Question 1

To which orbitals may 5d electrons make spectroscopic transitions in a hydrogenic atom?

Accepted Answer

A)   ns and np
B)   np and nd
C)   ns and nd
D)   np and nf D

Question 2

Calculate the Coulombic potential energy of an electron at a distance of 52.9 pm from a lithium, Li2+, nucleus.

Accepted Answer

A)   -4.37  10-18 J
B)   -1.31  10-17 J
C)   -5.20  1020 J
D)   9.63  106 J B

Question 3

The Rydberg constant for the Be3+ ion is 109731 cm-1. Calculate the ionization energy of a ground-state Be3+ ion.

Accepted Answer

A)   218 eV
B)   13.6 eV
C)   54.4 eV
D)   9.3 eV A

Question 4

Which terms can arise from the electronic configuration [He]2s22p2?

Accepted Answer

A)   3D, 1D, 3P, 1P, 3S and 1S
B)   1D, 3P, and 1S
C)   3D, 1D
D)   1S

Question 5

For a hydrogen atom, calculate the energy of an electron with principal quantum number n = 3.

Accepted Answer

A)   -2.421  10-19 J
B)   -1.835  10-23 J
C)   -2.421  10-17 J
D)   -1.835  10-25 J

Question 6

Atomic sulfur, S, has a ground electronic configuration that gives rise to the levels 3P2,1,0, 1D2 and 1S0. Use Hund's rule to predict which of these levels is lowest in energy.

Accepted Answer

A)   1S0
B)   1D2
C)   3P0
D)   3P2

Question 7

Calculate the overall change in energy when an electron is transferred from a sodium atom, Na, to a chlorine atom, Cl, to form a sodium ion, Na+, and chlorine ion, Cl-. The first ionization energy of sodium is 5.14 eV. The electron affinity of chlorine is +3.62 eV.

Accepted Answer

A)   1.52 kJ mol-1
B)   845 kJ mol-1
C)   147 kJ mol-1
D)   495 kJ mol-1

Question 8

A line in the Balmer series of the emission spectrum of atomic hydrogen is observed at a wavelength of 486.3 nm. Deduce the upper state principal quantum number for this transition.

Accepted Answer

A)   2
B)   3
C)   4
D)   5

Question 9

Calculate the wavenumber of the lowest energy transition in the B series of the electronic spectrum of the He+ ion. The Rydberg constant for He is RHe = 109707 cm-1.

Accepted Answer

A)   109707 cm-1
B)   5332 cm-1
C)   21941 cm-1
D)   21332 cm-1

Exam 8: Atomic Structure

To which orbitals may 5d electrons make spectroscopic transitions in a hydrogenic atom?

Calculate the Coulombic potential energy of an electron at a distance of 52.9 pm from a lithium, Li²⁺, nucleus.

The Rydberg constant for the Be³⁺ ion is 109731 cm^-1. Calculate the ionization energy of a ground-state Be³⁺ ion.

Which terms can arise from the electronic configuration [He]2s²2p²?

For a hydrogen atom, calculate the energy of an electron with principal quantum number n = 3.

Atomic sulfur, S, has a ground electronic configuration that gives rise to the levels ³P₂_,1,0, ¹D₂ and ¹S₀. Use Hund's rule to predict which of these levels is lowest in energy.

Calculate the overall change in energy when an electron is transferred from a sodium atom, Na, to a chlorine atom, Cl, to form a sodium ion, Na⁺, and chlorine ion, Cl^-. The first ionization energy of sodium is 5.14 eV. The electron affinity of chlorine is +3.62 eV.

A line in the Balmer series of the emission spectrum of atomic hydrogen is observed at a wavelength of 486.3 nm. Deduce the upper state principal quantum number for this transition.

Calculate the wavenumber of the lowest energy transition in the B series of the electronic spectrum of the He⁺ ion. The Rydberg constant for He is R_He = 109707 cm^-1.