JEE Questions for Chemistry Classification Of Elements And Periodicity In Properties Quiz 5 - MCQExams.com

A^‒ > A > A⁺

Ce-58 is an f-block element (lanthanide).

7 Horizontal and 18 vertical series.

Fr being the most metallic element has the highest tendency to lose electrons.

Actinide series

IE₁ of N is higher than that of O.

Atomic radius of neon being van der Waals’ radius is higher than that of fluorine which is in fact is covalent radius

Li is the lightest metal in the periodic table

It does not help to predict the stable valency states of the elements

IE₁ of Mg is higher than that of Na because of increased nuclear charge and also that of Al because in Mg a 3s-electron has to be removed while in Al it is the 3 p-electron. The IE₁ of Si is, however, higher than those of Mg and Al because of increased nuclear charge, Thus, the overall order is Na < Mg > Al < Si.

ns² np⁵

Polarity of the bonds

Elements (a), (b) and (d) belong to the same group since each one of them has two electrons in the shell. In contrast, element(c) has seven electrons in the valence shell and hence does not lie in the same group in which elements (a) (b) and (d) lie

Transition elements.

Metallic character decreases in a period and increases in a group.

Atomic size decreases along a period, but noble gases have much larger size than other elements of the same period.

Amongst isoelectronic ions, cations are smaller than anions.

Na⁺ and F^- ions are isoelectronic, therefore, F^- has the largest and Na⁺ has the lowest size. Further, Al with higher nuclear charge has lower size than Mg. Thus the overall order is : Na⁺ < Al < Mg < F^-

IE of element with electronic configuration (d) is lowest because of its biggest size. Among the remaining three elements of the same period (3^rd), IE of element with electronic configuration (b) is the highest due to greater stability of the exactly half- filled 3 p- subshell

Amongst O, S and Se the EA of O is the smallest due to inter-electronic repulsions present in its relatively compact 2p-subshell.EA of Se is,however, smaller than S due to its greater size.Thus, the overall sequence is S > Se > O.

Germanium is a metalloid

Bigger the size of the atom smaller will be its IE.

Within a group. IE decreases from top to bottom.

The element with Z = 43 lies in the 5th period. Therefore, the atomic number of the element which lies just above it in the 4th period should be 43 – 18 = 25. As such, its electronic configuration is (a).

For transition elements,d-sub shells are not filled with electrons monotonically (one at a time ) because of extra stability of d⁵ and d¹⁰ configurations. Besides these, there are many other exceptions, e.g. Nb, Mo, Ru, Rh, Pd etc.

IE₃ > IE₂ > IE₁.

Na^‒ > Na > Na⁺

Amongst isoelectronic ions, the size of the cation decreases as the magnitude of the charge increases

IE₂ of K is much higher than those of Ca and Ba because in case of K, the second electron has to be removed from noble gas (argon) core while this is not so in case of Ca and Ba. Out of Ca and Ba the IE₂ of Ca is higher than that of Ba due to smaller size. The overall sequence is K > Ca > Ba.