3- The electron configurations of two different atoms are: ls²2s²2p° and 1s°2s²2p°3s'. The first ionization energy of one is 1970 kJ/mol, and that of the other is 586 kJ/mol. Match each ionization energy with one of the given electron configurations. Justify your choice.

For each of the following pairs of atoms or ions, state which you expect to have the larger radius. (a) Sm or Sm3+ (b) Mg or Ca (c) I orXe (d) Ge or As (e) Sr+ or Rb

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?

An ion M2+ has the configuration [Ar]3d2, and an atom has the configuration [Ar]4s2. Identify the ion and the atom.

Using the periodic table and without looking at Table 7.3, write electron configurations for the following elements: (a) P (b) Zn (c) Zr (d) In (e) Pb (f) U Use the spdf and noble gas notations. When you have finished, check your answers with Table 7.3.

Consider the eight most abundant elements in the human body, as outlined in Exercise 156. Excluding hydrogen, which of these elements would have the smallest size? largest size? smallest first ionization energy? largest first ionization energy?

Periodic Properties I A hypothetical element, X, has the following ionization energy values: First ionization energy: 900 kJ/mol Second ionization energy: 1750 kJ/mol Third ionization energy: 14,900 kJ/mol Fourth ionization energy: 21,000 kJ/mol Another element, Y, has the following ionization energy values: First ionization energy: 1200 kJ/mol Second ionization energy: 2500 kJ/mol Third ionization energy : 19,900 kJ/mol Fourth ionization energy: 26,000 kJ/mol a To what family of the periodic table would element X be most likely to belong? Explain? b What charge would you expect dement X to have when it forms an ion? c If you were to place elements X and Y into the periodic table, would element Y be in the same period as element X? If not in the same period, where might they be relative to each other in the periodic table? d Would an atom of Y be smaller or larger than an atom of X? Explain your reasoning.

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.

6.84 Which graph correctly depicts the first ionization energy of three elements in groups 14 (dashed line) and 17 (solid line)? Explain the reasoning you used to make your choice.