Look at the following electron configurations. Which of the atoms will have similarchemical properties?1. 1s 2322p42. 1s22:22p33. 1s 25 2p°3s 3p^4s?310 4p42 and 31 and 21 and 3all of them

The chemical properties of an element is mainly determined by the electrons present in their…

Answered: Look at the following electron…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter8: The Periodic Table: Structure And Trends

Section: Chapter Questions

Problem 8.100QE

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The standard formation enthalpy of KCl is -571 kJmol-1. Plot the Born-Haber cycle and calculate the electron affinity of chlorine with the help of the data below. ΔH ° a (K) = 89 kJmol-1 BE (Cl-Cl) = 244 kJmol-1 IE (K) = 425 kJmol-1 ΔHL (KCl) = 719 kJmol-1
The standard formation enthalpy of KCl is -571 kJmol-1. Plot the Born-Haber cycle and calculate the electron affinity of chlorine with the help of the data below. ΔH°a(K) = 89 kJmol-1 BE(Cl-Cl) = 244 kJmol-1 IE(K) = 425 kJmol-1ΔHL(KCl) = 719 kJmol-1
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.
Given: 2H+(aq) + 2e– → H2(g); 0.00 VRb+(aq) + e– → Rb(s); –2.98 VF2(g) + 2e– → 2F–(aq); 2.87 VAl3+(aq) + 3e– → Al(s); –1.66 VPb2+(aq) + 2e– → Pb(s); –0.13 V Under standard-state conditions, which are the strongest reducing and oxidizing agents? Group of answer choices H+ and F2 Rb and Pb2+ Al3+ and F2 Rb and F2 Rb and F–
(a) Account for formation of the following series of oxidesin terms of the electron configurations of the elementsand the discussion of ionic K2O, CaO, Sc2O3, TiO2, V2O5, CrO3. (b) Name these oxides.(c) Consider the metal oxides whose enthalpies of formation(in kJ mol -1) are listed here. Calculate the enthalpy changes in the following general reactionfor each case:MnOm(s) + H2(g)----->nM(s) + mH2O(g)(You will need to write the balanced equation for each caseand then compute ΔH°.) (d) Based on the data given, estimatea value of ΔHf° for Sc2O3(s).
The reaction of lithium with sulfur is similar to that of sodium with sulfur. Write the balanced chemical equation for the reaction of lithium with sulfur. Include phase symbols.
At large interatomic separations, an alkali halide moleculeMX has a lower energy as two neutral atoms, M + X; atshort separations, the ionic form (M+)(X-) has a lowerenergy. At a certain distance, Rc, the energies of the twoforms become equal, and it is near this distance that theelectron will jump from the metal to the halogen atom during a collision. Because the forces between neutral atomsare weak at large distances, a reasonably good approximation can be made by ignoring any variation in potentialV(R) for the neutral atoms between Rc and R - `. For theions in this distance range, V(R) is dominated by theirCoulomb attraction.(a) Express Rc for the first ionization energy of the metalM and the electron affinity of the halogen X.(b) Calculate Rc for LiF, KBr, and NaCl using data fromAppendix F.
Assume that you have these materials:a) Li (s); b) Br2 (l); Ge (s) and d) Si(s).Choose the best electrical conductor among them and explain why.
The ionization enthalpies of group 15 elements are higher than those ofcorresponding members of group 14 and 16 elements. Assign the reason.
Determine the second ionization energy of calcium (in kJ mol-1) from the given data (all in kJ mol-1): AH°[CaCl,(s)] = -796 AH¡[Ca(g)] = 178 AH°[CI(g)] = 122 First ionization energy of Ca(g) = 590 Electron affinity of Cl(g) = -349 Lattice enthalpy of CaCl,(s) = -2260 А 1150 В 1235 C 1093 D 1210
7) The Figure 1 in the image shows the variation of ionisation energy, which increases across the periodic table. Account for the anomaly observed in groups 3A and 6A. (8) (8) Using specific examples, explain why atoms are distributed at strange angles in some molecules
( ME 213: Properties of Material) Calculate the force of attraction between a K+ and an O2- ion the centers of whichare separated by a distance of 1.5 nm. My understanding is that in ionic bonds all atoms acquire stable configuration. Here potassium gives oxygen one electron. But oxygen needs two electrons to be stable. Hence it will not be stable.

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Look at the following electron configurations. Which of the atoms will have similar chemical properties? 1. 1s 2322p4 2. 1s22:22p3 3. 1s 25 2p°3s 3p^4s?310 4p4 2 and 3 1 and 2 1 and 3 all of them