Advertisements
Advertisements
प्रश्न
Why the first ionisation enthalpy of sodium is lower than that of magnesium while its second ionisation enthalpy is higher than that of magnesium?
Advertisements
उत्तर
The first ionization enthalpy of magnesium is higher than that of Na due to the higher nuclear charge and slightly smaller atomic radius of Mg than Na. After the loss of the first electron, Na+ formed has the electronic configuration of neon (2, 8). The higher stability of the completely filled noble gas configuration leads to a very high second ionization enthalpy for sodium. On the other hand, Mg+ formed after losing the first electron still has one more electron in its outermost (3s) orbital. As a result, the second ionization enthalpy of magnesium is much smaller than that of sodium.
APPEARS IN
संबंधित प्रश्न
Which of the following elements will have the highest electronegativity?
Identify the wrong statement.
Which of the following is the second most electronegative element?
Which of the following orders of ionic radii is correct?
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"
Explain the periodic trend of ionisation potential.
By using Pauling's method calculate the ionic radii of K+ and Cl− ions in the potassium chloride crystal. Given that `"d"_("K"^+) - "Cl"^-` = 3.14 Å
Explain the following, give an appropriate reason.
Ionisation potential of N is greater than that of O
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.
State the trends in the variation of electronegativity in groups and periods.
