Home
Class 12
CHEMISTRY
The second ionisation energies are highe...

The second ionisation energies are higher than the first ionisation energies. This is mainly due to the fact the after the removal of the first electron, the atom changes into monovalent positive ion. In the ion, the number of electrons decreases but the nuclear charge remains the same. as a result of this, the remaining electrons are held more tightly by the nucleus and it becomes difficult to remove the second electron. therefore, the value of second ionisation energy. `(IE_(2))`, is greater than that of the first ionisatio energy `(IE_(1))`. similarly third ionisation energy `(IE_(3))` is greater than that of second `IE_(2)`.
Q. `IE_(1) and IE_(2)` of Mg metal are 178 and 348 kcal/mol respectively. the energy required for the given reaction is:
`Mg(s) to Mg^(+2)+2e^(-)`

A

`+170` kcal/mol

B

`+526` kcal/mol

C

`-170` kcal/mol

D

`-526` kcal/mol

Text Solution

AI Generated Solution

The correct Answer is:
To solve the problem of calculating the energy required for the reaction \( \text{Mg}(s) \rightarrow \text{Mg}^{2+} + 2e^{-} \), we will use the provided first and second ionization energies of magnesium. ### Step-by-Step Solution: 1. **Identify Ionization Energies**: - The first ionization energy (IE1) of magnesium is given as 178 kcal/mol. - The second ionization energy (IE2) of magnesium is given as 348 kcal/mol. 2. **Understanding the Reaction**: - The reaction involves the conversion of solid magnesium (Mg) to a magnesium ion with a +2 charge (\( \text{Mg}^{2+} \)) while releasing two electrons (\( 2e^{-} \)). - This process requires energy to remove the electrons from the magnesium atom. 3. **Calculate Total Energy Required**: - The total energy required for the reaction can be calculated by adding the first and second ionization energies: \[ \text{Total Energy} = \text{IE1} + \text{IE2} \] - Substituting the values: \[ \text{Total Energy} = 178 \, \text{kcal/mol} + 348 \, \text{kcal/mol} \] - Performing the addition: \[ \text{Total Energy} = 526 \, \text{kcal/mol} \] 4. **Conclusion**: - The energy required for the reaction \( \text{Mg}(s) \rightarrow \text{Mg}^{2+} + 2e^{-} \) is 526 kcal/mol. ### Final Answer: The energy required for the reaction is **526 kcal/mol**. ---
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • PERIODIC PROPERTIES

    VK JAISWAL ENGLISH|Exercise ONE OR MORE ANSWERS IN/ARE CORRECT|98 Videos
  • PERIODIC PROPERTIES

    VK JAISWAL ENGLISH|Exercise MATCHTHE COLUMN|11 Videos
  • PERIODIC PROPERTIES

    VK JAISWAL ENGLISH|Exercise MATCH THE COLUMN|11 Videos
  • p-BLOCK ELEMENTS

    VK JAISWAL ENGLISH|Exercise SUBJECTIVE PROBLEMS|35 Videos
  • QUALITATIVE INORGANIC ANALYSIS

    VK JAISWAL ENGLISH|Exercise SUBJECTIVE PROBLEMS|4 Videos

Similar Questions

Explore conceptually related problems

The second ionisation energies are higher than the first ionisation energies. This is mainly due to the fact the after the removal of the first electron, the atom changes into monovalent positive ion. In the ion, the number of electrons decreases but the nuclear charge remains the same. as a result of this, the remaining electrons are held more tightly by the nucleus and it becomes difficult to remove the second electron. therefore, the value of second ionisation energy. (IE_(2)) , is greater than that of the first ionisatio energy (IE_(1)) . similarly third ionisation energy (IE_(3)) is greater than that of second IE_(2) . Q. Correct order of ionisation potential of coinage metals is:

The second ionisation energies are higher than the first ionisation energies. This is mainly due to the fact the after the removal of the first electron, the atom changes into monovalent positive ion. In the ion, the number of electrons decreases but the nuclear charge remains the same. as a result of this, the remaining electrons are held more tightly by the nucleus and it becomes difficult to remove the second electron. therefore, the value of second ionisation energy. (IE_(2)) , is greater than that of the first ionisatio energy (IE_(1)) . similarly third ionisation energy (IE_(3)) is greater than that of second IE_(2) . Q. Successive ionisation energy of an atom is greater than previous one, because:

The second ionisation energies are higher than the first ionisation energies. This is mainly due to the fact that after the removal of the first electrons, the atom changes inot mono valent position ion. In the ion, the number of electrons decreases but the nuclear charge remains the same. As a result of this, the remaining electrons are held more tightly by the nucleus and it becomes difficult to remove the second electron . Therefore, the value of second ionisation energy . (IE_(2)) , is greater than that of the first ionisation energy (IE_(1)) . Similarly third ionisation energy (IE_(3)) is greater than that of second IE_(2) . Successive ionisation energy of an atom is greater than previous one, because

The first ionisation energy is maximum for

Why is the second ionisation energy of an element much greater than its first ionisation energy ?

The second ionisation enthalpies of elements are always higher than their first ionisation enthalpies because:

The ionisation energy will be higher when the electron is removed from:

The second ionisation enthalpy of an alkaline earth metal is higher than its first ionisation enthaply. Why is it so ?

The energy of the first electron in helium will be

Why are the second ionisation enthalpies of group 1 elements much higher than their first ionisation enthalpies ?