give unit of ionization enthalpy value
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In physics and chemistry, ionization energy (American English spelling) or ionisation energy (British English spelling), denoted Ei, is the minimum amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated neutral gaseous atom or molecule. It is quantitatively expressed as
In physics and chemistry, ionization energy (American English spelling) or ionisation energy (British English spelling), denoted Ei, is the minimum amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated neutral gaseous atom or molecule. It is quantitatively expressed asX(g) + energy → X+(g) + e−
In physics and chemistry, ionization energy (American English spelling) or ionisation energy (British English spelling), denoted Ei, is the minimum amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated neutral gaseous atom or molecule. It is quantitatively expressed asX(g) + energy → X+(g) + e−where X is any atom or molecule capable of ionization, X+ is that atom or molecule with an electron removed, and e− is the removed electron.[1] This is generally an endothermic process. Generally, the closer the outermost electrons to the nucleus of the atom , the higher the atom's or element's ionization energy.
In physics and chemistry, ionization energy (American English spelling) or ionisation energy (British English spelling), denoted Ei, is the minimum amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated neutral gaseous atom or molecule. It is quantitatively expressed asX(g) + energy → X+(g) + e−where X is any atom or molecule capable of ionization, X+ is that atom or molecule with an electron removed, and e− is the removed electron.[1] This is generally an endothermic process. Generally, the closer the outermost electrons to the nucleus of the atom , the higher the atom's or element's ionization energy.The sciences of physics and chemistry use different measures of 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 enthalpy, expressed as kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol).[2]
In physics and chemistry, ionization energy (American English spelling) or ionisation energy (British English spelling), denoted Ei, is the minimum amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated neutral gaseous atom or molecule. It is quantitatively expressed asX(g) + energy → X+(g) + e−where X is any atom or molecule capable of ionization, X+ is that atom or molecule with an electron removed, and e− is the removed electron.[1] This is generally an endothermic process. Generally, the closer the outermost electrons to the nucleus of the atom , the higher the atom's or element's ionization energy.The sciences of physics and chemistry use different measures of 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 enthalpy, expressed as kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol).[2]Comparison of Ei of elements in the periodic table reveals two periodic trends: