Why do elements of the same period have a larger atomic radius as they go further on

This is wrong!

Combined with the periodic table, the periodic law can be expressed as:

As the atomic number increases, the properties of the elements show a periodic and gradual change law:

In the same period, the metallicity of the element decreases from left to right and the non-metallicity increases from left to right, and in the same family, the metallicity of the element increases from top to bottom and the non-metallicity decreases from top to bottom;

In the same period, the highest positive oxidation number of the element increases from left to right (except for those without positive valence), and the lowest negative oxidation number gradually increases from left to right.

The elements of the same family are similar in nature.

Atoms with the same valence electron configuration have the same theoretical tendency to gain or lose electrons, which is why the properties of elements of the same group are similar.

The above rules do not apply to noble gases.

In addition, there are some bases for judging the metallicity and non-metallicity of elements, which can be used as a supplement to the periodic law

With the gradual change from left to right valence orbit from empty to full, the elements also gradually change from predominantly metallic to predominantly non-metallic.

With the same group of elements, since the higher the period, the higher the energy of the valence electrons and the easier it is to lose, so the elements ranked below are generally more metallic than the elements above.

The stronger the reduction of elemental elements, the stronger the metallicity; The stronger the elemental oxidation, the stronger the non-metallic property.

The more basic the most ** hydroxide of the element, the stronger the metallicity of the element; The more acidic the hydroxide, the stronger the elemental non-metallic.

The more stable the gaseous hydride of the element, the stronger the non-metallic property.

The radius of the atoms of the elements of the same period decreases from left to right, and the radius of the elements of the same group increases from top to bottom (except for noble gases).

There are also some conclusions that are drawn according to the periodic law:

The stronger the metallicity of an element, the smaller its first ionization energy will be; The stronger the non-metallic nature, the greater its first electron affinity.

Among the elements of the same period, the more "empty" the orbital, the more likely it is to lose electrons, and the more "full" the orbital, the easier it is to gain electrons.

Good luck with your learning and progress.

That's right. It should be getting smaller and smaller.

Why is it that the further back an element of the same period there are more protons, the greater the attraction to the electrons outside the nucleus, and the smaller the radius of the orbit of the electron motion.

The properties of an element change periodically with the increase of the atomic number of the element.

Because the number of nuclear charges of atoms in the same period increases with the increase of atomic number, that is, the number of protons increases, then the binding force of the nucleus to the electrons outside the nucleus increases, and the closer the electrons are to the nucleus, the smaller the radius.

The atomic radius is mainly affected by two factors: the number of electron layers and the number of nuclear charges. Generally speaking, the greater the number of electron layers, the smaller the number of nuclear charges, and the larger the atomic radius, which also makes the atomic radius have an obvious periodic degeneration law on the periodic table.

The atomic radius has a great influence on the chemical properties of the element, so the study of the atomic radius has great significance and value in the development of chemistry.

Isoperiod atomic radius magnitude rule:

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.

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 atoms of the synperiodic elements gradually decrease from left to right (except for noble gases).

In general, the higher the number of electron layers, the smaller the number of nuclear charges, and the greater the atomic radius. This also makes the atomic radius visible on the periodic table.

The law of periodic degeneration.

For example, compare the radius sizes of sodium and magnesium. If the charge of a nuclear charge increases by 1 from sodium to magnesium, its nucleus increases a certain effect on each electron outside the nucleus.

force, the atom tends to shrink, and the electron outside the nucleus also increases by one electron, and the radius of the atom tends to increase because the electron moves to occupy a certain space.

Add. 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.

The effect of increasing the subradius.

(2) The main group elements of the same period, from left to right, increase with the atomic number.

The number of electrons of the main group elements in the same period is the same, while the effective nuclear charge z* increases significantly from left to right, and z* increases significantly, while the secondary group element z* does not increase significantly.

The transition element z* increases slowly, and the atomic radius decreases more slowly, although the nuclear charge increases more, but up. (3) The shielding effect of the same group of elements increases from top to bottom, and the atomic radius decreases accordingly, and the atoms of the adjacent two elements increase by an electron inner shell in turn, resulting in an insignificant increase in the effective nuclear charge.

The magnitude of the atomic radius is mainly determined by the number of electrons outside the nucleus and the effective nuclear charge The effective nuclear charge (z*) is equal to the atomic number (z) minus the shielding constant, i.e., z*=z-.

1) The effective nuclear charge increases with the increase of atomic number and changes periodically.

In the periodic table:

Same period: As the number of nuclear charges increases, the atomic radius gradually decreases (except for noble gas atoms). For example: third cycle: Na>mg>Al>Si>P>S>Cl.

The same main group: the atomic radius gradually increases as the number of nuclear charges increases. For example:

The periodic table of group ia:h chemical elements is a list of chemical elements sorted from smallest to largest according to their 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, halogen elements, noble gases, etc.

This results in the periodic table forming an elemental partition with seven primary families, seven secondary groups, and zero families.