The element with a very high ionization enthalpy but zero electron gain enthalpy is ....

In which of the following arrangements is the order $NOT$ according to the property indicated against it?

Select the correct statements from the following:
$(a)$ Effective nuclear charge for nitrogen is $3.90$
$(b)$ $IP$ of $Ne$ is more than $Na^{+}$
$(c)$ Order of electronegativity $sp > sp^2 > sp^3$
$(d)$ Order of acidic character $NH_3 < PH_3 < AsH_3$

The electronic configurations of four elements are $:-$
$(I) \ [Xe] 6s^1$
$(II) \ [Xe] 4f^{14} 5d^1 6s^2$
$(III) \ [Ar] 4s^2 4p^5$
$(IV) \ [Ar] 3d^7 4s^2$
Select the incorrect statement about these elements $:-$

Point out the wrong statement: In a given period of the periodic table,the $s$-block element has,in general,a lower value of

To which group and period does the element belong if the electronic configuration of an element in its $-2$ oxidation state is $1s^2 2s^2 2p^6 3s^2 3p^6$?