Calculate the energy change in kilojoules per mole when lithium atoms lose an electron to bromine atoms to form isolated
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- Compare the electron affinity of fluorine to the ionization energy of sodium. Does the process of an electron being pulled from the sodium atom to the fluorine atom have a negative or a positive E? Why is NaF a stable compound? Does the overall formation of NaF have a negative or a positive E? How can this be?arrow_forwardSolid phosphorus pentabromide, PBr5, has been shown to have the ionic structure [PBr4] [Br]. Write the electron-dot formula of the PBr4+ cation.arrow_forwardThe lattice energy of an ionic solid such as NaCl is the enthalpy change H for the process in which the solid changes to ions. For example, NaCl(s)Na+(g)+Cl(g)H=786kJ/mol Assume that the ionization energy and electron a affinity are H values for the processes defined by those terms. The ionization energy of Na is 496 kJ/mol. Use this, the electron affinity from Table 8.4, and the lattice energy of NaCl to calculate H for the following process: Na(g)+Cl(g)NaCl(s)arrow_forward
- Calculate the lattice energy of potassium fluoride, KF, using the BornHaber cycle. Use thermodynamic data from Appendix C to obtain the enthalpy changes for each step. (Note: You will obtain a slightly different answer if you use values given in Chapter 8 for the ionization energy and electron affinity, which are energy values at 0 K rather than the enthalpy changes at 298 K.)arrow_forwardPotassium and hydrogen react to form the ionic compoundpotassium hydride. (a) Write a balanced equation for thisreaction. (b) Use data in Figures 7.10 and 7.12 to determinethe energy change in kJ/mol for the following two reactions:K(g) + H(g) ----> K+(g) + H-(g)K(g) + H(g) ------>K-(g) + H+(g)(c) Based on your calculated energy changes in (b), which ofthese reactions is energetically more favorable (or less unfavorable)?(d) Is your answer to (c) consistent with the descriptionof potassium hydride as containing hydride ions?arrow_forwardConsider an ionic compound, MXMX, composed of generic metal MM and generic, gaseous halogen XX. The enthalpy of formation of MXMX is Δ?∘f=−553ΔHf∘=−553 kJ/mol. The enthalpy of sublimation of MM is Δ?sub=105ΔHsub=105 kJ/mol. The ionization energy of MM is IE=483IE=483 kJ/mol. The electron affinity of XX is Δ?EA=−307ΔHEA=−307 kJ/mol. (Refer to the hint). The bond energy of X2X2 is BE=213BE=213 kJ/mol. Determine the lattice energy of MXMX. Δ?lattice=ΔHlattice= kJ/molarrow_forward
- Please, give simple words explenation. Additional examples very helpful. Please, write the answer clear or typed. Thank you Ionic radii Why is there an overall contraction in ionic radii? Why is radius of Ti^ 2+ less than theoretical value? Why is the radius of Cr^ 2+ larger than that of V^ 2+.arrow_forwardConsider an ionic compound, MXMX, composed of generic metal MM and generic, gaseous halogen XX. The enthalpy of formation of MXMX is Δ?∘f=−411ΔHf∘=−411 kJ/mol. The enthalpy of sublimation of MM is Δ?sub=101ΔHsub=101 kJ/mol. The ionization energy of MM is IE=461IE=461 kJ/mol. The electron affinity of XX is Δ?EA=−325ΔHEA=−325 kJ/mol. (Refer to the hint). The bond energy of X2X2 is BE=189BE=189 kJ/mol. Determine the lattice energy of MXMX.arrow_forwardIron can form two common ions: Fe2+ and Fe3+ a) Write the complete electron configuration for EACH ion. b) Use the configurations in question a) to identify and explain which ion is more stable.arrow_forward
- Using Coulomb's law to predict trends in lattice energy: E = kQ1Q2 / r ∝ QcatQan / IRcat + IRan Which of the following would you expect to have the largest lattice energy? LiCl NaF MgCl2 MgBr2 CaCl2arrow_forwardUsing their electron configurations, explain why Zn and Cd always form 2+ cationsarrow_forwardAre the valence electrons closer to the nucleus in Be or Mgarrow_forward
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