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 the electronic configuration of Aluminum (Al), we need to determine its atomic number and then fill the orbitals according to the Aufbau principle, Pauli exclusion principle, and Hund's rule. Step 1: Determine the number of electrons. Aluminum (Al) has an atomic number (Z) of 13. This means a neutral aluminum atom has 13 electrons. Step 2: Fill the orbitals in increasing order of energy (Aufbau principle). • The 1s orbital can hold 2 electrons: 1s^2 (Remaining electrons: 13 - 2 = 11) • The 2s orbital can hold 2 electrons: 2s^2 (Remaining electrons: 11 - 2 = 9) • The 2p orbital can hold 6 electrons: 2p^6 (Remaining electrons: 9 - 6 = 3) • The 3s orbital can hold 2 electrons: 3s^2 (Remaining electrons: 3 - 2 = 1) • The 3p orbital can hold up to 6 electrons. The remaining 1 electron goes into the 3p orbital: 3p^1 (Remaining electrons: 1 - 1 = 0) Step 3: Write the full spectroscopic notation. Combining the filled orbitals: 1s^2 2s^2 2p^6 3s^2 3p^1 Step 4: Write the noble gas shorthand notation. The noble gas preceding Aluminum is Neon (Ne), which has an electronic configuration of 1s^2 2s^2 2p^6. We can replace this core configuration with [Ne]. [Ne] 3s^2 3p^1 The electronic configuration of aluminum is: 1s^2 2s^2 2p^6 3s^2 3p^1 or [Ne] 3s^2 3p^1 That's 2 down. 3 left today — send the next one.