The trends from left to right in a period increase (nuclear charge), and moving down a group decreases (shielding).
On the Periodic Table of elements, electronegativity increases as you move left to right across a period.
atomic size decreases across a period
increase from left to right across a period.
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
increasing number of electrons
The trends from left to right in a period increase (nuclear charge), and moving down a group decreases (shielding).
On the Periodic Table of elements, electronegativity increases as you move left to right across a period.
The atomic radius decreases along the elements across a period. Along a group, there is an increment in the atomic radius of corresponding elements.
Electronegativity increases from left to right across a period from column 1 through column 17 but drops sharply from column 17 to column 18.
Atomic size generally increases as you go down a group
I really don't know?
what is the reason for ionization energy across a period
well, the periodic table is very useful because you have the atomic number, atomic mass, and even the trends across a period or down a group.
Across a period, the metallic character decreases.
Down the group electron affinity decreases Across a period electron affinity increases. However, it should be noted that chlorine is having higher electron affinity than flourine due to the small size of fluorine atom)
Yes, it is true, the properties of elements change in groups and periods.