Consider these ground-state ionization energies of oneelectron species:

H = 1.31 x 10³ kJ/mol

He⁺ = 5.24 x 10³ kJ/mol

Li²⁺ = 1.18 x 10⁴ kJ/mol

(a) Write a general expression for the ionization energy of any one-electron species.

(b) Use your expression to calculate the ionization energy of B⁴⁺.

(c) What is the minimum wavelength required to remove the electron from the n = 3 level of He⁺?

(d) What is the minimum wavelength required to remove the electron from the n = 2 level of Be³⁺?

general expression for the ionization energy of any one-electron species.

= z² x ground level energy / n²

z is atomic no, n is energy level.

ground level energy of

H = 1.31 x 10³ kJ/mol

He⁺ = 2² x 1.31 x 10³ kJ/mol = 5.24 x 10³ kJ/mol

Li²⁺ = 3² x 1.31 x 10³ kJ/mol = 1.18 x 10⁴ kJ/mol

b) the ionization energy of B⁴⁺.

= 5² x 1.31 x 10³ kJ/mol = 32.75 x 10³ kJ/mol

c) minimum energy required to remove the electron from the n = 3 level of He⁺ per mole

= 5.24 x 10³ / 9 kJ/mol

= 5.82 x 10² kJ/mol

= 5.82 x 10² x 10³ / 6.02 x 10²³ J

.9667 X 10⁻¹⁸ J

=.9667 X 10⁻¹⁸ / 1.6 X 10⁻¹⁹ eV

= 6.042 eV

= 1237.5 / 6.042

= 204.82 nm

=

d)