Question

Although nitrogen trifluoride (NF3) is a thermally stable compound, nitrogen triiodide (NI3) is known to be a highly explosive material. NI3 can be synthesized according to the equation BN(s) + 3 IF(g) → BF3(g) + NI3 (8) a. What is the enthalpy of formation for NI3 (s) given the enthalpy of reaction (-307 kJ) and the enthalpies of formation for BN(8) (-254 kJ/mol), IF(g) (-96 kJ/mol), and BF3(g) (-1136 kJ/mol)? kJ/mol b. It is reported that when the synthesis of NI3 is conducted using 4 moles of IF for every 1 mole of BN, one of the by-products isolated is (IF2]*[BF4] . What are the molecular geometries of the species in this by-product? The molecular geometry of IF2+ is The molecular geometry of BF4 is What are the hybridizations of the central atoms in each species in the by-product? The hybridization of IF2+ is The hybridization of BF4 is

Answer 1

Enthalpy of formation of reaction is given by AH, ° = (AH, °) products - (AH, rear tant -307 =((-1136)+(AH, O)))-((-254)+(3x-96)) on solving AH, 'N, = 287kJ/mol Hybridization of IF2+ = 2 bond pair (side atom F) + 2 lone pair (on lodine) hence hybridization is SP3 Hybridization of BF4 = 4 bond pair (side atom F) + O lone pair (on Boron) hence hybridization is SP3 Molecular Geometry of BF4 = Tetrahedral Molecular Geometry of IFz+ = Bent or angular

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