Effective nuclear charge (Z) increases going across a row in the Periodic Table. So when increasing amounts of protons and electrons to an atom(within the same level or row) the protons are more able to hold onto electrons tightly , reducing size.
Sodium (Na) has 11 protons in its nucleus, 1 valence electron, and 10 non-valence (inner shell) electrons. Because the charges of protons and electrons are equal and opposite, we can say that one electron will cancel out one of the protons. So those 10 inner shell electrons are going to cancel out 10 of those protons in the nucleus. Now let's focus on that one outer electron. Because the 10 inner-shell electrons have taken up 10 protons, the valence electron is held on by only one proton. Thus, its effective nuclear charge is 1.
Magnesium (Mg) has 12 protons in its nucleus, 2 valence electrons, and 10 non-valence electrons. As with the sodium atom, the 10 inner shell electrons cancel out 10 of the protons. Then we look at one of the two valence electrons. It will be held on by 2 protons. Thus, its effective nuclear charge is 2.
Now we can see why magnesium is smaller than sodium. A valence electron on sodium is held close to the nucleus effectivelyby one proton. A valence electron on magnesium is held close to the nucleus effectively by two protons. Therefore, the stronger pull on the magnesium valence electrons causes the electrons to move closer to the nucleus and the atomic radius is lessthan that of sodium.
ShieldingThe model described above is simplified. There's one more factor that we have to account for. Let's go back to the sodium atom. The 10 inner electrons are going to "shield" the valence electron from the positive nucleus. So the pull that the one valence electron "feels" is going to be less than one due to the interference or shielding of the inner electrons. This means that the atomic radius is going to be a bit bigger than originally predicted. This also forms the basis for the increasing atomic radius going down a group.when we go from left to right in a periodic table one atom is added with an electron in the same increasing shell. if electron is added then a proton is also added to the nucleus of that atom this results in the increasing of nuclear energyin the nucleus thus the attraction between the nucleus and the outermost electron increases thus the size of the atom decreases while going from left to right in a period of the periodic table.
Atomic radius decreases from left to right in periodic table. This is due to increase in nuclear charge.Across a period, more number of elements enter into same shell.The effective nuclear charge attracts the electrons and hence its size decreases.
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Across a period (from left to right) the effective nuclear charge increases and hence the size of an atom decreases.
The atomic radius decrease, with several exceptions in periods 6 and 5.
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
Down a group, the atomic radius increases as the number of shells or energy levels increases.
As a general rule, when moving left to right on the periodic table the atomic radius decreases due to increasing electromagnetic attraction of the nucleus to the electrons.
The atomic radius decrease, with several exceptions in periods 6 and 5.
The atomic radius decrease from left to right in the periodic table.
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
The atomic radius decreases as you go from left to right. or atomic radius cation radius && anion radius -barbie=]
from left to right the atomic radius decreases as the electrons that get added are added in the same shell as they are in the same period. the shielding effect remains constant but the proton number increases which inturn increases the effective nuclear pull on the electrons bringing the electrons closer to the nuclei hence decreasing the radius of the atom
the atomic radius decreses from left to right in periodic table due to increase in the number of succesive element the electrons of the outermost shell are more attracted towards nucleus and the atomic radius or atomic size decreases.
B. are located on the right on the Periodic TableC. have a small atomic radius
Generally is a decrease of atomic radius along a period, from left to right.
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
Down a group, the atomic radius increases as the number of shells or energy levels increases.
As a general rule, when moving left to right on the periodic table the atomic radius decreases due to increasing electromagnetic attraction of the nucleus to the electrons.