Quantum Chemistry Test Review

The series of spectral lines emitted by a hydrogen atom when an electron transitions from a higher energy level to the first energy level (n=1).

The series of spectral lines emitted by a hydrogen atom when an electron transitions from a higher energy level to the second energy level (n=2).

Electromagnetic radiation that has the longest wavelength and lowest energy.

Electromagnetic radiation that has the shortest wavelength and highest energy.

States that a specific orbital can hold a maximum of two electrons, and they must have opposite spins.

Electron configuration is a shorthand notation that describes the distribution of electrons in different energy levels (shells) and sublevels (orbitals) within an atom.

Orbital notation uses arrows to represent electrons filling sublevels, with each arrow representing one electron and pointing upwards or downwards to represent spin.

Electron configuration notation uses numerical superscripts to indicate the number of electrons in each sublevel, like 1s² 2s² 2p⁶.

Noble gas notation uses the electron configuration of the preceding noble gas in brackets, followed by the remaining electron distribution.

The number of electrons in an atom is equal to the atomic number. For ions (atoms with a charge), add the number of electrons to the atomic number if negatively charged (anion) or subtract the number of electrons from the atomic number if positively charged (cation).

Electrons fill orbitals and sublevels in a specific order, following the Aufbau principle, Hund's rule, and the Pauli exclusion principle. This order is determined by energy level, sublevels, and spin.

The Aufbau principle states that electrons fill sublevels in order of increasing energy. Some exceptions occur due to the stability of half-filled and fully-filled sublevels.

Hund's rule states that electrons individually occupy each orbital within a sublevel before pairing up within an orbital. This is due to the repulsion between electrons.

Aluminum (Al) has 13 electrons. Its electron configuration uses the noble gas configuration of Neon ([Ne]) to shorten the notation. It has 2 electrons in the 3s subshell and 1 electron in the 3p subshell.

Germanium (Ge) has 32 electrons. Its electron configuration shows the distribution of these electrons in each subshell. There are 4 electrons in the 4p subshell.

Rubidium (Rb) has 37 electrons. Its electron configuration uses the noble gas configuration of Krypton ([Kr]) to simplify the notation. There is only one electron in the 5s subshell.

Manganese (Mn) has 25 electrons. Its electron configuration shows the distribution of these electrons among the subshells. There are 5 electrons in the 3d subshell.

Strontium (Sr) has 38 electrons. Its electron configuration shows the distribution of these electrons among the subshells. It has a full 4d subshell and 2 electrons in the 5s subshell.

Titanium (Ti) has 22 electrons. Its electron configuration uses the noble gas configuration of Argon ([Ar]) for brevity and then lists the remaining electrons in the 4s and 3d subshells. It has two electrons in the 3d subshell.

Antimony (Sb) has 51 electrons. Its electron configuration shows the distribution of these electrons among the subshells. It has two electrons in the 5p subshell.

Cobalt (Co) has 27 electrons. Its electron configuration uses the noble-gas configuration of Argon ([Ar]) for brevity and then lists the remaining electrons in the 4s and 3d subshells. It has seven electrons in the 3d subshell.