A space probe identifies a new element in a sample collected from an asteroid. Successive ionization energies, in attojoules peratom, for the new element are given in the table.h₂ 13 TA1.017 4.108 5.074I0.507Is1 (1A)2 (2A)13 (3A)14 (4A)15 (5A)16 (6A)17 (7A)18 (8A)6.14716177.903 8.294To what family of the periodic table does this new element probably belong?

Ionization energy is simple terms can be described as a measure of the difficulty in removing an…

A space probe identifies a new element in a sample collected from an asteroid. Successive ionization energies, in attojoules per atom, for the new element are given in the table. 5 4.108 5.074 6.147 4 0.507 h O I (1A) 2 (2A) 13 (3A) 14 (4A) 15 (5A) 16 (6A) 17 (7A) 18 (8A) 1.017 14 Is 76 7.903 h 8.294 To what family of the periodic table does this new element probably belong?

A space probe identifies a new element in a sample collected from an asteroid. Successive ionization energies, in attojoules per atom, for the new element are given in the table. 5 4.108 5.074 6.147 4 0.507 h O I (1A) 2 (2A) 13 (3A) 14 (4A) 15 (5A) 16 (6A) 17 (7A) 18 (8A) 1.017 14 Is 76 7.903 h 8.294 To what family of the periodic table does this new element probably belong?

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 145AE: The successive ionization energies for an unknown element are I1 = 896 kJ/mol I2 = 1752 kJ/mol I3 =...

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The successive ionization energies for an unknown element are I1 = 896 kJ/mol I2 = 1752 kJ/mol I3 = 14,807 kJ/mol I4 = 17,948 kJ/mol To which family in the periodic table does the unknown element most likely belong?
6.82 A particular element has the following values for its first four ionization energies: 900, 1760, 14, 850, and 21,000 kJ/mol. Without consulting a list of ionization energy values, determine what group in the periodic table this element belongs in.
The changes in electron affinity as one goes down a group in the periodic table are not nearly as large as the variations in ionization energies. Why?
r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For example, the second ionization energy is the energy to remove a second electron from an element. Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the 1s orbital. l> X Y First 170 200 second 350 400 Third 1800 3500 fouth 2500 5000 entify the elements X and Y. There may be more than one answer. so explain completely.
Answer the following questions about first ionization energies. (a) Generally ionization energies increase on proceeding across a period, but this is not true for magnesium (738 kJ/mol) and aluminium (578 kJ/mol). Explain this observation. (b) Explain why the ionization energy of phosphorus (1012 kJ/mol) is greater than that of sulphur (1000 kJ/mol) when the general trend in ionization energies in a period would predict the opposite.
The electron affinity for sulfur is more negative than that for oxygen. How do you account for this?
The following numbers are the ratios of second ionization energy to first ionization energy: Na: 9.2 Mg: 2.0 Al: 3.1 Si: 2.0 P: 1.8 S: 2.3 Cl: 1.8 Ar: 1.8 Explain these relative numbers.
Name the element corresponding to each characteristic below. (a) the element with the electron configuration 1s22s22p63s23p3 (b) the alkaline earth element with the smallest atomic radius (c) the element with the largest ionization energy in Croup 5A (d) the element whose 2+ ion has the configuration [Kr]4d5 (e) the element with the most negative electron attachment enthalpy in Croup 7A (f) the element whose electron configuration is [Ar]3d104s2
6.63 At which ionization for chlorine would you expect the first large jump in ionization energy? Would this be the only large jump in energy if you continued to ionize the chlorine?
Using data from the text, determine the following values (justify your answer): a. the electron affinity of Mg2+ b. the ionization energy of CI. c. the electron affinity of Cl+ d. the ionization energy of Mg (electron affinity of Mg = 230 kJ/mol)
Three elements have the electron configurations 1s22s22P63s2, 1s22s22p63s23p4, and 1s22s22p63s23p64s2. The first ionization energies of these elements (not in the same order) are 0.590, 0.999, and 0.738 MJ/mol. The atomic radii are 104, 160, and 197 pm. Identify the three elements, and match the appropriate values of ionization energy and atomic radius to each configuration. Complete the following table with the correct information.