Atomic Structure and Ionisation Energy Practice Questions

Vocabulary-style study flashcards focusing on atomic structure, electron configurations, subatomic particles, and ionisation energy trends.

Element X (derived from $^{41}\text{K}$)

Scandium ($\text{Sc}$), which has an atomic number of 21 (2 more protons than potassium's atomic number of 19).

Electronic configuration of $\text{K}^+$

$$1s^2 2s^2 2p^6 3s^2 3p^6$$

Electronic configuration of Titanium ($\text{Ti}$)

$$1s^2 2s^2 2p^6 3s^2 3p^6 3d^2 4s^2$$

Electronic configuration of Cobalt ($\text{Co}$)

$$1s^2 2s^2 2p^6 3s^2 3p^6 3d^7 4s^2$$

First ionisation energy equation of Potassium

$$\text{K}(g) \rightarrow \text{K}^+(g) + e^-$$

Second ionisation energy equation of Scandium

$$\text{Sc}^+(g) \rightarrow \text{Sc}^{2+}(g) + e^-$$

Electronic configuration of $\text{Sc}^{2+}$

$$1s^2 2s^2 2p^6 3s^2 3p^6 3d^1$$

Group of Element Z

Group 14 (or Group 4), identified by the large increase between the 4th ($4356\,kJ\,mol^{-1}$) and 5th ($16091\,kJ\,mol^{-1}$) ionisation energies, showing 4 valence electrons.

Free radical

A chemical species with one or more unpaired electrons.

Shape of a 2s orbital

A spherical cloud of electron density centered symmetrically on the origin of the 3D coordinate axes.

First ionisation energy anomaly of Aluminium vs. Magnesium

Aluminium has a lower first ionisation energy than magnesium because its outermost electron is in a 3p subshell, which is higher in energy, further from the nucleus, and shielded by the 3s subshell.

Deflection of subatomic particles in an electric field

Protons curve upward toward the top negative plate, electrons curve downward toward the bottom positive plate with greater deflection due to smaller mass, and neutrons pass through un-deflected.

Subatomic composition of $^{23}\text{Na}$

11 protons, 12 neutrons, and 11 electrons.

Subatomic composition of $^{32}\text{S}^{2-}$

16 protons, 16 neutrons, and 18 electrons.

Subatomic composition of $^{86}\text{Sr}^{2+}$

38 protons, 48 neutrons, and 36 electrons.

Electronic configuration of $^{32}\text{S}^{2-}$ ion

$$1s^2 2s^2 2p^6 3s^2 3p^6$$

Radius order of isoelectronic species $\text{Mg}^{2+}$, $\text{Ne}$, and $\text{O}^{2-}$

$\text{Mg}^{2+} < \text{Ne} < \text{O}^{2-}$, because a higher proton number exerts a stronger attraction on the same number of electrons, shrinking the atomic/ionic radius.

First ionisation energy equation of Magnesium

$$\text{Mg}(g) \rightarrow \text{Mg}^+(g) + e^-$$

Second ionisation energy of Magnesium

Higher than its first ionisation energy because the second electron is removed from a positively charged ion ($\text{Mg}^+$), experiencing greater nuclear attraction.