This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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To write electronic configurations at the Advanced Level in Cameroon, you follow a set of rules that dictate how electrons fill atomic orbitals. Step 1: Understand the Fundamental Principles. • Aufbau Principle: Electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. The general order is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, ... • Pauli Exclusion Principle: No two electrons in the same atom can have identical values for all four quantum numbers. This means an atomic orbital can hold a maximum of two electrons, and these electrons must have opposite spins. • Hund's Rule: For degenerate orbitals (orbitals of the same energy, like the three p orbitals or five d orbitals), electrons will occupy each orbital singly with parallel spins before any orbital is doubly occupied. Step 2: Use Spectroscopic Notation. This notation shows the principal energy level (n), the type of orbital (s, p, d, f), and the number of electrons in that orbital as a superscript. Example: Carbon (Z=6) 1s^2 2s^2 2p^2 This means there are 2 electrons in the 1s orbital, 2 in the 2s orbital, and 2 in the 2p orbital. Step 3: Use Orbital Box Diagrams. These diagrams visually represent orbitals as boxes (or lines) and electrons as arrows (up for spin-up, down for spin-down). They clearly illustrate Hund's rule and the Pauli exclusion principle. Example: Oxygen (Z=8) ccccc 1s & 2s & 2p_x & 2p_y & 2p_z \\ & & & & Notice how the 2p orbitals are filled: one electron in each 2p_y and 2p_z before the 2p_x orbital is doubly occupied. Step 4: Use Noble Gas Shorthand Notation. For larger atoms, you can use the symbol of the preceding noble gas in brackets to represent the core electrons, followed by the configuration of the valence electrons. Example: Sodium (Z=11) The preceding noble gas is Neon (Z=10), with configuration 1s^2 2s^2 2p^6. [Ne] 3s^1 Example: Iron (Z=26) The preceding noble gas is Argon (Z=18), with configuration 1s^2 2s^2 2p^6 3s^2 3p^6. [Ar] 4s^2 3d^6 Step 5: Be Aware of Exceptions. Some elements, particularly transition metals, show exceptions to the Aufbau principle due to the added stability of half-filled or fully-filled d or f subshells. The most common examples are Chromium (Cr) and Copper (Cu). Example: Chromium (Z=24) Expected: [Ar] 4s^2 3d^4 Actual: [Ar] 4s^1 3d^5 (half-filled 4s and half-filled 3d are more stable) Example: Copper (Z=29) Expected: [Ar] 4s^2 3d^9 Actual: [Ar] 4s^1 3d^10 (half-filled 4s and fully-filled 3d are more stable) Last free one today — make it count tomorrow, or type /upgrade for unlimited.