Chemistry, what is the relationship between atomic radius magnitude and relative atomic mass? Thank

There are three factors that affect the radius of the atom: one is the number of nuclear charges, the more the number of nuclear charges, the greater the gravitational pull of the nucleus on the electrons outside the nucleus (causing the electrons to shrink to the nucleus), the smaller the atomic radius;

The second is the number of electrons outside the nucleus, because the electron movement occupies a certain space, the more electrons, the larger the atomic radius;

The third is the number of electron shells (the hierarchical arrangement of electrons is related to the size of the space near and far from the nucleus and the mutual exclusion between the electron clouds), the more electron shells, the larger the atomic radius.

The main factors that determine the relative atomic mass of an element are the number of protons and neutrons, because the mass of the electron is very small, only equivalent to 1 1836 of the mass of protons or neutrons, which is almost negligible, so the mass of the atom is mainly concentrated in the nucleus, and the nucleus is composed of protons and neutrons, so the relative atomic mass is determined by the number of protons and neutrons

In the same family, the larger the atomic number, the more layers, so the radius is larger. In the same period, the number of atomic layers is the same, and a larger atomic number means that there are more electrons in the outermost shell, and the nucleus.

The attraction is large, so the radius is small. The atomic number can traditionally be equated with the relative mass of the atom.

The larger the relative atomic mass, the larger the radius, hydrogen is a non-metal with the smallest radius, the more layers there are, the larger the radius of the same layer in the periodic table from left to right, the larger the atomic number, the smaller the radius, the same column, the larger the atomic number, the larger the radius, hope, listen to my exam this category will not be wrong.

Relative atomic mass is commonly used in junior high school:

Hydrogen H (1), Carbon C (12), Nitrogen N (14), Oxygen O (16), Sodium Na (23), Magnesium Mg (24).

Aluminum Al (27), Silicon Si (28), Phosphorus P (31), Sulfur S (32), Chlorine Cl (Potassium K (39).

Calcium Ca (40), manganese Mn (55), iron Fe (56), copper Cu (zinc Zn (65),

Silver AG (108), barium BA (137), iodine I (127).

Relative Atomic Mass Table:

1. It refers to the arrangement according to the atomic number. The data in this table is derived from the most recent periodic table, and is based on 12c=12. The atomic masses in square brackets in this table are the half-lives of the radioactive elements, the first backup, and the number of isotope mass rolls.

2. The uncertainty relative to the last digit of the atomic mass is added in parentheses after it. The atomic weight plus the square brackets is the mass of the isotope with the longest half-life of the radioactive element.

3. Since the actual mass of atoms is very small, it is very troublesome if people use their actual masses to calculate, for example, the actual mass of a hydrogen atom is kilograms, and the mass of an oxygen atom is kilograms.

4. The mass of a carbon-12 atom is kilograms. The relative atomic mass of an element is the weighted average of the relative atomic mass of its various isotopes. The lowest number in the periodic table is the relative atomic mass.

5. Relative atomic mass refers to the ratio of the average atomic mass of any atom to the 1 12 atomic mass of a carbon-12 atom based on the ratio of 1 12 of the atomic mass of a carbon-12 atom to the relative atomic mass of the atom. The atomic weight is a unit of mass, the symbol u, which is defined as 12 12 of the atomic mass of carbon.

Different atoms have different radius sizes, so the radius size of one atom is not certain. The radius of an atom refers to the distance from the center of the atom to the outermost position of the electron in the outermost electron orbital, usually expressed in pico-meters (pm) or angstroms ( ). The magnitude of the radius of different atoms depends on their electron configuration and the charge number of the nucleus.

The electron configuration of an atom refers to the arrangement of electrons in an atom, and the electron configuration of different atoms may affect the size of the atom. For example, as the number of electrons in the valence shell of an atom increases, its radius usually increases. In addition, the increase in the number of nuclear charges of an atom will also reduce the radius of the atom because the increase in the number of protons in the nucleus will attract more electrons and make the electron cloud more compact, thus reducing the size of the atom.

In conclusion, the radius size of different atoms is different and can be affected by a variety of factors. Through the study of atomic radius, we can have a deeper understanding of atomic structure and chemical properties, which is of great significance for the research and application of chemistry, physics and other fields.

The comparison law of atomic radius is as follows: the atomic radius of atoms of the same periodic element gradually decreases from left to right; The atomic radius of the atoms of the same main group elements gradually increases from top to bottom. Atomic radius is a parameter that describes the size of an atom.

According to different scales and measurement methods, the definition of atomic radius is very different, the common ones are orbital radius, van der Waals radius, covalent radius, metal radius, etc. The atomic radius of the same atom according to different definitions can vary greatly, so when comparing the relative sizes of different atoms, the data used must be consistent.

Isoperiod atomic radius magnitude rule:For example, compare the radius sizes of sodium and magnesium. If the nuclear charge increases by 1 from sodium to magnesium, the nucleus increases a certain force on each electron outside the nucleus, and the atom tends to shrink, while the electron outside the nucleus also increases by one electron, and the atomic radius tends to increase because the electron movement occupies a certain space.

Experiments have shown that the atomic radius of sodium is greater than that of magnesium, which indicates the effect of the increased nuclear charge on the reduction of the atomic radius. Thus, the atoms of the co-periodic elements gradually decrease from left to right (except for noble gases).

The above content refers to: Encyclopedia - Atomic Radius.

How does the radius of the proto-hidden xun compare the size?

The size of the atomic radius is generally compared according to the position of Yuanchang tapoin in the periodic table, and the atomic radius gradually increases from top to bottom.

Look at it three times in turn:

If you look at the number of electron layers, when the large radius and large electron layers are the same.

Second, when looking at the number of nuclear charges, when the number of electronic layers is the same and the number of nuclear charges is the same.

Third, look at the number of electrons in the outermost shell, the radius of many is larger, such as the radius of chloride ions is greater than the chlorine atom, I taught students to memorize like this when I was a teacher, and it is much better than several in other books.

Ionic radius: 1. Ions with the same number of electron layers are judged according to the size of their nuclear power cores: the ionic radius of the nuclear power nucleus is small, and the ionic radius of the nuclear power nucleus is large;

2. Ions with different electron layers are judged according to the number of electron layers: the ion radius of the ion with more electron layers is large, and the ion radius of the ion with less electron layer is small.

Atomic radius: 1. If in the same period, the larger the atomic number, the smaller the radius.

2. If it is not the same cycle, the larger the period, the larger the half-meridian.

3. For the same atom, the anion semi-meridian and the atomic semi-meridian are greater than the yang sub-meridian.

4. For the same number of electrons and the number of atomic layers, the semi-meridian is as small as sodium and fluorine).

Atomic radius refers to the radius of the electron cloud around the nucleus. The radius of the atom is determined by the distribution of the electron cloud, which in turn is affected by the charge number of the atom and the mass of the nucleus.

In the same element, the higher the charge number of the atom, the denser the electron cloud of the atom will be, and the radius of the atom will be smaller. In the same element, the greater the mass of the atom, the denser the electron cloud of the atom will be, and the radius of the atom will be smaller.

However, the influence of these two factors is limited, so in the same element, the atomic radius is not getting smaller and smaller. For example, in the third period element, the atomic radius from lithium to chlorine tends to decrease first and then increase. Thus, the atom with the largest atomic radius is probably the one with a smaller charge number and a larger mass in the same element.

Note that atomic radius is not an absolute quantity, it is relative and depends on the method and standard of measurement.