Ionization energy decrease down the group.So in halogens,Fluorine has highest 1st ionization energy.
Argon. As you go across (left to right) on the periodic table the energy of an atom increases. Argon is farthest left of chlorine therefore making Argon have a higher ionization energy level.
Potassium has a higher ionization energy than cesium.
The second ionization energy of sodium is so much greater than the first because the first electron is removed from the valence shell, while the second electron is removed from the core orbitals. Additionally, the sodium atom has a positive charge after the first ionization, which thus attracts the remaining electrons more strongly. Both of these factors lead to a much higher second ionization energy compared to the first.
Bromine has because the ionization energy increases as you move across and decreases as you move down.
Ionization energy represents the energy required to remove electrons from an atom. The first and second ionization energies are relatively small because the lectrons must be removed from the 2s orbital. For the third ionization energy the electron must be removed from the 1s orbital which has less energy than the 2s, and so requires much more energy to be removed.
Chlorine has a higher ionization energy. Chlorine's tendency is to gain electrons, not lose them as metals usually do.
Argon. As you go across (left to right) on the periodic table the energy of an atom increases. Argon is farthest left of chlorine therefore making Argon have a higher ionization energy level.
Potassium has a higher ionization energy than cesium.
Krypton has a higher value.
Halogens, specially fluorine
Antimony. The higher an element is in a group, the smaller it is, requiring more energy (ionization energy) to remove an electron.
ionization energies of mg is less than chlorine because chlorine requires only one electron to complete its octet so it will not prefer to loose its electron morover its electronegativity is also higher and it is of smaller size than mg so electtron removal is difficult
The relationship between atomic numbers and first ionization energies is that within the same period, as atomic number increases so does first ionization because as nuclear charge increases and atomic radius decreases, electrons become harder to remove. However, within the same group, the first ionization energy decreases as atomic number increases because of the added energy level, the electrons are farther from the nucleus and easier to remove.
The second ionization energy of sodium is so much greater than the first because the first electron is removed from the valence shell, while the second electron is removed from the core orbitals. Additionally, the sodium atom has a positive charge after the first ionization, which thus attracts the remaining electrons more strongly. Both of these factors lead to a much higher second ionization energy compared to the first.
Core electrons. Probably the 1s level would require the most ionization energy to pull these electrons.
The energy required to remove electron from atom are called ionization energy. Larger atom or molecule have lower ionization energy and molecule have higher ionization energy.
In general, ionization INCREASES as you move to the right and up in the periodic table, making P (Phosphorus) higher than Ca (Calcium).