Question

Which of the following samples contains the largest number of atoms: 2.0 g He, 2.0 g Ne, or 2.0 g Ar? How do you know? Justify your choice. Consider the elements aluminum (Al), sodium (Na), and sulfur (S). a. Arrange these three elements in order of increasing ionization energy. b. Discuss how the structures of the atoms of these three elements determine the relative strengths of the attractive electrostatic forces. Be sure to specify what is interacting to create the attractive electrostatic forces that are important in determining the ionization energies. c. Explain how ionization energies are related to the strengths of the electrostatic forces in atoms to support your claim in part a.

Answer 1

o-sanoly - Number of moles of number of moles of Number of moles of He weight = 2 = - mult ve- & ol more Ar= 2 = 60 = o-os male me Sample contains langest number because it has more number of moles, @ The in incheasing oraded of Ionisatich enengy - Na <AKS (from left to right increases achoss a period) from left to right, atomic number increases. As mone number of electrons are added to the same shell (across a period), 15e att bonce between nucleus and valence electrons incheaks There done with the increase is inter moleulah of nuclean toxce of attractions more energy is required to demore the electron bohom 15e Valence Shell and hence ionisation energy ý increasing @ Al loss toace of a period, brom left to rights nuclead attraction on valence electrons increases atomic size decreases, s, Ionisation eneagy increases