10. Periodic Properties of the Elements

Which electron configuration violates the Pauli exclusion principle?

Use the periodic table to write an electron configuration for each element. Represent core electrons with the symbol of the previous noble gas in brackets. c. Zr

Use the periodic table to write an electron configuration for each element. Represent core electrons with the symbol of the previous noble gas in brackets. b. Ge

Use the periodic table to determine the element corresponding to each electron configuration. d. [Kr] 5s2

Use the periodic table to determine the element corresponding to each electron configuration. b. [Ar] 4s23d2

What noble-gas configurations and charge are the following elements likely to attain in reactions in which they form ions? (c) S

What noble-gas configurations and charge are the following elements likely to attain in reactions in which they form ions? (b) Ca

The following do not represent valid ground-state electron configurations for an atom either because they violate the Pauli exclusion principle or because orbitals are not filled in order of increasing energy. Indicate which of these two principles is violated in each example. (b) 3Xe46s3

The following electron configurations represent excited states. Identify the element and write its ground-state condensed electron configuration. (b) 3Ne43s13p44p1.

Scientists have speculated that element 126 might have a moderate stability, allowing it to be synthesized and characterized. Predict what the condensed electron configuration of this element might be.

Give the expected ground-state electron configurations for atoms with the following atomic numbers. (c) Z = 80

The discovery of hafnium, element number 72, provided a controversial episode in chemistry. G. Urbain, a French chemist, claimed in 1911 to have isolated an element number 72 from a sample of rare earth (elements 58–71) compounds. However, Niels Bohr believed that hafnium was more likely to be found along with zirconium than with the rare earths. D. Coster and G. von Hevesy, working in Bohr's laboratory in Copenhagen, showed in 1922 that element 72 was present in a sample of Norwegian zircon, an ore of zirconium. (The name hafnium comes from the Latin name for Copenhagen, Hafnia). (d) Using their electron configurations, account for the fact that Zr and Hf form chlorides MCl4 and oxides MO2.

The discovery of hafnium, element number 72, provided a controversial episode in chemistry. G. Urbain, a French chemist, claimed in 1911 to have isolated an element number 72 from a sample of rare earth (elements 58–71) compounds. However, Niels Bohr believed that hafnium was more likely to be found along with zirconium than with the rare earths. D. Coster and G. von Hevesy, working in Bohr's laboratory in Copenhagen, showed in 1922 that element 72 was present in a sample of Norwegian zircon, an ore of zirconium. (The name hafnium comes from the Latin name for Copenhagen, Hafnia). (a) How would you use electron configuration arguments to justify Bohr's prediction?

Consider the noble gas xenon. (a) Write the electron configuration of xenon using the abbreviation of the previous noble gas.