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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Step 1: Explain the general increase in ionization energies from sodium to silicon. As we move across a period from left to right (from sodium to silicon), the nuclear charge (number of protons) increases. Electrons are added to the same principal energy level, meaning the shielding effect from inner electrons remains relatively constant. This results in a greater effective nuclear charge experienced by the valence electrons, pulling them more strongly towards the nucleus. Consequently, more energy is required to remove an electron, leading to a general increase in first ionization energy. Step 2: Determine the electronic configurations for magnesium and aluminum. • Magnesium (Mg) has an atomic number of 12. Its electronic configuration is 1s^2 2s^2 2p^6 3s^2 or [Ne] 3s^2. • Aluminum (Al) has an atomic number of 13. Its electronic configuration is 1s^2 2s^2 2p^6 3s^2 3p^1 or [Ne] 3s^2 3p^1. Step 3: Explain why aluminum has a lower first ionization energy than magnesium. Magnesium's first electron to be removed is from a filled 3s subshell (3s^2). Aluminum's first electron to be removed is from a 3p subshell (3p^1). The 3p electron in aluminum is at a slightly higher energy level and is shielded by the inner 3s^2 electrons. This additional shielding and the higher energy of the 3p orbital mean that the 3p electron in aluminum is less attracted to the nucleus and requires less energy to remove compared to a 3s electron in magnesium. a) The general increase in ionization energies from sodium to silicon is due to the increase in effective nuclear charge across the period. As the atomic number increases, the number of protons in the nucleus increases, leading to a stronger attraction for the valence electrons. Since electrons are added to the same principal energy level, the shielding effect does not significantly increase, making it harder to remove an electron. b) • Magnesium (Mg) electronic configuration: [Ne] 3s^2 • Aluminum (Al) electronic configuration: [Ne] 3s^2 3p^1 Aluminum has a lower first ionization energy than magnesium because the electron being removed from aluminum is a 3p electron, while the electron being removed from magnesium is a 3s electron. The 3p electron in aluminum is at a slightly higher energy level and is shielded by the filled 3s^2 subshell. This shielding reduces the effective nuclear charge experienced by the 3p electron, making it easier to remove compared to a 3s electron in magnesium, which is closer to the nucleus and experiences less shielding. Send me the next one 📸