Advertisements
Advertisements
Question
IE1 and IE2 of Mg are 179 and 348 kcal mol−1 respectively. The energy required for the reaction \[\ce{Mg -> Mg^2+ + 2e^-}\] is
Options
+ 169 kcal mol−1
− 169 kcal mol−1
+ 527 kcal mol−1
− 527 kcal mol−1
Advertisements
Solution
+ 527 kcal mol−1
APPEARS IN
RELATED QUESTIONS
Identify the wrong statement.
Which one of the following arrangements represent the correct order of least negative to most negative electron gain enthalpy
Which one of the following is the least electronegative element?
The element with positive electron gain enthalpy is
Is the definition given below for ionisation enthalpy is correct?
"Ionisation enthalpy is defined as the energy required to remove the most loosely bound electron from the valence shell of an atom"
How would you explain the fact that the second ionisation potential is always higher than the first ionisation potential?
Why the first ionisation enthalpy of sodium is lower than that of magnesium while its second ionisation enthalpy is higher than that of magnesium?
Explain the following, give an appropriate reason.
The formation of \[\ce{F^-_{(g)}}\] from \[\ce{F_{(g)}}\] is exothermic while that of \[\ce{O^2-_{(g)}}\] from \[\ce{O_{(g)}}\] is endothermic.
What is the screening effect?
Briefly give the basis for Pauling's scale of electronegativity.
