. Which alkali metal would be expected to have the lowest first ionizationenergy?W●Which labeled element in the third period of the chart above has the highestquantity electron affinity energy?A/●Type the letter from the given chart of the alkaline earth metal that has thelargest atomic radius.A/Select from the given letters, the letter of the element that would be the mostelectronegative on this periodic chart.AOIIActivGo to63°F Cle x|H|VRESYou will use the known periodic trends to compare properties for elements indicatewith letters in this periodic table. Consider their relative positions for thesequestions. Your answers will be letters as indicated above, not the actual elementsymbol they would coordinate to. (Do not use a real periodic to answer thisquestion.)●Which alkali metal would be expected to have the lowest first ionizationenergy?BIHON>TDLIQA0

In this question, we have to write the letter following te trend for the given questions.

. Which alkali metal would be expected to have the lowest first ionization energy? A/ . Which labeled element in the third period of the chart above has the highest quantity electron affinity energy? Type the letter from the given chart of the alkaline earth metal that has the largest atomic radius. A/ ● Select from the given letters, the letter of the element that would be the most electronegative on this periodic chart. A O II Activ Go to 63°F Cle

. Which alkali metal would be expected to have the lowest first ionization energy? A/ . Which labeled element in the third period of the chart above has the highest quantity electron affinity energy? Type the letter from the given chart of the alkaline earth metal that has the largest atomic radius. A/ ● Select from the given letters, the letter of the element that would be the most electronegative on this periodic chart. A O II Activ Go to 63°F Cle

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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. Fr->Fr+ + e- / B->B+ + e- Al->Al+ + e- / He-> He+ + e- He->He+ + e- / Ti->Ti+ + e-
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Order the elements below from smallest to largest 1st ionization energy. Mg, Cl, K, As _____ < ____< _____< ______,
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10. Which of the following elements would have the greatest difference between the first and the second ionization energies? A) Ca B) Sr C) Na D) CI E) C
5. Isoelectronic ions are the species that have the same number of electrons. Part a. What +2 ion is isoelectronic with Na+? What -2 ion? Part b. Which of the following has (have) the same electron configuration as (isoelectronic with) Ar? A. K- B. Ca2+ C. 02- D. CI-
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Choose the symbol of an atomic ion for each of the following electron configurations: 1s 2s 2p° a. ONi+ OLit O Ge+ OF O Ge?+ OCI 1s 2s 2p°3s*3p°4s" b. O Br ON O Ca²+ O Ca* OB 1s 2s 2p с. Oc+ Oc+ Oct ON+ ONi+ omnts remaining
Which arrangement is in the correct order of increasing first ionization energy? Select one: a. F < C < Li b. Be < Mg < Ca c. Rb < K < Na d. Si < Ar < S e. Cl < Br < F