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IB
S1.3.1 Emission spectra and energy levels

IB Chemistry S1.3.1 Emission Spectra and Energy Levels Questionbank

IB Chemistry Topic S1.3.1 Emission Spectra and Energy… | RevisionDojo

Paper

Level

Question

HLPaper 2

The diagram below shows the energy levels of the $\mathrm{He}^{+}$ ion.

(a)

State what the energy value $0\ \mathrm{kJ\ mol^{-1}}$ represents for the $\mathrm{He}^{+}$ ion.

IB Chemistry Topic S1.3.1 Emission Spectra and Energy Levels Questionbank

Practice IB Chemistry Topic S1.3.1 Emission Spectra and Energy Levels with authentic exam-style questions for both SL and HL students. This question bank focuses on the exact syllabus content for S1.3.1 Emission Spectra and Energy Levels and mirrors Paper 1A, 1B, 2 style where relevant.

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[1]

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(b)

Calculate the wavelength, in nm, of the photon emitted when an electron falls from $n=4$ to $n=2$ .

(Planck’s constant $h = 6.63 \times 10^{-34}\ \mathrm{J\ s}$ , speed of light $c = 3.00 \times 10^8\ \mathrm{m\ s^{-1}}$ , Avogadro’s constant $N_A = 6.022 \times 10^{23}\ \mathrm{mol^{-1}}$ )

[3]

(c)

Determine the first ionization energy of the $\mathrm{He}^{+}$ ion in $\mathrm{kJ\ mol^{-1}}$ .

[2]

(d)

Compare the energy required for the electron transitions from $n=2$ to $n=3$ for the $\mathrm{He}^{+}$ ion and the H atom.

[3]

(e)

Sketch a diagram showing the emission spectrum for $\mathrm{He}^{+}$ corresponding to transitions ending at $n=1$ (Lyman series), indicating the trend in line spacing.

[3]

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(f)

Discuss why the emission lines converge at high frequencies, and how this convergence relates to ionization.

[2]

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