What else can you get from the periodic table about the elements?

The following information can be obtained from each square of the periodic table: atomic number, element name, element symbol, extranuclear electronic configuration, atomic weight, element classification (metallic or non-metallic, or transition element, or noble gas).

The ordinal number (number of protons) of the element

Relative atomic mass (mass number).

The elements are metallic and non-metallic and do not emit radiation.

Periodic Family E-Book Outermost E-Book Valence electron configuration.

1 atomic radius.

1) The atomic radius of the periodic elements (except the noble gas elements) decreases with the increasing atomic number, except for the first period;

2) The atomic radius of elements of the same group increases from top to bottom as the number of electron layers increases.

2 Elemental valence.

1) Except for the first period, from left to right in the same period, the highest positive valence of elements increases from alkali metal +1 to +7, and the negative valence of non-metallic elements increases from carbon group -4 to -1 (except for fluorine without positive valence and oxygen without +6 valence);

2) The highest positive and negative values of elements in the same main family are the same.

3) All elements are zero-valent.

3 The melting point of an element.

1) With the increase of atomic number of elements in the same period, the melting point of the elemental element increases, and the melting point of the non-metallic element decreases.

2) From top to bottom, the melting point of the elemental metal element decreases, and the melting point of the non-metallic elemental increases.

4 Metallicity and non-metallicity of the elements.

1) The number of electron layers of an element in the same period is the same. Therefore, with the increase of the number of nuclear charges, the easier it is for atoms to obtain electrons, decreasing metallicity from left to right, and increasing non-metallic properties.

2) The outermost number of electrons in the same main group element is the same, so with the increase of the number of electron layers, the atom is more likely to lose electrons, increasing in metallicity from top to bottom, and decreasing in non-metallic property.

5 The most ** acidity and alkalinity of oxides and hydrates.

The stronger the metallicity of the element, the stronger the alkalinity of the hydrate of its most ** oxide; The stronger the non-metallic nature of the element, the more acidic the hydrate of the most ** oxide.

6 Non-metallic gaseous hydrides.

The stronger the element non-metallic, the more stable the gaseous hydride. The stronger the non-metallic nature of the non-metallic elements in the same period, the more acidic the gaseous hydride aqueous solution is. The stronger the non-metallic nature of the non-metallic elements of the same main group, the weaker the acidity of the gaseous hydride aqueous solution.

7. Oxidation and reduction of elemental matter.

The stronger the metallicity of the general element, the stronger the reduction of its element, and the weaker the cationic oxidation of its oxides; The stronger the non-metallic nature of the element, the stronger the oxidation of its elemental substances, and the weaker the reducibility of its simple anions.

This paragraph] infers the law of the position of the elements.

The law that should be kept in mind to determine the position of an element in the periodic table:

1) The number of periodic elements is equal to the number of electron shells outside the nucleus;

2) The ordinal number of the main group elements is equal to the number of electrons in the outermost shell.

The radius of anion and cation is distinguished by the magnitude of the law.

Since the anion is the outermost shell of electrons, the electrons are gained, and the cations are the ones that have lost electrons.

So, in general, (the same element).

1) Radius of cations (atomic radius.

2) Anion Radius》Atomic Radius.

3) Anion Radius》Cation Radius.

4) Or to summarize in a word, for ions with the same extranuclear electronic configuration, the larger the atomic number, the smaller its ionic radius.

A lot. The relative atomic mass of 1 atom.

2 The corresponding family of each atom (the same group has similar chemical properties) 3 Whether the individual atom is a metal or a noble gas.

4 Whether the individual atoms are radioactive or not.

5 Electron distribution in each layer of each atom.

That's all the basic periodic table that advanced scientists use, and I can't go on and on.

Elemental major axes, secondary axes, atomic weights, elemental properties (e.g. metal or non-metal), etc.

From the periodic table, we know the relative atomism of each atom. The corresponding family of each atom (the same group has similar chemical properties.

Whether the individual atoms are metals or noble gases.

Whether the individual atoms are radioactive or not.

The distribution of electrons in each layer of the individual atoms.

Periodic table of chemical elements.

A list of chemical elements sorted from smallest to largest according to atomic number. The list is generally rectangular in shape, with spaces in the period of some elements, so that elements with similar characteristics are grouped into the same family, such as alkali metal elements, alkaline earth metals, and halogen group elements.

Noble gases, etc.

This results in the formation of meta-pure state partitions in the periodic table, which are divided into seven main groups, seven secondary groups, families, and 0 groups. Because of its ability to accurately ** the properties of various elements and the relationships between them, it is widely used in chemistry and other scientific fields as analytical chemistry.

Useful frameworks for behavior.

A lot. The relative atomic mass of 1 atom.

2 The corresponding family of each atom (the same group has similar chemical properties), 3 Whether each atom is dry or not, whether it is a genus of gold or a noble gas.

4 Whether the individual atoms are radioactive or not.

5 Electron distribution in each layer of each atom.

The main discoverers of the periodic table areMendeleev.

The ancient Greeks believed that there were four elements: water, earth, fire, and air, while ancient China believed in the five elements of metal, wood, water, fire, and earth. It is only in modern times that people have come to understand that there are many kinds of elements, and there are more than four or five.

In the 18th century, scientists have discovered more than 30 kinds of elements, such as gold, silver, iron, oxygen, phosphorus, sulfur, etc., and by the 19th century, 54 elements have been discovered.

Russian scientist Mendeleev discovered the periodic law of the elements, unraveling the mystery of the grinding cavity.

Ivanovich Mendeleev was born on February 7, 1834 in Topolsk, Siberia, where his father was the principal of the secondary school. At the age of 16, he entered the Department of Natural Sciences Education at the St. Petersburg Pedagogical Institute. After graduating, Mendeleev went to Germany for further studies, concentrating on physical chemistry.

In 1861 he returned to China and became a professor at St. Petersburg University.

When compiling lecture notes on inorganic chemistry, Mendeleev found that the Russian textbooks of this blind subject were outdated, and the foreign language textbooks could not meet the new teaching requirements, so there was an urgent need for a new textbook on inorganic chemistry that could reflect the level of development of contemporary chemistry.

This thought inspired the young Mendeleev. When Mendeleev wrote chapters on chemical elements and the properties of their compounds, he ran into a difficult problem. In what order?

At that time, there were 63 kinds of chemical elements discovered in the chemical community. In order to find a scientific way to classify the elements, he had to study the intrinsic connections between the elements in question.