IB Chemistry SL 1.3 Electron Configurations

Practise interpreting emission spectra and quantised energy levels, sketching s and p orbitals, and writing atom or ion electron configurations.

[Maximum number: 8]

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.

(a)

Deduce the electron arrangements of the lithium ion, $\mathrm{Li}^{+}$ , and the boron atom, B .
$\mathrm{Li}^{+}$ :
B:

[ 2 ]

$\mathrm{Li}^{+}: 2 / 1 \mathrm{~s}^{2}$ ;
$B: 2,3 / 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{1}$ ;

(b)

Every element has its own unique line emission spectrum.

[ 6 ]

(i)

Distinguish between a continuous spectrum and a line spectrum.

[ 2 ]

(ii)

Draw a diagram to show the electron transitions between energy levels in a hydrogen atom that are responsible for the two series of lines in the ultraviolet and visible regions of the spectrum. Label your diagram to show three transitions for each series.

[ 4 ]

[Maximum number: 1]

What is the maximum number of electrons that can occupy the n=3 main energy level?

A

3

B

8

C

18

D

28

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IB Chemistry SL 1.3 Electron Configurations

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Covered syllabus points

1.3 Electron configurations question 1

Question (a)

Question (b)

Question (i)

Question (ii)

1.3 Electron configurations question 2