Atomic size decreases across a period
it decreases
Electronegativity increases across (left to right) the periodic table and decreases on going down.
Across a period the metallic character decreases
Electronegativity generally decreases as you go down a group on the periodic table due to the increasing distance between the nucleus and valence electrons, reducing the attractive force. Across a period, electronegativity generally increases due to the increasing nuclear charge, pulling valence electrons closer and increasing their attraction.
A good example of periodicity would be the size of an atom which decreases across the Periodic Table but increases down the column
The atomic radius generally decreases across a period of the periodic table from left to right due to increased nuclear charge pulling electrons closer to the nucleus. This results in a stronger attractive force, leading to a smaller atomic radius.
Electropositivity decreases along a period. The metallic character also decreases.
As you move across the periodic table from left to right (across a period), the atomic radius of the elements tends to decrease.
it increases then decreases
As you move from left to right across the periodic table, electronegativity increases, and as you move down the table electronegativity decreases.
As you move from left to right across the Periodic Table, electronegativity increases, and as you move down the table electronegativity decreases.
On the Periodic Table of elements, electronegativity increases as you move left to right across a period.