In general, atomic radius decreases across a period and increases down a group. Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius.
Likewise, which of the following explain the trend in atomic radii size down a group? Periodic Trends of Atomic Radius An atom gets larger as the number of electronic shells increase; therefore the radius of atoms increases as you go down a certain group in the periodic table of elements. In general, the size of an atom will decrease as you move from left to the right of a certain period.
Regarding this, what is the trend in 1st ionization energy from top to bottom down a group?
Moving left to right across a period, atomic radius decreases, so electrons are more attracted to the (closer) nucleus. The general trend is for ionization energy to decrease moving from top to bottom down a periodic table group. Moving down a group, a valence shell is added.
What trend in atomic radius do you see as you go down a group on the periodic table?
Group Trend The atomic radius of atoms generally increases from top to bottom within a group. As the atomic number increases down a group, there is again an increase in the positive nuclear charge. However, there is also an increase in the number of occupied principle energy levels.