic.

1.By hf hcl hbr hi order:

Aqueous solution acidic reducibility: enhanced;

Stability: Weakened.

2.In order:

Aqueous solution acidity: enhanced;

Stability Reductiveness: Weakened.

Rule: Stability of hydride The reducibility is consistent with the non-metallic properties of the element, whereas the acidity of the aqueous solution of hydride is not necessarily consistent with the non-metallic properties of the element.

On the contrary, strong acidity means that H+ is difficult to ionize, isn't it stable?

HI is the most acidic and the most unstable; HF is the least acidic, but the most stable.

HF is a weak electrolyte. Weak acid.

HCl is a strong electrolyte, a strong acid.

So you can't say that.

Analysis: Generally, chemical bonds.

The shorter the bond length, the greater the bond energy of the chemical bond, the stronger the chemical bond, the stronger the bond, the more stable the molecular structure, and the more difficult it is to decompose. Atomic radius of f, cl, br, i.

As the bond lengths of HF, HCL, HBR, and Hi increase, the bond energy decreases, and the stability of the molecule decreases.

Answer: The bond length of HF, HCL, HBR, and Hi increases sequentially, the bond energy decreases sequentially, and the stability of the molecule decreases sequentially.

Among the hydrohalic acids, hydrochloric acid (hydrochloric acid), hydrobromic acid and hydroiodic acid are all strong acids, and their acidity increases sequentially.

Hydrofluoric acid is a weak acid, but it becomes a strong acid when its concentration is greater than 5 mol l. The reason for this anomaly is that when the concentration of HF increases, associative ions are formed to further dissociate HF.

However, HF shows exceptions in many properties, due to the strong hydrogen bonds between HF molecules, so in hydrogen halide, it has the largest heat of melting, heat of vaporization and the highest boiling point, and the melting point is also greater than HCl and HBR. From the point of view of chemical properties, hydrogen halide and hydrohalic acid also show regular changes, and HF also shows some particularities.

The ability to absorb electrons from F to I gradually decreases, but the radius of the atom from Bright F to I increases, so the corresponding negative ions have a weaker attraction to H+, so the protons are more likely to dissociate. That is, the more acidic it is.

HF is very acidic, and HI is the strongest acid among anaerobic acids.

1. The atomic radius of F, Cl, Br, I increases, and the length of the covalent bond with H increases, which is easy to be destroyed by water and ionized H+, and the acidity is enhanced.

2. It is easy to form hydrogen bonds between HF molecules, so that HF in the solution of the same concentration is associated, resulting in a decrease in effective concentration, very little ionized H+, and very weak acidity.

HF,10,HCl H2S HF (weak, exceptional) HI,2,fluoroaluminum, bromide, iododo-sulfur, relative activity, 2, back, common strong acid HCI HBR HI H2SO4 HNO3

Hf is a weak acid is a special case, H2S is a common weak acid, 2, according to the non-metallic property, 2, H2S "HF" HCL "Hi, 1, look at his oxidation.

The more oxidizing it is, the less acidic it is. ,0,HF HCl Unsoluble water is a molecular state, and the strength of the acid is determined according to the concentration of hydrogen ions ionized by the acid molecule dissolved in water, which should be HCl>H2S>Hi>HFBy the way, hf is a special case, hcl, hbr, hi are all strong acids, hf is a weak acid, this is the law of the periodic table:

Taking the elements of the third row as the standard, the elements below the three rows are similar in nature to the elements in the third row, while the elements in the second row are special cases, Cl is in the third row, and Br, I are in the four or five lines, so Br, I and Cl are similar in nature, so Hbr, Hi, HCL are strong acids, and F is in the second row. 0,

Acidity from strong to weak: Hi>HBR>HCl>HF, where HF is a weak acid and the rest are strong acids.

The acidity of the aqueous solution of gaseous hydride mainly depends on the degree of ionization of the gaseous hydride in the aqueous solution, and the degree of ionization is related to the polarity of the bond and the polarity of the molecule, and the enhancement of the two polarities can increase the degree of ionization.

For hydrides, increased electronegativity enhances the polarity of the bond, and an increase in the atomic radius enhances the polarity of the molecule. The electronegativity of fluorine, chlorine, bromine and iodine decreases sequentially, the polarity of the bond decreases, and the degree of ionization decreases, which is a secondary contradiction. However, the atomic radius increases significantly, the molecular polarity increases, and the degree of ionization increases, which is the main contradiction. Therefore, the aqueous solution of halogen gaseous hydride becomes more acidic with the increase of atomic number, but the difference is not very large.

Hf is a weak acid because it also has hydrogen bonds between its molecules, which weakens the ionization of Hf.

Due to the hydrogen bonds between the HF acid molecules, the melting boiling point is higher.

The melting boiling point is independent of stability.

The melting boiling point is related to the intermolecular forces.

The higher the molecular weight, the greater the van der Waals force and the higher the boiling point. Hydrogen bonding is also an intermolecular force that is much stronger than van der Waals forces.

In terms of molecular weight, Hi>HBr>HCl>HF

HI is about 6 times more than HF, and the Van der Waals force is much greater than the Van der Waals force of HF. But HF has intermolecular hydrogen bonding.

In fact, the melting point of Hi is greater than that of Hf, because when the Hf solid becomes a Hf liquid, only a small part of the hydrogen bonds are broken (liquid Hf also has hydrogen bonding and polymerizes to (Hf)2 and so on). The Van der Waals force of Hi is already competing with the part of the hydrogen bond that HF breaks. The comparison between the melting point of Hi and the melting point of Hf was once presented as a question in a chemistry competition.

The melting point of Hi is much higher than that of Hf, which is about the same as HBR. HCl has a small molecular weight and no hydrogen bonding, and has the lowest melting point. i.e., Hi>HF>HBR>HCl

For the boiling point, it is the molecule that overcomes almost all the force, and the hydrogen bond strength is many times that of the van der Waals force, so the hydrogen bond containing it is higher.

Boiling Point: HF>HI>HBR>HCl

In addition to the intermolecular forces, the melting point is also related to other factors such as viscosity. For example, the melting point of hydrogen peroxide is less than that of water. Therefore, when using molecular weight comparison, it is more accurate to compare the boiling point.

Attached: specific data.

Melting point, boiling point.

hf－，hcl－，－

hi－，－

Because of the hydrogen bonding, the maximum HF, while the other molecular forces mainly depend on the relative molecular mass, and the melting and boiling point with the relative molecular mass is larger.

The acidity of hydrohalic acid Hx, from top to bottom, is enhanced.

So, HF is a weak acid.

The acidity of HCl, HBR, and HI is enhanced, and HI is the strongest acid among anaerobic acids.

It can be possible from chemical bonds.

As the radius of F-Cl-Br-I increases, the bond length of H-X increases, and the bond energy decreases, becoming more and more easily broken in water molecules.

Under the action, it is easier to break, that is, in the aqueous solution, it is easier to ionize H+, that is, the acidity is enhanced.

In the periodic table, the weaker the non-metallic nature of the non-hydrogen element, the stronger the acidity of the anaerobic acid. Since i, br, ci and f are in the same family, the order of acidity should be as follows: hi>hbr>hcl>hf.

The only criterion for judging the strength of acidity is to determine whether the hydrogen atoms in it are easily ionized into hydrogen ions in water. The more easily an acid ionizes, the more acidic it is.