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.
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
1. Hydrogen (H2) and oxygen (O2) react to produce water (H2O). (a) Write down the equation for the above reaction. (b) The enthalpy change of reaction is –286 kJ mol-!. Is the reaction endothermic or exothermic? (c) What kinds of bonds are broken during the reaction? (d) What kinds of bonds are formed during the reaction? (e) Construct a diagram showing the change in enthalpy for the reaction.
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
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
14.
(ii) Construct and label a Born-Haber cycle for strontium difluoride, SrF2. Calculate the lattice energy of SrF2 using the following data: First electron affinity of fluoride =–328.0 kJ mol"1 First ionization energy of strontium = 549.0 kJ mol" Second ionization energy of strontium = 1064.0 kJ mol"! Enthalpy of atomization of fluoride = 75.3 kJ mol" Enthalpy of atomization of strontium = 164.0 kJ mol"! Enthalpy of formation of strontium difluoride = -1224.4 kJ mol"!
18.) Choose all the statements that are correct. (1) Like atomic size, electronegativity decreases going across a period and increases going down a group. (2) The second most electronegative element is chlorine. (3) Electronegativity is directly proportional to atomic number. (4) Like ionization energy, electronegativity increases going across a period and decreases going down a group. (5) Electronegativity is a measure of the ability of an atom to attract electrons and form a negative ion. (6) Electronegativity is a measure of the ability of an atom in a molecule to attract electrons go itself. (7) Electronegativity was first proposed by Linus Pauling. Group of answer choices (2) (1) (4) (3) (5) (7) (6)
Provide the Lewis structure and name of this molecules

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