Question

How do you complete the following equation to illustrate the first ionization energy for one mole of magnesium atoms?
$Mg(g)+?Kcal\to Mg(g)+{{e}^{-}}$

Answer 1

Hint: Mole is generally represented by the symbol mol. It is generally described as the unit of measurement for the amount of substance in SI where SI stands for International System of units. It is defined on the basis of Avogadro’s number.

Complete answer:
Ionization energy can be described as the amount of energy needed to remove the most loosely bound electron i.e. electron present in the outermost electron from an isolated gaseous atom of an element in its lowest energy state or also known by ground state to produce a cation is known as ionization potential.
Ionization potential is an endothermic process which is generally expressed by the term I or I.P. and measured in electron volts. Energy removed to the first electron is called first ionization energy and to remove second electron it is termed as second ionization energy and so on in their respective manner.
Hence the first ionization energy for one mole of magnesium atoms should be equal to 1Kcal as we know that 1kcal is defined as the energy needed to remove an electron from 1 mole of the given substance and in the question 1 mol is given. Therefore the equation should be as follows:
$Mg(g)+1Kcal\to Mg(g)+{{e}^{-}}$

Note:
A mole of a substance or particle can also be defined as containing exactly $6.022\times {{10}^{23}}$particles which may be atoms, molecules or ions where $6.022\times {{10}^{23}}$ is known as the Avogadro’s number.