The Periodic Table is organized into atomic number (how many protons) and size of each element. The sizes of each elemental atom increase from left to right and top to bottom. Hydrogen (H) is the smallest atom, while Cesium (Cs) is the largest.
Generally, atomic size increases as you descend a group. For example, lithium in group 1A is very small because there are only three electrons to accommodate. Potassium is in group 1A but is two periods lower. It has 17 electrons to accommodate and they take up more space. Radii also increase as you move left within a row.
Size typically increases going down a group due to an increasing number of electron shells, where the inner shells reduce the attractive forces of the nucleus and repel the electrons in the outer shell
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Decrease because the number of protons increase
decreases because the charge increases which means the electrons are more tightly held
When going left to right in a given row of the periodic table the atomic radius increases. When moving top to bottom of a given column the atomic radius increases.
decrease
Atomic size generally increases as you go down a group
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
it decreases
Electronegativity, electron affinity, nonmetalic nature, acidic nature of oxides, valency with respect to oxygen ( from 1 to 7), number of electrons in the outer most shell ( 1 to 8) increases across a period from left to right
decreases
Atomic radius
across a period, the atomic size decreases as the effective nuclear charge increases.
Down a period the atomic radius increases as the number of shells (or energy levels) increases. Across a period the atomic radius decreases as the effective nuclear charge increases.
Atomic size decreases across a period as the effective nuclear charge increases. Atomic size increases down a group as the energy level (shells) increases.
idk if this is an answer but this is what i found in my book. atomic raduis increases down a group and decreases across a period
Atomic size decreases across a period
Atomic size generally increases as you go down a group
It decreases as you move from left to right because there is an increase in positive charge in the nucleus as you go from left-to-right. Each time you go over an element it has one more electron and proton added to the principal energy level, so the nucleus pull increases and it holds the valence electron in tighter.
atomic size decreases across a period
It decreases.
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
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