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Chapter 7: Problem 39

Write equations that show the processes that describe the first, second, and third ionization energies of a boron atom.

Short Answer

Expert verified
The first, second, and third ionization energies of a boron atom can be represented by the following equations: 1. \(B(g) \rightarrow B^{+}(g) + e^{-}\) 2. \(B^{+}(g) \rightarrow B^{2+}(g) + e^{-}\) 3. \(B^{2+}(g) \rightarrow B^{3+}(g) + e^{-}\)

Step by step solution

01

Write the equation for the first ionization energy

First ionization energy corresponds to the removal of the first electron from a neutral boron atom (B). The process can be described by the following equation: \(B(g) \rightarrow B^{+}(g) + e^{-}\) Here, \(B(g)\) represents a boron atom in the gaseous state, and \(B^{+}(g)\) represents a boron ion with a positive charge in the gaseous state after losing one electron, represented by \(e^{-}\).
02

Write the equation for the second ionization energy

Second ionization energy corresponds to the removal of the second electron from the remaining boron ion with a charge of +1. The process can be described by the following equation: \( B^{+}(g) \rightarrow B^{2+}(g) + e^{-} \) Here, \(B^{+}(g)\) represents the boron ion with a single positive charge from the previous step, and \(B^{2+}(g)\) represents a boron ion with a double positive charge in the gaseous state after losing another electron, again represented by \(e^{-}\).
03

Write the equation for the third ionization energy

Third ionization energy corresponds to the removal of the third electron from the remaining boron ion with a charge of +2. The process can be described by the following equation: \(B^{2+}(g) \rightarrow B^{3+}(g) + e^{-}\) Here, \(B^{2+}(g)\) represents the boron ion with a double positive charge from the previous step, and \(B^{3+}(g)\) represents a boron ion with a triple positive charge in the gaseous state after losing a third electron, again represented by \(e^{-}\).

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Most popular questions from this chapter

(a) Among the nonmetallic elements, the change in atomic radius in moving one place left or right in a row is smaller than the change in moving one row up or down. Explain these observations. (b) Arrange the following atoms in order of increasing atomic radius: \(S i\). \(\mathrm{A} 1\), Ge, Ga.

(a) What is the trend in first ionization energies as one proceeds down the group 7 A elements? Explain how this trend relates to the variation in atomic radii. (b) What is the trend in first ionization energies as one moves across the fourth period from \(\mathrm{K}\) to \(\mathrm{Kr}\) ? How does this trend compare with the trend in atomic radii?

Make a simple sketch of the shape of the main part of the periodic table, as shown (a) Ignoring \(\mathrm{H}\) and \(\mathrm{He}\), write a single straight arrow from the element with the smallest bonding atomic radius to the element with the largest. (b) Ignoring \(\mathrm{H}\) and \(\mathrm{He}\), write a single straight arrow from the element with the smallest first ionization energy to the element with the largest. (c) What significant observation can you make from the arrows you drew in parts (a) and (b)? [Sections \(7.3\) and 7.4]

What is the relationship between the ionization energy of an anion with a \(1-\) charge such as \(\mathrm{F}\) and the electron affinity of the neutral atom, F?

Use electron configurations to explain the following observations: (a) The first ionization energy of phosphorus is greater than that of sulfur. (b) The electron affinity of nitrogen is lower (less negative) than those of both carbon and oxygen. (c) The second ionization energy of oxygen is greater than the first ionization energy of fluorine. (d) The third ionization energy of manganese is. greater than those of both chromium and iron.
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