when you go down a group you get more shells and in those shell are electrons the further away the electrons are from the protons and neutrons the less energy you need to pull of the electrons.
The ionisation energy decreases down the group. The atomic radius increases down the group. So the ability to loose electron increases.
The ionization energy increases going across a periodic table.This is because of increasing nuclear charge.
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
It decreases when going down a group.
It decreases when going down a group.
As you go from right to left in a period in the periodic table the ionization energy increases. While going from top to bottom in a group in the periodic table the ionization energy decreases .
The ionization energy increases going across a periodic table.This is because of increasing nuclear charge.
In a group the first ionization energy decrease going down.In a period the first ionization energy increase from left to right.
from left to right in a row on the periodic table the ionization energy increases. going down a column the ionization energy decreases.
The correct answer is: The ionization energy increases because there are more protons to pull on the electrons.
Electronegativity and first ionization energy both increase going up the Periodic Table.
Electronegativity and first ionization energy both increase going up the Periodic Table.
It decreases when going down a group.
The first ionization energy decreases because the outermost electron is farther from the nucleus. Apex
The correct answer is: The ionization energy increases because there are more protons to pull on the electrons.
The ionisation energy increases across a period. Across a period, nuclear charge increases. The tendency to loose electron decreases.
It decreases when going down a group.
It decreases when going down a group.