IB Chemistry HL 1.3 Electron Configurations Questions

Practise IB Chemistry HL 1.3 by interpreting line spectra and hydrogen transitions, building electron configurations and using ionization-energy data to infer electron structure.

Exam points

Compare line and continuous spectra, linking emitted or absorbed lines to electron transitions.
Read hydrogen lines to assign transitions to n=1/2/3, compare energies and explain convergence.
Calculate maximum electron capacity with 2n² from the principal quantum number n.
Sketch spherical s and dumbbell p orbitals, showing the p-orbital node and orientation.
Write atom and ion configurations to Z=36, including Cr/Cu exceptions and 4s electron loss.
Apply Aufbau, Hund and Pauli rules in orbital boxes to infer pairing and para-/diamagnetism.
Calculate photon energy or wavelength from spectral data using E=hf and c=fλ.
Identify the convergence limit as ionization and calculate first IE from spectral data.
Explain first-ionization-energy trends using nuclear charge, shielding, distance and subshell pairing.
Infer outer-electron count or group from jumps in successive-ionization-energy data.
Explain successive ionization-energy changes as charge, shielding and shell distance change.

Covered syllabus points

1.3.1—Emission spectra 1.3.2—Hydrogen emission spectrum 1.3.3—Main energy levels 1.3.4—Sublevels 1.3.5—Orbitals and electron spin 1.3.6 (HL)—Ionization energy (IE)1.3.7 (HL)—Successive ionization energies

[Maximum number: 1]

Carbon is produced by fusion reactions in stars.

Outline how the spectra of light from stars can be used to detect the presence of carbon.

[Maximum number: 3]

Magnesium is a group 2 metal which exists as a number of isotopes and forms many compounds.

(a)

Magnesium ions produce no emission or absorption lines in the visible region of the electromagnetic spectrum. Suggest why most magnesium compounds tested in a school laboratory show traces of yellow in the flame.

[ 1 ]

(b)

Explain the convergence of lines in a hydrogen emission spectrum.

[ 1 ]

(c)

State what can be determined from the frequency of the convergence limit.

[ 1 ]

[Maximum number: 1]

What is the maximum number of electrons in energy level n = 4?

[Maximum number: 1]

Magnesium is a group 2 metal which exists as a number of isotopes and forms many compounds.

Explain the convergence of lines in a hydrogen emission spectrum.

[Maximum number: 1]

Lithium and boron are elements in period 2 of the periodic table. Lithium occurs in group 1 (the alkali metals) and boron occurs in group 3. Isotopes exist for both elements.

The electron configuration of boron is $1 s^{2} 2 s^{2} 2 p^{1}$ . Draw the shape of an s orbital and a $\mathrm{p}_{x}$ orbital on the axes below.

[Maximum number: 1]

Titanium and vanadium are consecutive elements in the first transition metal series.

State the full electron configuration of the ${ }_{22}^{48} \mathrm{Ti}^{2+}$ ion.

$1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 3 \mathrm{~d}^{2}$

[Maximum number: 1]

Magnesium is a group 2 metal which exists as a number of isotopes and forms many compounds.

State what can be determined from the frequency of the convergence limit.

[Maximum number: 1]

Titanium and vanadium are consecutive elements in the first transition metal series.

Sketch a graph of the first six successive ionization energies of vanadium on the axes provided.

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