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- Which of the four atoms Na, P, Cl, or K (a) has the largest atomic radius? (b) has the highest ionization energy? (c) is the most electronegative?17) The first three ionization energy of an element X are 590, 1145, and 4912 kJ•mol^-1. What is the most likely formula for the stable ion of X? What is the valence electron configu.ration for Group SA (lS) elements?Metallic character increases when going down a group. Give some examples illustrating how Bi and Sbhave metallic characteristics not associated with N, P,and As. Elemental nitrogen exists as N2 whereas in the gas phase the elements phosphorus, arsenic, and antimony consist of P4' As4, and Sb4 molecules, respectively.Give a possible reason for" this difference between N2 and the other Group SA (lS) elements. White phosphorus is much more reactive than black or red phosphorus. Explain.
- Explains the writing method that allows you to complete the configuration phosphorus electron (Z = 15). In your answer, highlight the following principles and concepts. The configuration written by layer and sublayer (1s 2, 2s 2, etc.) The use of quantum cells The Pauli principle of exclusion Hund's ruleA) Which of the halogen elements has the highest density in its standard state? B) Which of the elements of the third period should have the highest 2nd ionization energy? C) For which of Al, Si or P is the absolute value of the Electron Affinity greatest? D) Which of the ions Mg2+, Sr2+, Ca2+, Be2+, Ba2+, or Ra2+ is the smallest? E) For the elements: X = Br, I, Cl, or H, which has the the smallest average X-C bond energy?The first ionization energy of the oxygen molecule is the energyrequired for the following process:O2(g)---->O2 +(g) + e-The energy needed for this process is 1175 kJ/mol, very similarto the first ionization energy of Xe. Would you expect O2 to reactwith F2? If so, suggest a product or products of this reaction.
- Despite the expected decrease in atomic size, there is an un-expected drop in the first ionization energy between Groups2A(2) and 3A(13) in Periods 2 through 4. Explain this pattern interms of electron configurations and orbital energies.The Properties, Reactions and Applications of Oxygen Give its symbol, atomic structure, its electronic configuration, the elemental state of its two allotropes, (including a definition of the term allotrope). The discovery of dioxygen and the means of production with a balanced chemical equation. A comparison of the elemental state of oxygen to that of sulfur.In the series of group 5A hydrides, of general formulaMH3, the measured bond distances are P¬H, 1.419 Å;As¬H, 1.519 Å; Sb¬H, 1.707 Å. (a) Compare these valueswith those estimated by use of the atomic radii inFigure 7.7. (b) Explain the steady increase in M¬H bonddistance in this series in terms of the electron configurationsof the M atoms.