As you go along the groups, you add one proton and one electron.
The more protons you add, the higher the positive charge in the nucleus gets.
Similarly, the more electrons you add, the more negative the shell of electrons gets.
With rising opposing charges in the nucleus and in the electrons, the electrons become more and more attracted to the nucleus, making the atom get smaller and more "tightly packed" in a way. Since the electrons are more attracted to the nucleus, it gets harder and harder to pull one of them away. So 1st ionization energy would increase as you go down a group.
The ionization energy decrease down in a group and increase from left to right in a period.
In a group the first ionization energy decrease going down.In a period the first ionization energy increase from left to right.
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
Ionization energy generally increases across a period as a result of a higher nuclear charge, however there are some exceptions such as Boron which has a lower ionization energy than Beryllium (because it is in a P orbital), and Oxygen which has a lower ionization energy than nitrogen (Because ionization decreases the electron electron repulsion in its orbitals).
ionization energy
When moving left to right across the PT the ionization energy increases. As you go down, the ionization energy, decreases.
In a group the first ionization energy decrease going down.In a period the first ionization energy increase from left to right.
The ionization energy increases going across a periodic table.This is because of increasing nuclear charge.
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
ionization energy
Ionization energy generally increases across a period as a result of a higher nuclear charge, however there are some exceptions such as Boron which has a lower ionization energy than Beryllium (because it is in a P orbital), and Oxygen which has a lower ionization energy than nitrogen (Because ionization decreases the electron electron repulsion in its orbitals).
When moving left to right across the PT the ionization energy increases. As you go down, the ionization energy, decreases.
Ionization energy increases as we go across a period. Its value decreases as we go down a group.
The correct answer is: The ionization energy increases because there are more protons to pull on the electrons.
Across a period, first ionization energy increases. However, when going down a group, first ionization energy generally decreases. As you go down a group, atoms hove more total electrons so they don't really care that much about their outermost ones.
The correct answer is: The ionization energy increases because there are more protons to pull on the electrons.
First ionization energy increase
Atomic number, ionization energy and electronegativity