The periodicity is related to the electronic configuration. That is, all chemical and phyical properties are a manifestation of the electronic configurfation of the elements.
The atomic and ionic radii generally decrease in a preiod from left or right. As a consequence , the ionisation enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words, the ionisation enthalpy of the extreme left element in a period is the least and the electron left element on the extreme right is the highest negative. This results into high chemical reactivity at two extgremes and the lowest in the centre. Similarly down the group, the increase in atomic and ionic radii result in gradual decrease (with excetption in some third period elements) in electron gain enthalpies in the case of main group elements .
These properties can be related with the
(i) reducing and oxidising behacviour of the elements
(ii) metallic and no-metallic charcter of element
(iii) acidic, basic , amphoteric and neutral character of the oxides of the elements.
Which of the following statement is incorrect?

Options

A. In general metallic character increases down the group and decreases across a period
B. In general reducing property decreases down the group and increases across a period
C. In general, the oxide formed by the element on extreme right to the periodic table is the most acidic
D. Chemical reactivity of non-metals in terms of oxidising power increases from nitrogen to fluorine across the period

Answer

B

Explanation

As ionisation energies decrease down the group the reducing character increases and as across the period , ionisation energies increases, so reducing character, decreases.