In which one of the following pairs the radius of the second species is greater than that of the first?
O2– and N3– both are isoelectronic but differ in the charge possessed by them. As the negative charge increases, the electrons are held less and less tightly by the nucleus, therefore, radius increases form O2– to N3–.
The correct order of ionisation energy of C, N, O, F is
The electron affinity values (in kg mol–1) of three halogens X, Y and Z are respectively –349, –333 and –325. Then X, Y and Z respectively, are
Which of the following has the highest second ionisation energy?
The electronic configuration of the element with maximum electron affinity is
The first ionisation energy of oxygen is less than that of nitrogen. Which of the following is the correct reason for this observation?
The charge/size ratio of a cation determines its polarizing power. Which one of the following sequences represents the increasing order of the polarizing power of the cationic species, K+, Ca2+, Mg2+, Be2+?
Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of the given atomic species?
Which is likely to show inert pair effect?
The correct order of the size of iodine species is
The increasing order of the first ionisation enthalpies of elements B, P, S and F (lowest first) is