The melting temperature properties generally change as you go from left to right in the Periodic Table by going down/decreasing.
Along a period, nuclear charge increases. hence, atomic radius decreases.
Along a period, nuclear charge increases. hence, atomic radius decreases.
For periodic trends we will examine1- Electronic configuration 2- Ionization energy 3- Atomic radius
The nonmetallic properties and the atomic radius generally decrease when the elements in period 3 are considered ordered. The order used is from left to right.
All of the elements in any one period of the Periodic Table have the same number of valence electrons.
Down a group, the atomic radius increases as the number of shells or energy levels increases.
Atomic radius generally decreases as you go from left to right in the same period. Atomic radius increases as you go down the same group.
The larger the highest energy level, the larger the atomic radius.
It tends to increaseThe atomic radius increases down the group
atomic radius decreases from bottom to top of the periodic table.
Atomic Mass
Ionic radius (or radii) increases as you move down a group and across a period.