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Inorganic Chemistry
- Look in Appendix D and compare the electron configurations shown there with the fusion enthalpies for the metals shown in Table 9.7. Is there any correlation between these configurations and this property? Does strength of attraction among metal atoms correlate with number of valence electrons? Explain your answers.arrow_forwardConsider a hypothetical ionic compound AB (comprised of A* and B ions). Given the following enthalpy data and using a Born-Haber cycle calculation, predict AHiattice in kJ mol. AG) + Bs) - AB 4H = -384 kJ mol As) → Ag) ArH = 105 kJ mol B(s) - Bg) A,H = 101 kJ mol1 First ionization energy of Ag) = 501 kJ mol" Answes=? Electron affinity enthalpy of Bro (exothermic) = -348 kJ molarrow_forwardCalculate the fraction of atom sites that are vacant for lead (Pb, Z = 82) at its melting temperature (327 degrees C). Assume that the energy for vacancy formation is 0.55 eV/atom. Calculate the fraction of vacant sites at room temperature (25 degrees C). What is the ratio of these two values?arrow_forward
- Explain how periodic trends in ionization energy and electron affinity explain why atoms of elements in Group I andGroup II tend to bond with other elements by forming positive ions in ionic compounds. Explain with electronconfiguration of elements belonging to Group I and Group II.arrow_forward69°F Mostly cloudy esc Two sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next least energy, and so on. ionization ClCl + e Rb Rb + e Ca - Ca + e Explanation energy required ? ? ? Check ionization S→S +e Bi Bi + e Fr Fre X Search 118 ? energy required ? ? S v v v Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 2 B oloarrow_forwardPhotoelectron spectroscopy applies the principle of the photoelectric effect to study orbital energies of atoms and mol ecules. High-energy radiation (usually UV or x-ray) is absorbed by a sample and an electron is ejected. The orbital energy can be calculated from the known energy of the radiation and the mea sured energy of the electron lost. The following energy differences were determined for several electron transitions: ∆E2→1 = 4.098x10-17 J ∆E3→£1 = 4.854x10-17 J ∆E5→1 = 5.242x10-17 J ∆E4→2 = 1.024x10-17 J Calculate ∆E and l of a photon emitted in the following transitions: (a) level 3 → 2; (b) level 4 → 1; (c) level 5→4.arrow_forward
- Explain why Xe, and to a limited extent Kr, form com-pounds, where as He, Ne, and Ar do not.arrow_forwardSpecify the full electron configuration, noble gas notation electron configuration, orbital diagram (boxes and arrows) and specify whether it is diamagnetic or paramagnetic for C6H6N2Sarrow_forwardElectron arrangements with 8 electrons in the outermost shell tend to be more stable than other arrangements. How many electrons would need to be removed from a calcium atom to leave an electron arrangement with 8 electrons in the outermost shell?arrow_forward
- Consider selenium oxychloride (SeOCl2):How many regions of electron density surround the central atom?arrow_forwardGiven: Enthalpy of atomisation of calcium =+ 178 kJ First ionisation energy of calcium =+590 kJ Second ionisation energy of calcium = +1145 kJ Enthalpy of atomisation of chlorine =+ 121 kJ Electron affinity of chlorine Lattice energy of calcium chloride =- 2258 kJ = - 346 kJ Construct a Born-Haber cycle for calcium chloride, CaCl2 by using the data given above. Hence, calculate the enthalpy of formation of calcium chloride. b. The enthalpy of solution for calcium chloride crystal is -81.3 kJ mol'. Based on the data from the above Born-Haber cycle, calculate the enthalpy change for the reaction below: Ca" (g) + 2CI (g)–→ Ca* (aq) + 2CI¯ (aq)arrow_forwardgive handwritten answer-In 1889, James Dewar demonstrated that hydrogen reaches the solid state if cooled to a temperature below 14.01 K (-259.14 C). What happens to the energy levels of hydrogen in the solid state? Please explain thoroughly.arrow_forward
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