Ionization energy increases as we go across a period. Its value decreases as we go down a group.
Helium (He) has the highest ionization energy.
Ionization energy decreases with the rise of atomic number in a group of periodic table.
The ionization energy increases going across a periodic table.This is because of increasing nuclear charge.
group 1
It decreases when going down a group.
The ionization energy is the energy needed to extract an electron from an atom.The value of the ionization energy increase from left to right in a period of the periodic table and decrease in a group from the above to down.
the nobles gases are the greatest ionization group
Helium (He) has the highest ionization energy.
Ionization energy increases to the right and up on the periodic table. Ionization energy is the energy required to remove an electron. It can be conceptualized as the opposite of electron affinity, though this is not precisely true.
Across a row on the periodic table ionization energy increases. Down a column, ionization energy decreases. --------------------------------------------------------- The first Ionization energy of Boron is 800.6 kJ mol-1
the bottom of the Periodic Table. why? a metal looses electrons and at the bottom of the periodic table is the lowest amount of ionization energy (the energy needed to remove electrons) with low ionization energy, not much energy is needed to remove those electrons making it faster and easier to do so.
from left to right in a row on the periodic table the ionization energy increases. going down a column the ionization energy decreases.
ionization energy
The elements in the lower right part of the Periodic Table. Cs, Fr, Ra, Ba etc.
Ionization energy decreases with the rise of atomic number in a group of periodic table.
Electronegativity and first ionization energy both increase as you move up the periodic table
The correct answer is: The ionization energy increases because there are more protons to pull on the electrons.