The question asks about the order of non-metallic character of the elements B (Boron), C (Carbon), N (Nitrogen), F (Fluorine), and Si (Silicon). To determine the correct order, we must first understand the concept of non-metallic character in the context of the periodic table.
The non-metallic character of an element is defined by its ability to gain electrons and form anions. Non-metals are generally located on the right side of the periodic table. As you move across a period from left to right, the non-metallic character increases due to a decrease in atomic size and an increase in electronegativity. Within a group, the non-metallic character decreases as you move down because the additional electron shells make it more challenging to attract electrons.
Based on the above analysis, the order of non-metallic character from highest to lowest is:
Therefore, the correct option is:
F > N > C > Si > B
The non-metallic character is governed by electronegativity and position on the periodic table. As such, fluorine, being the most electronegative and furthest right on the period, has the highest non-metallic character, followed by nitrogen, carbon, silicon, and boron.
Given below are two statements:
Statement (I): According to the Law of Octaves, the elements were arranged in the increasing order of their atomic number.
Statement (II): Meyer observed a periodically repeated pattern upon plotting physical properties of certain elements against their respective atomic numbers.
In the light of the above statements, Choose the correct answer from the options given below:
The correct orders among the following are:
[A.] Atomic radius : \(B<Al<Ga<In<Tl\)
[B.] Electronegativity : \(Al<Ga<In<Tl<B\)
[C.] Density : \(Tl<In<Ga<Al<B\)
[D.] 1st Ionisation Energy :
In\(<Al<Ga<Tl<B\)
Choose the correct answer from the options given below :