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Answer:
Hello, The atomic radius of an element increase when you move from the top to the bottom of a family.
Explanation:
As we move down the group atomic radii increased with increase of atomic number. The addition of electron in next level cause the atomic radii to increased. The hold of nucleus on valance shell become weaker because of shielding of electrons thus size of atom increased.
As the size of atom increases the ionization energy from top to bottom also decreases because it becomes easier to remove the electron because of less nuclear attraction and as more electrons are added the outer electrons becomes more shielded and away from nucleus.
while in case of period atomic radius decrease as we move from left to right because the electrons are added with in the same shell. When the electron are added, at the same time protons are also added in the nucleus. The positive charge is going to increase and this charge is greater in effect than the charge of electrons. This effect lead to the greater nuclear attraction. The electrons are pull towards the nucleus and valance shell get closer to the nucleus. As a result of this greater nuclear attraction atomic radius decreases. Hope That Helps!
The atomic radius increases as you move from the top to the bottom of a group because the number of occupied levels increases.
But first, you have to know that the atomic radius represents the distance between the nucleus and the outermost electron shell (that is, the valence shell).
By means of the atomic radius it is possible to determine the size of the atom.
On the other hand, the effective nuclear charge is the net nuclear charge that an electron experiences when it is in a polyelectronic atom (that is, it has more than one electron).
In other words, the effective charge is the electric charge that the nucleus of a hypothetical atom would have capable of attracting its only electron with the same force with which the nucleus of the real atom attracts that same electron in the presence of all other electrons.
With the above, it is possible to say that by increasing the atomic number of the elements of a group (column), the number of occupied levels increases, while the effective nuclear charge on the outermost electron is the same.
Thas is, going down in a group of the periodic table increases the effective nuclear charge, but the number of electrons added with respect to the previous element of the same group increases in a complete shell.
The effect of adding new electronic layers is predominant, so they are increasingly distanced from the atomic nucleus and the atomic radius is greater.
In summary, in groups, the atomic radius increases with the atomic number, that is, downwards.
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