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Chemistry Foundational Principles Mastery Hub: The Industry

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Q1Domain Verified
In the context of the Aufbau principle as detailed in "The Complete Atomic Structure & Periodicity Course 2026," which of the following electron configurations for a neutral ground-state atom of Scandium (Sc, Z=21) demonstrates a fundamental misunderstanding of orbital filling order?
$1s^2 2s^2 2p^6 3s^2 3p^6 3d^1 4s^2$
$1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^1$
$1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^1$
$1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^2$
Q2Domain Verified
Considering the concept of effective nuclear charge ($Z_{eff}$) and its impact on atomic radii as explored in "The Complete Atomic Structure & Periodicity Course 2026," which statement accurately describes the trend of $Z_{eff}$ and its consequence for the first ionization energies across Period 3 of the periodic table?
$Z_{eff}$ decreases across Period 3, leading to a decrease in first ionization energies.
$Z_{eff}$ remains relatively constant across Period 3, resulting in a steady increase in first ionization energies.
$Z_{eff}$ increases across Period 3, but first ionization energies show a slight dip at Group 15 and 16 due to electron-electron repulsion in half-filled and fully-filled subshells.
$Z_{eff}$ increases across Period 3, leading to a significant increase in first ionization energies due to stronger attraction to valence electrons.
Q3Domain Verified
In the context of molecular orbital theory as presented in "The Complete Atomic Structure & Periodicity Course 2026," when considering the diatomic molecule $O_2$, the relative ordering of the $\sigma_{2p}$ and $\pi_{2p}$ molecular orbitals is crucial for understanding its magnetic properties. Which statement accurately reflects this ordering and its consequence for paramagnetism?
The $\sigma_{2p}$ molecular orbital is lower in energy than the $\pi_{2p}$ molecular orbitals, and the filling of the degenerate $\pi_{2p}^*$ antibonding orbitals with unpaired electrons explains the paramagnetism of $O_2$.
The $\sigma_{2p}$ molecular orbital is lower in energy than the $\pi_{2p}$ molecular orbitals, leading to diamagnetism in $O_2$.
The $\pi_{2p}$ molecular orbitals are lower in energy than the $\sigma_{2p}$ molecular orbital due to stronger sigma overlap, resulting in diamagnetism.
The $\pi_{2p}$ molecular orbitals are lower in energy than the $\sigma_{2p}$ molecular orbital due to effective pi overlap, and the filling of the degenerate $\pi_{2p}^*$ antibonding orbitals with unpaired electrons explains the paramagnetism of $O_2$.

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