The electronegativity of the following elements increases in the order
Correct answer: C. Si, P, C, N
- A. C, N, Si, P
- B. N, Si, C, P
- C. Si, P, C, N
- D. P, Si, N, C
Explanation
Electronegativity is the tendency of an atom to attract a bonding pair of electrons. In the periodic table, electronegativity generally increases across a period (from left to right) and decreases down a group (from top to bottom). In this question, the elements are Si, P, C, and N. Silicon (Si) and phosphorus (P) are in the same period, but Si is to the left of P, so P is more electronegative. Carbon (C) and nitrogen (N) are also in the same period, with N being to the right of C and thus more electronegative. Comparing between groups, N and C are above Si and P, making them more electronegative overall. Hence, the correct order is Si, P, C, N. Other options are incorrect as they do not accurately reflect these trends in electronegativity.
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About Periodic Properties and Trends
Periodic properties arise from electron configuration and effective nuclear charge, producing trends in atomic and ionic radius, ionization energy, electron affinity, electronegativity, metallic character and reactivity. Comparisons run across periods and down groups, with attention to common exceptions. The topic also relates these trends to the behavior of s-block and p-block elements.
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