As you move down any group on the Periodic Table, atomic radius increases (due to extra energy levels of electrons, which expand the atom's volume.) Electrons that are farther away from the nucleus are easier to remove, due to gradually weaker Coulombic forces moving down the group. So, ionization energy decreases with each increment downward. This explains, for example, why cesium (Cs) is more reactive than sodium (Na).
Because down in the group the atomic radius is higher and the attraction between nucleus and electrons is lower.
Electronegativity decrease down in a group.
it increases
It's decrease because florine has the most activity.
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
Because the atomic radius increases down the group 1 and decreases down the group of halogen
Electronegativity decrease down in a group.
The ionization energy decrease moving down in a group.
it increases
It's decrease because florine has the most activity.
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
1. In a period is a trend of decrease from left to right but it is not absolute.2. In a group the atomic radius increase moving down.
The electronegativity increase in a period from left to right; in a group decrease by descending.
The bonds between the electrons
The boiling point decrease from lithium to caesium.
Because the atomic radius increases down the group 1 and decreases down the group of halogen
1. The ionization energy decrease down in the group.2. The cause is that the distance between the nucleus and the electron shell increase and the needed energy to extract an electron decrease.
because down the group the cation becomes gets larger so the hydration energy decreases. so the solubility decreases