Atomic Theory, Periodic Trends, and Photoelectron Spectroscopy Flashcards

Vocabulary flashcards covering core atomic structure, photoelectron spectroscopy, periodic trends, and photon emission energy based on the lecture notes.

Excited State Electron Configuration of Magnesium

The electron configuration $1s^2 2s^2 2p^6 3s^1 3p^1$, which represents an excited state where a valence electron from the $3s$ orbital is promoted to a $3p$ orbital.

Oxygen First Ionization Energy Anomaly

The deviation of oxygen's first ionization energy from the general periodic trend, caused by electron-electron repulsion between paired electrons in its occupied $2p$ orbitals.

Second Ionization of Oxygen

The ionization process represented by the equation $\text{Energy} + \text{O}^+(g) \rightarrow \text{O}^{2+}(g) + 1e^-$.

Valence Electron Jump Identification (Aluminum)

The identification of an element as aluminum ($\text{Al}$) based on a massive jump between its third ($2{,}745\text{ kJ}\text{ mol}^{-1}$) and fourth ($11{,}577\text{ kJ}\text{ mol}^{-1}$) ionization energies, indicating the removal of a core electron.

Photoelectron 1s Peak Binding Energy (Fluorine vs. Carbon)

The peak (Peak X) assigned to fluorine $1s$ core electrons at higher binding energy than carbon $1s$ electrons, because fluorine possesses a greater nuclear charge.

Radiation Energy and Photoionization Threshold

The principle that radiation with a longer wavelength ($2.1 \times 10^{-6}\text{ m}$) has energy too low to overcome the Coulombic force holding an electron, whereas radiation with a shorter wavelength ($4.7 \times 10^{-10}\text{ m}$) carries sufficient energy to permanently eject the electron.

Strontium vs. Barium Light Emission

A comparison showing that strontium emission ($650\text{ nm}$ red light) has a longer wavelength, lower frequency, and lower energy than barium emission ($590\text{ nm}$ green light).

Core Shell Coulombic Attraction in Nitrogen

The physical principle explaining that in a nitrogen atom ($1s^2 2s^2 2p^3$), the core $1s$ electrons experience the strongest Coulombic attraction because they are located closest to the nucleus.

Anion-Forming Electron Configuration

An electron configuration such as $[\text{Kr}] 5s^2 4d^{10} 5p^5$, which represents a neutral halogen atom that readily gains an electron to form a $-1$ charged anion.

Comparative Atomic and Ionic Radii (Fluorine and Chlorine)

The relationship where a fluoride anion ($\text{F}^-$) expands beyond the fluorine atomic radius of $72\text{ pm}$, and a neutral chlorine atom ($\text{Cl}$) has a larger radius than $72\text{ pm}$ due to an additional principal energy level.

Unpaired Electrons in Transition Metals

The ground-state electronic feature where manganese ($4s^2 3d^5$) contains 5 unpaired electrons in its $3d$ subshell, more than titanium ($2$), nickel ($2$), or zinc ($0$).

Cesium First Ionization Energy

The periodic property of cesium ($\text{Cs}$) having the lowest first-ionization energy among elements like $\text{Pb}$, $\text{Br}$, and $\text{Se}$ due to its large atomic radius and weak effective nuclear pull on its outermost electron.

Period 2 Atomic Radius Trend

The systematic decrease in atomic size across Period 2 from lithium ($152\text{ pm}$) down to fluorine ($72\text{ pm}$) and neon ($70\text{ pm}$) resulting from increasing effective nuclear charge.

Sulfur Ground State Unpaired Electrons

A ground-state sulfur atom with electron configuration $1s^2 2s^2 2p^6 3s^2 3p^4$, which contains exactly two unpaired electrons in its $3p$ subshell.