CHE 170 (Mayo) Fall 2019 Review I Cor Arrange the following elements from greatest to least tendency to accept an electron. Rank from greatest to least tendency to accept an electron. To rank items as equivalent, overlap them. View Available Hint(s) Reset Help Least tendency Greatest tendency Na Mg Si The correct ranking cannot be determined. Previous Answers Submit Incorrect; Try Again; 7 attempts remaining ヘロの Provide Feedback Et DELL PADVANTAGE M OUCATION LOAN 20276 wwww Loa 0e g X

CHE 170 (Mayo) Fall 2019 Review I Cor Arrange the following elements from greatest to least tendency to accept an electron. Rank from greatest to least tendency to accept an electron. To rank items as equivalent, overlap them. View Available Hint(s) Reset Help Least tendency Greatest tendency Na Mg Si The correct ranking cannot be determined. Previous Answers Submit Incorrect; Try Again; 7 attempts remaining ヘロの Provide Feedback Et DELL PADVANTAGE M OUCATION LOAN 20276 wwww Loa 0e g X

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter2: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 11ALQ: Consider the following statement "The ionization energy for the potassium atom is negative, because...

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The outermost electron in an alkali-metal atom is sometimes described as resembling an electron in the corresponding state of a one-electron atom. Compare the first ionization energy of lithium with the binding energy of a 2s electron in a one-electron atom that has nuclear charge Zeff , and determine the value of Zeff that is necessary for the two energies to agree. Repeat the calculation for the 3s electron of sodium and the 4s electron of potassium.
In the hydrogen atom, the electron is in its lowest energy state, n=1. The maximum electron energy that a hydrogen atom can have is 0 kJ/mole, at which point the electron would essentially be removed from the atom and it would become a H+ ion. How much energy does it take to ionize one hydrogen atom in kilojoules per mole and in Joules per atom? (Hint: calculate ΔE where εfinal is zero and εinitial is –1312.04 kJ/mol.)
Quesion 10- (Please showall of your work so I can understand going forward) You may need to use a special periodic table to answer the question, it is attached in the images below. You will also need to look at the images to see the figure for the dot sturcture. a) Draw the electron dot structure for Fa. c) Would nitrogen have a larger or smaller ionization energy compared to Fa? (Please explain your answer)
The 2s and 2p energy levels are different. Which of thefollowing is the best explanation for why this is the case?(i) The 2s and 2p energy levels have different energies inthe hydrogen atom, so of course they will have differentenergies in the sodium atom, (ii) The energy of the 2porbital is higher than that of the 2s in all many-electronatoms. (iii) The 2s level in Na has electrons in it, whereasthe 2p does not.
(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).
(a) Write the electron configuration for Li and estimate theeffective nuclear charge experienced by the valence electron.(b) The energy of an electron in a one-electron atom or ion equals (-2.18 x 10-18 J) aZ2/n2 b, where Z is the nuclear chargeand n is the principal quantum number of the electron. Estimatethe first ionization energy of Li. (c) Compare the resultof your calculation with the value reported in Table 7.4 andexplain the difference. (d) What value of the effective nuclearcharge gives the proper value for the ionization energy? Doesthis agree with your explanation in part (c)?
There are some exceptions to the trends of first and succes-sive ionization energies. For each of the following pairs, explainwhich ionization energy would be higher:(a) IE₁ of Ga or IE₁ of Ge(b) IE₂ of Ga or IE₂ of Ge(c) IE₃ of Ga or IE₃ of Ge(d) IE₄ of Ga or IE₄ of Ge
The first ionisation energy of the chlorine atom is 1251 kJ/mol. Without looking atyour text book, say which of the following values would be the more likely ionisationenergy for the iodine atom. Explain your choice.(a) 1000 kJ/mol (b) 1400 kJ/mol
Given the following ions/atoms: A) O2- B)Na, C) Se2-, D)Sr 2+, E) KrPut these atoms/ions in order of increasing radius
Determine the second ionization energy of calcium (in kJ mol−1) from the given data (all in kJ mol−1):ΔHf°[CaCl2(s)] = −796ΔHf°[Ca(g)] = 178ΔHf°[Cl(g)] = 122First ionization energy of Ca(g) = 590Electron affinity of Cl(g) = −349Lattice enthalpy of CaCl2(s) = −2260 a)1150 b)1235 c) 1093 d) 1210
(a) Account for formation of the following series of oxidesin terms of the electron configurations of the elementsand the discussion of ionic compounds in Section 2.7: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.Oxide K2O1s2 CaO1s2 TiO21s2 V2O51s2ΔHf° -363.2 -635.1 -938.7 -1550.6Calculate the enthalpy changes in the following general reactionfor each case:MnOm1s2 + H21g2¡nM1s2 + mH2O1g2(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 Sc2O31s2.
Arrange the following in order of increasing ionization energy. Rb, F, Al, As, B, Se Options 1) ??<??<?<??<?<?? 2) ??<??<??<?<?<?? 3) ??<??<?<??<?<?? 4) ??<??<?<??<??<? 5) ??<??<??<?<?<??

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