8. Circle the correct choice in each set with the larger atomic radius: a. Ba or Mg b. N³ or Na 9. Circle the correct choice in each set with the more favorable electron affinity: a. Na or Mg b. Li or F c. Si or P 10. Circle the correct choice in each set with the lower first ionization energy: a. N or O b. Xe or He d. K or Ca 11. Circle the atom or ion that is isoelectronic to a noble gas. Write the electron configurations out for help! a. In³+ b. V2+ c. Zn²+ d. Y³+ e. Sc

8. Circle the correct choice in each set with the larger atomic radius: a. Ba or Mg b. N³ or Na 9. Circle the correct choice in each set with the more favorable electron affinity: a. Na or Mg b. Li or F c. Si or P 10. Circle the correct choice in each set with the lower first ionization energy: a. N or O b. Xe or He d. K or Ca 11. Circle the atom or ion that is isoelectronic to a noble gas. Write the electron configurations out for help! a. In³+ b. V2+ c. Zn²+ d. Y³+ e. Sc

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 8.90QE

See similar textbooks

Similar questions

Answer the questions below concerning ground state electron configurations. (a) What element has the electron configuration [Ar]3d64s2? (b) What element has a 2+ ion with the configuration [Ar]3d5? Is the ion paramagnetic or diamagnetic? (c) Mow many unpaired electrons are in a Ni2+ ion? (d) The configuration for an element is given here. What is the identity of the element? Is a sample of the element paramagnetic or diamagnetic? How many unpaired electrons does a 3 ion of this element have? (e) What element has the following electron configuration? Write a complete set of quantum numbers for electrons 1-3.
Based on their positions in the periodic table, predict which has the smallest first ionization energy: Li, Cs, N, I.
Fluoride ion, F, has no unpaired electrons. Vanadium forms four binary fluoridesVF2, VF3, VF4, and VF5. Assume that all four are ionic compounds. (a) Which fluoride is diamagnetic? (b) Which fluoride has the greatest attraction to a magnetic field? (c) Which fluoride has two unpaired electrons per vanadium?
Answer the following questions, assuming that ms, could have three values rather than two and that the rules for n, l, and ml are the normal ones. a. How many electrons would an orbital be able to hold? b. How many elements would the first and second periods in the periodic table contain? c. How many elements would be contained in the first transition metal series? d. How many electrons would the set of 4f orbitals be able to bold?
Select the smaller member of each pair. (a) P and P3- (b) V2+ and V4+ (c) K and K+ (d) Co and Co3+
How many valence electrons do each of the following elements have, and what are the specific valence electrons for each element? a. Ca b.O c. element 117 d. In e. Ar f. Bi
Select the larger member of each pair. (a) Ca and Ca2+ (b) Sr and Sr2+ (c) F and F- (d) Cu+ and Cu2+