Considering the elements B, C, N, F, and Si, the correct order of their non-metallic character is:
- B > C > Si > N > F
- Si > C > B > N > F
- F > N > C > B > Si
- F > N > C > Si > B
The Correct Option is D
Solution and Explanation
The non-metallic character of elements increases from left to right across a period.
Thus, the decreasing order of non-metallic character is \(F > N > C > B\).
Again, the non-metallic character of elements decreases down a group.
Thus, the decreasing order of non-metallic characters of \(C\) and \(Si\) are \(C > Si\).
However, \(Si\) is less non-metallic than \(B\) i.e., \(B > Si\).
Hence, the correct order of their non-metallic characters is :
\(F > N > C > B > Si\).
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Concepts Used:
Trends in Periodic Table
The following trend in periodic properties of elements is observed:
Atomic size Trends:
The distance between the centre of the nucleus and the outermost shell of an atom is known as the atomic radius. In a group the atomic size increases due to the addition of shells as we move from one period to another. Across a period the atomic size decreases as the number of shells remain the same while the nuclear charge increases.
Metallic character Trends:
The elements which lose electrons to form cations are known as metals. Metallic character increases as we move down the group because the atomic size increases which lead to easy loss of electrons. On the other hand, it decreases across a period as we move from left to right.
Non-metallic character Trends:
The elements which have a tendency to gain electrons are known as non-metals. The tendency to gain electrons increases on moving across a period due to an increase in the nuclear charge and decrease in the atomic size. Hence, non-metallic character increases across a period.
Ionization potential Trends:
Ionization potential is defined as the amount of energy required to remove an electron from the outermost shell of a gaseous atom and convert it into a positively charged gaseous ion. The periodic properties in terms of ionization potential increase because the atomic size decreases across a period due to increase in the nuclear charge.
Melting Point Trends:
The melting point of an element is basically the energy required to change the state of an element from its solid state to its liquid state. Which essentially implies breaking a few bonds. Thus, higher the stronger the bond between the atoms, higher will be the melting point.
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