Advertisements
Advertisements
Question
Explain the following, give an appropriate reason.
The electron affinity values of Be and Mg are almost zero and those of N (0.02 eV) and P (0.80 eV) are very low.
Advertisements
Solution
Be (Z = 4) 1s2 2s2
Mg (Z = 12) 1s2 2s2 2p6 3s2
Noble gases have the electronic configuration of ns2 np6. All these are completely filled and are more stable. For all these elements Be, Mg and noble gases, the addition of electrons is unfavorable and so they have zero electron affinity.
Nitrogen (Z = 7) 1s2 2s2 2px1 2py1 2pz1.
It has a half-filled electronic configuration. So the addition of electrons is unfavorable and it has a very low electron affinity value of 0.02 eV.
Phosphorus (Z = 15) 1s2 2s2 2p6 3s2 3px1 3py1 3pz1.
It also has a half-filled electronic configuration. Due to the symmetry and more stability, it has a very low electron affinity value of 0.80 eV.
APPEARS IN
RELATED QUESTIONS
Various successive ionisation enthalpies (in kJ mol-1) of an element are given below.
| IE1 | IE2 | IE3 | IE4 | IE5 |
| 577.5 | 1,810 | 2,750 | 11,580 | 14,820 |
The element is
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 electronic configuration of the atom having maximum difference in first and second ionisation energies is
Which of the following orders of ionic radii is correct?
The First ionisation potential of Na, Mg and Si are 496, 737 and 786 kJ mol-1 respectively. The ionisation potential of Al will be closer to
In what period and group will an element with Z = 118 will be present?
What is the screening effect?
State the trends in the variation of electronegativity in groups and periods.
