Show work. Don't use Ai for answering this.... Molecular Structure and Physical PropertiesConsider the following statements and determine which are true and which are false.NO3 has three resonance Lewis structures.☑ Selenium tetrafluoride (SeF4) is a non-polar molecule.The formal oxidation state of an atom in a molecule (or molecular ion) can be calculated as:(the number of valence electrons on a free atom) minus (half the number of electrons in bonds to that atom) minus (the number of unshared electrons assigned to the atom in themolecule)☑ KrF 4 is a polar molecule.☑ Carbon tetrachloride (CCI4) is a polar molecule.Bond angles for IF6+ are 60 °.

1.)2.) SeF4 is a polar molecule due to the electronegativity of the fluorine and selenium.…

Answered: Molecular Structure and Physical…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 78QRT

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(e) The mean bond enthalpy for chlorine is +242 kJ mol·l and that for fluorine is +158 kJ mol-". The enthalpy of formation of CIF (g) is 56 kJ mol·l (ii) Calculate the enthalpy of formation of, gaseous Chlorine Trifluoride, CIF3 (g), using the bond enthalpy value you obtained in part (i). (iii) The bond enthalpy of CIF3 calculated in part (ii) is likely to be different than that determined from experiment. Explain.
Answer the following questions that relate to the chemistry of nitrogen. (a) Two nitrogen atoms combine to form a nitrogen molecule, as represented by the following equation. 2 N(g) ® N2(g) Using the table of average bond energies below, determine the enthalpy change, AH, for the reaction. Average Bond Energy (k) mol-1) Bond N-N 160 N=N 420 N°N 950 (b) The reaction between nitrogen and hydrogen to form ammonia is represented below. N2(g) + 3 H2(g)® 2 NH3(g) AH° = -92.2 kJ Predict the sign of the standard entropy change, AS', for the reaction. Justify your answer. (C) The value of AG° for the reaction represented in part (b) is negative at low temperatures but positive at high temperatures. Explain.
Calculate the lattice energy of AgBr(s) using the following thermodynamic data (all data is in kJ/mol). Ag(s) ΔHsublimation = 265 kJ/mol Ag(g) Ionization energy = 711 kJ/mol Br-Br(g) Bond energy = 173 kJ/mol Br(g) Electron affinity = -345 kJ/mol AgBr(s) ΔH°f = -120 kJ/mol ______________ kJ/mol
[chemical bonding] find: overall charge, formal charge, formal oxidation number on Nitrogen
Determine the enthalpy for the ammonia formation reaction from the following bond energy data: E (H-H) = 436kJ / mol, E (N-H) = 389kJ / mol, E (N triple bond N) = 946kJ / mol
Use the bond enthaplies in this table to determine triangleH for the formafion of hydrazine, N2H4, according to this equation.
(A) Balance this reaction. Then use the bond enthapies given in the table below to calculate the enthalpy of reaction for the balanced reaction. kJ/mol(B) Balance this reaction. Then use the bond enthapies given in the table below to calculate the enthalpy of reaction for the balanced reaction. kJ/mol(C) Balance this reaction. Then use the bond enthapies given in the table below to calculate the enthalpy of reaction for the balanced reaction kJ/mol
Thortveitite is a mineral that contains the silicate ion [Si2O7]6-. The structure of this ion is such that the each Si atom is bonded to three terminal oxygen atoms, and the seventh O atom forms a bridge between the two Si atoms:[O3Si-O-SiO3]6- Draw a Lewis dot structure of this ion. What is the formal charge on each Si atom?
From the Lewis diagram of SiF4, determine: A) The formal charge on the silicon atom. B) The formal oxidation number of the silicon atom. C) The overall charge of the molecular species.
Estimate the enthalpy of reaction( AH), using bond enthalpy values given below 2H2(g) + 02(g) 2H20(g) ( AHO) = ? > Bond energies are given: BE (H - H)= 436 kJ/mol. BE (O=0)= 496 kJ/mol. BE (O - H)= 463 kJ/mol. A. + 367.2 kJ/mol B. + 534.1 kJ/mol C. - 484.0 kJ/mol D. - 490.2 kJ/mol
Predict the standard enthalpy change for the reaction below using the standard molar enthalpy of formation data provided: 4 NH3 + 3 O2 -> 2 N2 + 6 H2O H2O, ΔHf = -285.8 kJ/mol NH3, ΔHf = -46.19 kJ/mol N2 and O2, ΔHf = 0 kJ/mol -239.6 kJ/mol -1530 kJ/mol -1900 kJ/mol -332.0 kJ/mol
Arrange the following elements in order of increasing electronegativity: gallium, germanium, calcium, arsenic

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