8.30. Periodic Properties II
Consider two hypothetical elements, W and Z. Element W has anelectron affinity of -150 kJ/mol, and element Z has an electronaffinity of -38 kJ/mol.
â¢ c. Assuming that the elements are in the same period, whichelement would you expect to have the smaller first ionizationenergy?

answers

watching

184

views

For unlimited access to Homework Help, a Homework+ subscription is required.

Join us on Discord

Chemistry Study Group

Join now

Related questions

Element W has an electron affinity of ?150 kJ/mol, and element Z has an electron affinity of ?38 kJ/mol. Do the valence electrons in element Z feel a greater effective nuclear charge than those in element W? Explain how you arrived at your answer.

grayfish277

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

To what family of the periodic table would element X be most likely to belong? Explain?
What charge would you expect dement X to have when it forms an ion?
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?
Would an atom of Y be smaller or larger than an atom of X? Explain your reasoning.

turquoisecheetah392

Please show all work necessary! Thank you :)

1. Four elements have the following ionization energies in kJ/mol: 762, 709, 579, and 558. The elements, in random order are Ga, Ge, In, and Sn. Which element has an ionization energy of 558 kJ/mol? 762 kJ/mol?

2. The first four ionization energies for aluminum are 578, 1,817, 2,745, and 11,577 kJ/mol. These values represent the formation of the Al¹^+, Al²⁺, Al³⁺, and Al⁴⁺ ions respectivly. Suggest a reason for the comparatively high fourth ionization energy of aluminum. Use your periodic table.

3. Suggest a reason why iodine likes to form negative ions as opposed to positive ones.