How to explain the strength of hydride acidity and alkalinity in terms of electron density

The question is complicated, hydrogen can be related to the periodic table.

Neutral removal of noble gases.

The vast majority of the outer elements form hydrides. Without scoping the problem, it is difficult to explain the problem in a small amount of space (if it is a textbook, the content is enough to write a chapter). First of all, you are talking about whether the hydride is a non-metallic hydride (which can be acidic or alkaline) or a metal hydride (both are extremely strong Lewis bases, of course, there are differences in the alkalinity of different metals).

The other is to compare the hydride itself (to use the Lewis acid-base theory.

explanations), or compare their acidity and alkalinity in aqueous or non-aqueous solutions (explained by acid-base ionization theory and acid-base proton theory, respectively). In addition, there are many factors that affect acidity and alkalinity, and there is an electron cloud near hydrogen.

Density (not electron density) can only explain the gradual change law of hydride acidity of the sixth and seventh main group congeners, while there is no very clear law of hydride acidity and alkalinity between different periodic elements of different groups, which often requires specific analysis of specific problems, that is, it is necessary to comprehensively investigate the induction effect, hydrogen bonding effect, spatial effect and other factors existing in the two hydrides being compared.

It was therefore suggested that the issue be narrowed down to facilitate discussion.

Hydride acidity and alkalinity is because the more nuclear charges, the larger the radius of the atom, the more electrons outside the nucleus, the higher the electron density, the less binding the hydrogen atom, the easier it is to ionize hydrogen ions, the more acidic it is, the weaker the alkalinity.

Oxygenated acids can be expressed by electron density to indicate the strength of acidity; The lower the electron density on hydrogen, the more acidic it is.

There are many ways to compare metallicity, but the most important ones are:

1) The degree of intensity (difficulty) of the reaction with water or acid.

2) The alkalinity of the hydrate corresponding to the most ** oxide.

3) Mutual replacement.

There are also many ways to compare non-metallic properties, and the important ones are:

1) Degree of difficulty with H2 compounds, stability of hydrides.

2) The acidity of the hydrate corresponding to the most ** oxide.

3) Mutual replacement.

Stable, acidic, alkaline.

1) Alignment to the right: increasing stability of hydrides, increasing acidity, and weakening alkalinity 2) Downward of the same main group: decreasing stability of hydrides, weakening acidity, and increasing alkalinity Atomic radius:

1) In the same period, from left to right, decreasing in turn.

2) The same main family increases from top to bottom.

3) Anions of the same element are greater than their atomic radius, while cations are smaller than their atomic radius 4) For particles with the same electron shell structure, the larger the nuclear charge, the smaller the radius.

To remember the periodic table, the position of each element. It is possible to determine the metallicity and non-metallic properties of chemicals, the stability, acidity, alkalinity, and atomic radius of gaseous hydrides.

Metallicity refers to liveliness.

Reduction of nature. Non-metallic is oxidizing.

Stability depends on the chemical structure.

The atomic radius looks at the molecular weight.

Acidity and alkalinity is to see whether it is acidic or alkaline.

The closer to the lower left corner of the periodic table is the most metallic and the more alkaline it is. The closer to the upper right corner the more non-metallic and acidic it is. The more layers of electrons an atom has, the larger the radius.