Write equations that show the process for (a) the first twoionization energies of zinc (b) the fourth ionization energy of calcium.

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Identify the element and its atomic number: Zinc (Zn) has an atomic number of 30, and Calcium (Ca) has an atomic number of 20.

For the first ionization energy of zinc, write the equation for the removal of the first electron: \( \text{Zn} \rightarrow \text{Zn}^+ + e^- \).

For the second ionization energy of zinc, write the equation for the removal of the second electron from the \( \text{Zn}^+ \) ion: \( \text{Zn}^+ \rightarrow \text{Zn}^{2+} + e^- \).

For the fourth ionization energy of calcium, first consider the removal of three electrons to form \( \text{Ca}^{3+} \): \( \text{Ca} \rightarrow \text{Ca}^{3+} + 3e^- \).

Write the equation for the removal of the fourth electron from the \( \text{Ca}^{3+} \) ion: \( \text{Ca}^{3+} \rightarrow \text{Ca}^{4+} + e^- \).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It is a key concept in understanding how atoms interact and form ions. The first ionization energy refers to the energy needed to remove the first electron, while subsequent ionization energies involve removing additional electrons, which generally require more energy due to increased positive charge in the ion.

Zinc and Calcium Electron Configuration

The electron configuration of an element describes the distribution of electrons in its atomic orbitals. For zinc (Zn), the electron configuration is [Ar] 3d10 4s2, indicating it has two electrons in the outermost shell. Calcium (Ca), with the configuration [Ar] 4s2, also has two outer electrons. Understanding these configurations is essential for predicting the ionization processes and the energies involved.

Sequential Ionization Energies

Sequential ionization energies refer to the energies required to remove electrons one after another from an atom. As electrons are removed, the remaining electrons experience a greater effective nuclear charge, making subsequent ionizations more difficult and energy-intensive. This concept is crucial for understanding why the first ionization energy is lower than the fourth for elements like calcium, as the removal of more electrons leads to increased stability in the remaining electron configuration.

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Ionization Energy

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Textbook Question

In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 201 pm (Li–F), 282 pm (Na–Cl), 330 pm (K–Br), and 367 pm (Rb–I), respectively. (b) Calculate the difference between the experimentally measured ion–ion distances and the ones predicted from Figure 7.8.

Textbook Question

In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 201 pm (Li–F), 282 pm (Na–Cl), 330 pm (K–Br), and 367 pm (Rb–I), respectively. (c) What estimates of the cation– anion distance would you obtain for these four compounds using neutral atom bonding atomic radii? Are these estimates as accurate as the estimates using ionic radii?

Textbook Question

Write equations that show the processes that describe thefirst, second, and third ionization energies of a chlorineatom. Which process would require the least amount ofenergy?

Textbook Question

Which element has the highest second ionization energy: Li, K, or Be?

Textbook Question

Identify each statement as true or false:(a) Ionization energies are always endothermic.(b) Potassium has a larger first ionization energy than lithium.(c) The second ionization energy of the sodium atom is larger than the second ionization energy of the magnesium atom.(d) The third ionization energy is three times the first ionization energy of an atom.

Textbook Question

(a) What is the general relationship between the size of an atom and its first ionization energy?