ionization energies (IE) have to do with things called ions. Ions are atoms which have gained or lost electrons. The ionization energy is the amount of energy it takes to detach one electron from a neutral atom. Some elements actually have several ionization energies. When this is the case, we refer to them as the "first ionization energy" or 'I', "second ionization energy" or 'I2', and so on. Notice that the energy variable follows Ii where i is the orbital from which the electron is lost. Ionization is endothermic meaning that the atom or molecule increases its internal energy (takes energy from an outside source).
Trend in Periodic Table
Ionization energy decreases down the GROUP because the size of the atom increases down the group and also the nuclear attraction become less due to the increase in size so the electrons that are present in the outermost shell become loosely bonded so the minimum amount of energy is required to remove an electron from the outermost shell.
Ionization energy (aka ionization potential), which is the amount of energy required to remove an electron from an atom (meaning to form a cation [positive charge]), increasesgoing across a period (row) and decreases going down a group or family (column).
Note: the above trends are for GROUP A Elements
Explanation: The reason it increases going across a period is because the number of outermost electrons increases going across the periods. The atomic radius (size of atom going from nucleus to outermost electron shell) decreases going across periods, meaning that as an electron is added to an element's outermost shell a proton is also added to the nucleus. This increases the attraction between the electrons and the protons in the nucleus, meaning there will be an increase in energy required to remove an electron. Plus, elements with more valence electrons are going to be more likely to attract electrons to gain a noble gas configuration (octet rule). (Think of the Group A numbers as representing the number of valence electrons a group number has). Thus, the energy required to remove those outermost electrons is going to increase.
The reason it decreases going down a family/group is because the atomic radius increases going down a family/group. This means that the distance between the outermost electrons and the atomic nucleus increases, meaning the attraction between those electrons and the radius is weaker. Thus, the energy required to remove those outermost electrons is going to decrease.
Atomic radius, or the size of an element going from the nucleus to the outermost shell, is going to decrease going across periods and will increase going down a group/family.
Explanation: The reason atomic radius decreasesgoing across periods is because as stated earlier in this answer, whenever an electron is added to an atom going across periods, a proton is also added. The attraction between the electrons in the outermost shell and the protons in the nucleus increases. Thus, the distance between the nucleus and the outermost electrons (atomic radius) decreases.
The reason atomic radius increases going down a group/family is because the number of valence electrons (and protons) increases as the atomic number increases. There will be new electron shells added going down a group/family because of this. Thus, the atomic radius increases going down a group/family.
Ionization energy decreases down a periodic table column as the atomic number increases, because as the atomic number increases, the valence electrons have more inner shells between the valence electrons and the atom's nucleus, thereby reducing the electrostatic attractive force between the nucleus and the valence electrons.
as atomic radius increases, ionisation energy decreases.
Atomic radius is inversely proportional to first ionization energy
As Atomic radius INCREASE, Ionization energy DECREASE
Ionization energy increases from left to right across a period, and decreases down a group.
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Ionization energy decreases with the rise of atomic number in a group of periodic table.
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As we move from left to right, the atomic number increases, the ionisation energy increases, the electronegativity increases, the electronaffinity increases.
Al has atomic number 13, and silicon has atomic number 14. The extra electron that silicon has is in a 3p orbital. In simple terms the extra charge on the silicon nucleus contracts the electron shell, this increases the energy to remove an electron and also decreases the atomic radius. Al, first ionization energy 577.5 kJ/mol, atomic radius 125pm Si, first ionization energy 786.3 kJ/mol, atomic radius 110pm
Group IIA metals (alkali earth) become more reactive with non-metals as you go higher in atomic numbers.
as atomic number increases, ionization energy also decreases
Atomic number, ionization energy and electronegativity
Ionization energy decreases with the rise of atomic number in a group of periodic table.
Down a group, the atomic number generally increases, size increases, ionization energy decreases, reactivity increases.
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.
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As we move from left to right, the atomic number increases, the ionisation energy increases, the electronegativity increases, the electronaffinity increases.
As one proceeds down the group 7A elements, the first ionization energy decreases. this means that the outermost electron is more readily removed as we go down a group.
Al has atomic number 13, and silicon has atomic number 14. The extra electron that silicon has is in a 3p orbital. In simple terms the extra charge on the silicon nucleus contracts the electron shell, this increases the energy to remove an electron and also decreases the atomic radius. Al, first ionization energy 577.5 kJ/mol, atomic radius 125pm Si, first ionization energy 786.3 kJ/mol, atomic radius 110pm
as atomic number is increase the size of the atom goes on increasing as more number of electron is added to the outer most orbit so the nuclear force exerted by the nucleus on electron is less so the affinity to loose electorn is more as the atomic number is increase that is the reason ionization energy decrease with increase in atomic number
Radon (as down a group, the atomic size increases and the ionization energy decreases)
Group IIA metals (alkali earth) become more reactive with non-metals as you go higher in atomic numbers.