Consider the following compounds: (i) IF5 (ii) ClI4^- (iii) XeO2F2 (iv) NH2^- (v) BCl3 (vi) BeCl2 (vii) AsCl4^+ (viii) B(OH)3 (ix) NO2^- (x) ClO2^+.
Then, calculate value of "x + y - z", here x, y

Question

Consider the following compounds: (i) IF5 (ii) ClI4^- (iii) XeO2F2 (iv) NH2^- (v) BCl3 (vi) BeCl2 (vii) AsCl4^+ (viii) B(OH)3 (ix) NO2^- (x) ClO2^+.
Then, calculate value of "x + y - z", here x, y and z are total number of compounds in given compounds in which central atom used their all three p-orbitals, only two p-orbitals and only one p-orbital in hybridisation respectively :

Prashant Kotian · Accepted Answer

Correct answer: 8

**SOLUTION:**
X (USING ALL THREE P-ORBITALS, SP3/SP3D/SP3D2): IF5, CLI4^-, XEO2F2, NH2^-, ASCL4^+ (TOTAL = 5)
Y (USING TWO P-ORBITALS, SP2): BCL3, B(OH)3, NO2^-, CLO2^+ (TOTAL = 4)
Z (USING ONE P-ORBITAL, SP): BECL2 (TOTAL = 1)
X + Y - Z = 5 + 4 - 1 = 8.. Step 1: The strength of a hydrogen bond (X-H...Y) is directly proportional to the electronegativity of the highly electronegative atoms (X and Y) involved, as a more electronegative atom creates a greater partial positive charge on the hydrogen and holds a stronger partial negative charge on the acceptor atom. Step 2: Comparing Fluorine, Oxygen, and Nitrogen, their electronegativities decrease in the order: F (4.0) > O (3.5) > N (3.0). Step 3: Consequently, the strength of the hydrogen bonds follows the decreasing order of H...F > H...O > H...N, which corresponds to option (a).

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