How many acids is H6TeO6? Chemistry, inorganic chemistry, how many acids are these?

Structurally, H6TeO6 should be a hexa-coordinated regular octahedral structure, and the chemical environment of the six Hs is the same, which may be 6-element in the sense of proton acid. But it's like boric acid is not a 3 yuan acid but a 1 yuan Lewis acid, it may also be a Lewis acid, but even if it is, it cannot be 3 yuan, because if it is 3 yuan, it will have to combine 3 OH to become a "9 coordination", and the "9 coordination" is not a stable structure, which is different from the case of boric acid; In addition, most inorganic chemistry textbooks do not discuss the issue of several yuan acid separately, so I am still more inclined to think that it is a 6 yuan acid. However, its acidity is very weak, k1 = 6, and the k value in the future will be even smaller, and it is difficult to find specific data. I'll check the CRC again in a few days.

It should be 6 elemental acid.

Generally speaking, judging a few yuan acid is to see how many hydrogen are connected to oxygen, this question te is bonded with 6 sp3d2 mixed orbital domains and 6 oxygen, the molecular shape is a regular octahedron, and 6 hydrogen are connected to oxygen, and the solid is 6 yuan acid.

ps.In general, when drawing the structural formula of an acid, oxygen is bonded to the central atom, and the dissociable hydrogen is attached to the oxygen, and the oxygen without hydrogen must be bonded with the central atom with a coordination bond (the central atom provides the electron pair, and the oxygen provides the empty orbit domain).

With ternary acids, only three hydrogen energy really turns into ions. According to the statement upstairs, ch3cooh is a quaternary acid (it should be a monobasic acid)?

It should be a six-membered weak acid, which can be regarded as a direct connection between Te and six hydroxyl groups.

3 elemental acids. It's not that a few of the molecular formula is a few.

Rather, it depends on the number of h that can be ionized.

Hexatroic acid. There are a few H elements that are several elemental acids.

Sorry, excuse me, but I'm: The early summer rose is wrong, so it's not hydroxyl, right?!

Ternary. You'll see if -oh can be taken off??? Take it off.

This specific structure should be remembered, look at -oh, and h can be ionized only when it is connected to o.

2 elementary acids, monobasic acids, and quaternary acids.

In addition to oxygen, the most ** of oxygen group elements are +6 valence, so the general chemical formula of the most ** oxide hydrate is H2Ro4 (such as H2SO4 sulfuric acid, H2SEO4 selenic acid), but there are also compounds like H6Ro6, such as prototelluric acid H6TeO6, which does not seem to have a hydrate in the form of H4Ro5? See.

The valency of R in the hydrate of the most ** oxide of the sixth main group element R is +6 valence (except O), so its chemical formula is H2Ro4 (H4Ro5, H6Ro6 and other hydrates are not required in secondary school).

The sixth main group is the oxygen group elements, oxygen (O), sulfur (S), selenium (Se), tellurium (Te), polonium (Po), UUH six elements, of which polonium is a metal, tellurium is a metalloid, oxygen, sulfur, selenium is a typical non-metallic element. They form hydrates of the most ** oxides.

The chemical formula is H2XO4 (X stands for Oxygen Group Elements, except for oxygen).

He is 6 valence. Highest oxide RO3. Hydrate H2Ro4

1 Red: copper, Cu2O, magenta solution, phenolphthalein in alkaline solution, litmus in acidic solution, liquid bromine (dark brown-red), red phosphorus (dark red), phenol oxidized by air, Fe2O3, (FesCN) 2+ (blood red).

The white one has eh, you also go 4 HCO3 mglbro 5n you h4 cl white spirit P paraffin.

Tellurium is one of the VI A group (halogen-like) and belongs to the semi-metal.

In appearance, tellurium is not much different from most other metals, all have a metallic luster, silvery-white, and dissolve poorly in polar solvents such as water, liquid ammonia, and hydrogen sulfide.

However, if you come into contact with tellurium, you will get bad breath. This is because tellurium will bind to the oil on **, and go through a series of changes in the body to produce salted fish-flavored Te(CH3)2 and garlic-flavored H2Te, both of which will be excreted through your respiratory and urethra. As a result, the employees of the tellurium plant suffered from bad breath.

At room temperature, tellurium is divided into crystalline tellurium and amorphous tellurium. Crystalline tellurium is a spiral structure with a melting point of 452, which is oxidized to TeO2 when melted in air. It is flammable, burns and emits a blue flame, and the product is also TeO2.

It reacts slowly with sulfuric acid to form Te4S2O10, while it reacts much faster with nitric acid. Amorphous tellurium looks like black powder, but unlike crystalline tellurium, amorphous tellurium reacts faster with sulfuric acid and produces polytellurium ions, which turn the solution red.

Similar to sulfur and selenium, liquid tellurium is more reactive, for example, it can ignite sodium to produce Na2Te.

In general, simple compounds containing Te2- ions are not alkaline in aqueous solution, but (H4TeO6)2- is easily hydrolyzed to make the solution alkaline. That's because Telluric acid (H6TeO6) is not very acidic, and after ionization, it will re-adsorb hydrogen ions.

The properties that need to be embodied by chemical changes are chemical properties.