Successive ionization energies: Lithium vs Beryllium examples

📚 Quick Study Guide

• ⚛️ Ionization energy is the energy required to remove an electron from a gaseous atom or ion.
• 📈 Successive ionization energies refer to the energies required to remove subsequent electrons. Each successive ionization energy is *always* greater than the previous one.
• ➕ The jump in ionization energy is especially large when removing an electron from a new, filled electron shell (core electrons).
• 🔑 For Lithium (Li), you'll see a large jump between the 1st and 2nd ionization energies ($IE_1$ and $IE_2$) because after removing one electron, you're removing a core electron.
• ✨ For Beryllium (Be), the large jump happens between the 2nd and 3rd ionization energies ($IE_2$ and $IE_3$) for the same reason.
• 📏 Ionization energy generally increases across a period (left to right) and decreases down a group in the periodic table.
• 📝 The general equation for ionization energy is: $X(g) + energy \rightarrow X^+(g) + e^-$

🧪 Practice Quiz

1. Which element will have a significantly larger difference between its first and second ionization energies?
   1. A. Beryllium (Be)
   2. B. Boron (B)
   3. C. Lithium (Li)
   4. D. Carbon (C)
2. Why is the second ionization energy of an element always greater than its first ionization energy?
   1. A. The nuclear charge decreases.
   2. B. The remaining electrons experience greater repulsion.
   3. C. It is easier to remove an electron from a neutral atom.
   4. D. The remaining electrons experience a greater effective nuclear charge.
3. Which of the following represents the first ionization energy of Lithium (Li)?
   1. A. $Li(s) \rightarrow Li^+(g) + e^-$
   2. B. $Li(g) \rightarrow Li^+(g) + e^-$
   3. C. $Li^+(g) \rightarrow Li^{2+}(g) + e^-$
   4. D. $Li(g) + e^- \rightarrow Li^-(g)$
4. For Beryllium (Be), which ionization energy would show the largest increase compared to the previous one?
   1. A. $IE_1$
   2. B. $IE_2$
   3. C. $IE_3$
   4. D. $IE_4$
5. Which of the following statements accurately describes the trend in successive ionization energies?
   1. A. They generally decrease.
   2. B. They generally increase.
   3. C. They remain constant.
   4. D. They fluctuate randomly.
6. What is the primary reason for the large jump in ionization energy when removing a core electron?
   1. A. Core electrons are further from the nucleus.
   2. B. Core electrons experience less shielding.
   3. C. Core electrons are at a lower energy level and experience a greater effective nuclear charge.
   4. D. Core electrons have higher kinetic energy.
7. If the first ionization energy of Lithium is $520 \frac{kJ}{mol}$ and the second ionization energy is $7298 \frac{kJ}{mol}$, what does this suggest about the electron configuration of Lithium?
   1. A. Lithium has two valence electrons.
   2. B. Lithium has a stable noble gas configuration after losing one electron.
   3. C. Lithium readily forms $Li^{2+}$ ions.
   4. D. Lithium has a very low electronegativity.