Classification of Elements and Periodicity

Element "E" belongs to the period 4 and group 16 of the periodic table. The valence shell electron configuration of the element, which is just above "E" in the group is

Match List - I with List - II :

Choose the correct answer from the options given below :

Among the following, basic oxide is :

Given below are two statements. One is labelled as Assertion A and the other is labelled as Reason R.

Assertion A: The first ionization enthalpy for oxygen is lower than that of nitrogen.

Reason R: The four electrons in 2p orbitals of oxygen experience more electron-electron repulsion.

In the light of the above statements, choose the correct answer from the options given below.

The correct order of electron gain enthalpy (-ve value) is :

The IUPAC nomenclature of an element with electronic configuration [Rn] $5f^{14}6d^17s^2$ is :

The first ionization enthalpies of Be, B, N and O follow the order

The total number of acidic oxides from the following list is

NO, $\mathrm{N_2O}$, $\mathrm{B_2O_3}$, $\mathrm{N_2O_5}$, CO, $\mathrm{SO_3}$, $\mathrm{P_4O_{10}}$

Given two statements below :

Statement I : In $\mathrm{Cl_2}$ molecule the covalent radius is double of the atomic radius of chlorine.

Statement II : Radius of anionic species is always greater than their parent atomic radius.

Choose the most appropriate answer from options given below :

The metal that has very low melting point and its periodic position is closer to a metalloid is

The incorrect statement is

Outermost electronic configurations of four elements A, B, C, D are given below :

(A) $3s^2$
(B) $3s^23p^1$
(C) $3s^23p^3$
(D) $3s^23p^4$

The correct order of first ionization enthalpy for them is :

In which of the following pairs, electron gain enthalpies of constituent elements are nearly the same or identical ?

(A) Rb and Cs
(B) Na and K
(C) Ar and Kr
(D) I and At

Choose the correct answer from the options given below :

The correct decreasing order for metallic character is

The first ionization enthalpy of Na, Mg and Si, respectively, are : 496, 737 and 786 kJ mol$^{-1}$. The first ionization enthalpy (kJ mol$^{-1}$) of Al is :

For Periodic Table which of the following statements are TRUE

A. Shielding increases as we go down in the group.
B. Shielding increases sharply across the period.
C. Ionization enthalpy increases down the group.
D. Metallic character increases down the group.
E. Electronegativity decreases down the group.

Choose the correct answer from the following options :

Consider the elements Mg, Al, S, P and Si, the correct increasing order of their first ionization enthalpy is :

The 1st, 2nd, and the 3rd ionization enthalpies, $I_1$, $I_2$, and $I_3$, of four atoms with atomic numbers $n$, $n+1$, $n+2$, and $n+3$, where $n < 10$, are tabulated below. What is the value of $n$?

The option(s) with only amphoteric oxides is(are)

The group having isoelectronic species is :