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) + 3IF(g) → BF3(g) + NI3(g)
a. What is the enthalpy of formation for NI3(s) given the enthalpy of reaction (−307 kJ) and the enthalpies of formation for BN(s) (−254 kJ/mol), IF(g) (−96 kJ/mol), and BF3(g) (−1136 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? What are the hybridizations of the central atoms in each species in the by-product?

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) + 3IF(g) → BF3(g) + NI3(g)
a. What is the enthalpy of formation for NI3(s) given the enthalpy of reaction (−307 kJ) and the enthalpies of formation for BN(s) (−254 kJ/mol), IF(g) (−96 kJ/mol), and BF3(g) (−1136 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? What are the hybridizations of the central atoms in each species in the by-product?

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