answer must be correct or i will give down vote Draw resonance Structures for thefollowing 2 ions. Use arrows toShow apparent movement ofelectrons.J+NX←

I have shown the arrows which depict the flow of electrons across the molecule and give rise to…

Answered: Draw resonance Structures for the…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter7: Covalent Bonding

Section: Chapter Questions

Problem 77QAP

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7.107 How do the Lewis symbols for C, Si, and Ge reflect the similarity in their electron configurations?
Consider the following information. • The lattice energy of CsCl is AH lattice = -657 kJ/mol. • The enthalpy of sublimation of Cs is AH sub = 76.5 kJ/mol. • The first ionization energy of Cs is IE₁ = 376 kJ/mol. • The electron affinity of Cl is AHEA = -349 kJ/mol. • The bond energy of Cl, is BE = 243 kJ/mol. Determine the enthalpy of formation, AH₁, for CsCl(s). AH₁ = G Search or type URL % 5 A MacBook Pro 6 & 7 * CO 8 9 O - O 0 kJ/mol A I P
Suppose there is an element X which occurs naturally as X2(g).X2(g) + 2O2(g) → X2O4(g)ΔHof of O(g) is 249 kJ/molΔHof of X(g) is 458.5 kJ/molΔHof of X2O4(g) is 31 kJ/molThe X-X single bond energy is 116 kJ/molUse the above data to estimate the average bond energy in X2O4. Give your answer to the nearest 1 kJ/mol.
What is the lattice energy of RbBr? Use the given information below.Heat of formation for RbBr = -389.20 kJ/molHeat of sublimation for Rb = 82.00 kJ/molIonization Energy for Rb = 409.00 kJ/molBond dissociation energy for Br2 = 190.00 kJ/molElectron affinity of Br = -325.00 kJ/molHeat of vaporization for Br2 = 30.90 kJ/mol
The following Lewis diagram represents the valence electron configuration of a main-group element. •X• (Express your answer as a chemical symbol.) The element in period 5 that has this valence electron congfiguration is
Using the following data, calculate the lattice energy of calcium chloride: Ca2+(g) + 2Cl– (g) → CaCl2(s) ΔHlattice = ? Sublimation enthalpy of calcium ΔH = 177.8 kJ/mol First ionization energy of calcium ΔH = 590.2 kJ/mol Second ionization energy of calcium ΔH = 1144.2 kJ/mol First electron affinity of chlorine ΔH = –349 kJ/mol Heat of formation of CaCl2(s) ΔH = –795.4 kJ/mol Bond energy of Cl2 (see Table 2) Use Hess’s law to calculate the lattice energy of calcium chloride. set-up must show all the chemical equations and you must show how their H values add up to give your answer.
Consider the following information. • The lattice energy of KCl is AHjattice = -701 kJ/mol. • The enthalpy of sublimation of K is AH sub = 89.0 kJ/mol. • The first ionization energy of K is IE1 = 419 kJ/mol. • The electron affinity of Cl is AHEA = -349 kJ/mol. • The bond energy of Cl, is BE = 243 kJ/mol. Determine the enthalpy of formation, AHf, for KCl(s). ΔΗ- kJ/mol
Use the following data to estimate Δ Hf° for barium chloride. Ba (s) + Cl2 (g) ⟶ BaCl2 (s) Lattice energy = -2056 kJ/mol First ionization energy of Ba = 503 kJ/mol Second ionization energy of Ba = 965 kJ/mol Electron affinity of Cl = -349 kJ/mol Bond energy of Cl2 = 239 kJ/mol Enthalpy of sublimation of Ba = 178 kJ/mol
Using the following data, estimate the overall enthalpy of formation (in kJ/mol) for potassium chloride: K(s) + ½ Cl₂(g) → KCI(s). Process Lattice energy of KCI lonization energy of K Electron affinity of Cl Bond dissociation energy of Cl, Enthalpy of sublimation for K Question 21 of 28 Change in Energy (AHO) -690 kJ/mol 419 kJ/mol -349 kJ/mol 239 kJ/mol 90 kJ/mol
What is the lattice energy of NaCl? Use the given information below.Heat of formation for NaCl = -411.1 kJ/molHeat of sublimation for Na = 107.3 kJ/molIonization energy for Na = 496.0 kJ/molBond dissociation energy for Cl 2 = 240 kJ/molElectron affinity of Cl = -349.0 kJ/mol
Group the following ions into one of two groups based on the ion size compared to itsrespective neutral parent atom: (1) larger ionic radiusthan neutral atom OR (2)smaller ionic radiusthan neutral atom. Ions - Li, Be, N, O, F, Na, Mg, Al, P, S, Cl, K, Ca Explain BOTH of the two groupings based on the principles of attractive/repulsive forces between theelectron(s) and proton(s) and how those forces affect the distance between the nucleus and atom’s vsion’s valence electrons.
Given the following information: Heat of sublimation of Li(s) = 166 kJ/mol Bond energy of HF = 565 kJ/mol Ionization energy of Li(g) = 520. kJ/mol Electron affinity of F(g) = –328 kJ/mol Lattice energy of LiF(s) = –1030 kJ/mol Bond energy of H2 = 432 kJ/mol Calculate the net change in energy for the following reaction: 2Li(s)+2HF(g)-> 2LiF(s) +H2(g) Change in energy = kJ

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Draw resonance Structures for the following 2 ions. Use arrows to Show apparent movement of electrons. J + NX ←