Entrance Test Preparation

Study Notes

Entrance Test Preparation - 2024

Neutral atom with one electron in the 3d subshell indicates it belongs to the 3rd period and has 7 electrons in the outermost shell.
Maximum number of electrons in a shell can be calculated using the formula 2n², where n represents the principal quantum number.
Orbitals sharing the same values of n + l will have similar energy levels, exemplified by 3d and 3d*.
The Aufbau principle arranges subshells in order of increasing energy, following the n + l rule.
The element with a valence shell electronic configuration of 3s² is magnesium (Mg).
For electrons within different s-orbitals, only the principal quantum number changes while keeping other quantum numbers constant.
An oxide where the element (X) has 50% mass of oxygen and a relative atomic mass of 32 leads to an empirical formula of MO.
The decomposition of calcium carbonate that generates 2.24 dm³ of carbon dioxide corresponds to the decomposition of 1 mole of the reactant.
The molecular formula for glucose is C₆H₁₂O₆, illustrating the percentage relationships of its constituent elements.
The electron configuration [Ar] 4s² belongs to calcium (Ca).
The splitting of spectral lines in a magnetic field is explained by the magnetic quantum number (m).
The d-subshell has five possible shapes for its orbitals.
An orbital can be conceptualized as a region where there is a high probability of finding an electron, or as a spread of charge rather than just a fixed energy level.
Moving to higher shells results in increases in the size of shells, subshells, and orbitals, reflecting a greater spatial extent for electron distribution.

Description

Prepare for your upcoming entrance tests with this quiz focused on atomic structure and electron configurations. Test your knowledge of electron shells, subshells, and orbital theories. Ideal for students gearing up for competitive exams.