There are no difference in the number of shells in magnesium and sulphur. Both elements contain 3 shells. However, the total number of electrons in the shells are different. Magnesium has 12 electrons in its shells whereas sulphur has 16 electrons in its shell. In addition, the electrons in the valence shell (outermost shell) are also different. Magnesium has 2 electrons in its valence shell whereas sulphur has 6 electrons in its valence shell.
Elements are arranged into rows in order of increasing mass, so that elements with similar properties were in the same column. They are organized by type, such as nonmetals, metals, and metalloids, and solids, liquid, gas, or not found in nature.
The atomic radius of elements increases as you go down a group. This increase in radius as you go down a period is primarily caused by the increasing principal quantum number of the outer electron shells.
Atoms of these elements do not combine with other atoms, even atoms of the same element, because their valence electron shells are full.
According to the Modern Periodic Law, the properties of the elements are repeated after certain regular intervals when these elements are arranged in order of their increasing atomic numbers. Further an examination of the electronic configuration of the various elements clearly indicates that with a gradual increase in atomic number there occurs a repetition of similar outer electronic configurations after certain regular intervals. By correlating these two observations, we can say that, the cause of periodicity in properties is the repetition of similar outer electronic configurations at certain regular intervals. When we go across the period the no. of shells remains same but the number of electrons keep increasing .this result in more force of attraction among electrons and protons and thus atomic size decreases. But when we go down the group, the no. of valence electrons remains same but the no. of shells keep increasing.this result in less force of attraction. Therefore, atomic size increases.
The elements of period 3 has same number of shells as sodium. These elements are Mg, Al , Si, P , S, Cl and Ar.
As we descend down the group, the atomic radii increases. This is because the number of shells increases.
the atomic masses and atomic numbers... group number and period number... valence electrons and number of shells... these all determine the chemical properties of elements...
The elements in a group do not have the same number of shells, however, the elements in a horizontal row do have the same number of shells.
Electron shells
Atomic size increases down the group. The number of shells increases causing more atomic radius.
All of the elements in the same period (row) of the periodic table as sodium have this property.
The same number of electron shells,thus similar atomic structure.
Dmitri Mendeleev and Lothar Meyer first arranged the elements in the increasing order of atomic masses. Bohr and Henry Moseley then arranged the elements in the increasing order of atomic number.
Elements in the same column have the same number of valence electrons, and form ions with the same charge.
atoms try to get 10 electrons on shells around the atom. how many shells the atom has is based on the atomic number and atomic mass the atomic number determines how many shells their are.
Down the group, atomic radius increases. This is due to increase in number of shells.