Question

Ionization energy (Ei) is the amount of energy required to remove an electron from a neutral gaseous atom or gaseous ion. Electrons are attracted to the positively charged nucleus; therefore removing an electron requires energy. The process is endothermic, and so ionization energies have a positive value. The first ionization energy (Ei1) is the energy associated with the removal of an electron from the neutral gaseous atom. The reaction is represented for the generalized atom X as X→X++e− The amount of energy required to remove an electron is related to the effective nuclear charge and the stability of the electron configuration of the atom. It therefore shows periodic variation generally increasing from left to right in a period and from bottom to top of a group. In general, metals have lower Ei1 values than nonmetals. Exceptions to this general trend from left to right occur when a completely filled s subshell or half-filled p subshell is encountered. These stable configurations have larger than expected Eil values.

Part A Based on position in the periodic table and electron configuration, arrange these elements in order of decreasing Ei1. Rank the elements from highest to lowest ionization energy. To rank items as equivalent, overlap them. View Available Hint(s) Reset Help S As Se Ga K Rb Lowest ionization energy Highest ionization energy From Highest ionization energy to Lowest ionization energy. No items in the box. Background Image The correct ranking cannot be determined.

Answer 1

First Ionization energy values of the geven elements S = 1000 kJ/mol periodi As = 960 kilmol From left to right ionization energy increases. Se= 950 kJmol Group : Gaz 580 kg/mol From Top to boltom ionization energy decreases. k = 420 ks/mol Rb= hoo ks/mol Highest to lowest imization energy: s > As > Se > Ga > K > Rb lowest ionization energy = Rb Choo kil mol) Highest ionization energy =s (1000 ks/mol)