Deck 8: Atomic Structure

Question 1

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

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

Answer 1

B

Question 2

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

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

Answer 2

A

Question 3

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.

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

Answer 3

D

Question 4

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.

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

Question 5

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

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

Question 6

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

Question 7

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

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

Question 8

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

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

Question 9

Atomic sulfur, S, has a ground electronic configuration that gives rise to the levels ³P_2,1,0, ¹D₂ and ¹S₀. Use Hund's rule to predict which of these levels is lowest in energy.

A) ¹S₀
B) ¹D₂
C) ³P₀
D) ³P₂