Explain the sequence of ionization enthalpy in frequency and in mass
Answers
Answer:
In physics and chemistry, ionization energy (American English spelling) or ionisation energy (British English spelling), is the minimum amount of energy required to remove the most loosely bound electron of an isolated neutral gaseous atom or molecule.[1] It is quantitatively expressed as
Periodic trends for ionization energy plotted against the atomic number. Within each of the seven periods the ionization energy is at a minimum for the first column of the periodic table (the alkali metals), and progresses to a maximum for the last column (the noble gases). The maximum ionization energy decreases from the first to the last row in a given column, due to the increasing distance of the outer electron shell from the nucleus as inner shells are added.
X(g) + energy ⟶ X+(g) + e−
where X is any atom or molecule, X+ is the ion with one electron removed, and e− is the removed electron.[2] This is generally an endothermic process. As a rule, the closer the outermost electrons to the nucleus of the atom, the higher the atom's ionization energy.
The sciences of physics and chemistry use different units for ionization energy. In physics, the unit is the amount of energy required to remove a single electron from a single atom or molecule, expressed as electronvolts. In chemistry, the unit is the amount of energy required for all of the atoms in a mole of substance to lose one electron each: molar ionization energy or approximately enthalpy, expressed as kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol).[3]
Explanation:
bhi may tumse eak baat kahne chataho bura mat manna kabi kabi to apna dimag laga liya karo hamese dosto ke bharose per rahate ho