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Chapter 7: Problem 32

Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. If such an atom does not exist explain why: (a) \(\mathrm{Cl}^{-}\) (b) \(\mathrm{Sc}^{3+}\) (c) \(\mathrm{Fe}^{2+}\), (d) \(\mathrm{Zn}^{2+}\), (e) \(\mathrm{Sn}^{4+}\).

Short Answer

Expert verified
(a) \(\mathrm{Cl}^-\) has the same electron configuration as \(\mathrm{Ar}\). (b) \(\mathrm{Sc}^{3+}\) has the same electron configuration as \(\mathrm{Ar}\), but \(\mathrm{Ar}\) doesn't have an equal number of protons as either ion. (c) \(\mathrm{Fe}^{2+}\) has the same electron configuration as \(\mathrm{Cr}\). (d) \(\mathrm{Zn}^{2+}\) has the same electron configuration as \(\mathrm{Ni}\). (e) There is no neutral atom with the electron configuration of \(\mathrm{Sn}^{4+}\) because when an atom loses electrons, it may result in ion configurations that deviate from a neutral atom's patterns.

Step by step solution

01

Write the electron configuration of the given ion.

We start by writing the electron configuration of the given ion. (a) \(\mathrm{Cl}^-\): \(\mathrm{Cl}\) has 17 electrons, so when it gains one electron, it becomes \(\mathrm{Cl}^-\) with 18 electrons. The electron configuration for 18 electrons is \(1s^2 2s^2 2p^6 3s^2 3p^6\). (b) \(\mathrm{Sc}^{3+}\): \(\mathrm{Sc}\) has 21 electrons, so when it loses three electrons, it becomes \(\mathrm{Sc}^{3+}\) with 18 electrons. The electron configuration for 18 electrons is \(1s^2 2s^2 2p^6 3s^2 3p^6\). (c) \(\mathrm{Fe}^{2+}\): \(\mathrm{Fe}\) has 26 electrons, so when it loses two electrons, it becomes \(\mathrm{Fe}^{2+}\) with 24 electrons. The electron configuration for 24 electrons is \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6\). (d) \(\mathrm{Zn}^{2+}\): \(\mathrm{Zn}\) has 30 electrons, so when it loses two electrons, it becomes \(\mathrm{Zn}^{2+}\) with 28 electrons. The electron configuration for 28 electrons is \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10}\). (e) \(\mathrm{Sn}^{4+}\): \(\mathrm{Sn}\) has 50 electrons, so when it loses four electrons, it becomes \(\mathrm{Sn}^{4+}\) with 46 electrons. The electron configuration for 46 electrons is \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10}\).
02

Identify the neutral atom with the same electron configuration, if possible.

We now check if there is a neutral atom with the same electron configuration. (a) 18 electrons: This is the electron configuration for \(\mathrm{Ar}\), a noble gas. (b) 18 electrons: This is the electron configuration for \(\mathrm{Ar}\), a noble gas. Note that \(\mathrm{Cl}^-\) and \(\mathrm{Sc}^{3+}\) have the same electron configuration, but \(\mathrm{Ar}\) doesn't have an equal number of protons as either ion. (c) 24 electrons: This is the electron configuration for \(\mathrm{Cr}\). (d) 28 electrons: This is the electron configuration for \(\mathrm{Ni}\). (e) 46 electrons: There is no neutral atom that has this electron configuration.
03

Explain why no neutral atom has the same electron configuration if appropriate.

For (e), there is no known neutral atom with the electron configuration of \(\mathrm{Sn}^{4+}\). The reason is that when an atom loses electrons, it may not follow the expected patterns of electron distribution, which generally occur in neutral atoms. This can result in ion configurations that deviate from a neutral atom's patterns.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Ions
Ions are atoms or molecules that have gained or lost one or more electrons, resulting in a net electric charge. When an atom loses electrons, it becomes a positively charged ion, known as a cation. Conversely, if it gains electrons, it forms a negatively charged ion, called an anion.
  • Positive ions (cations) form when an atom loses one or more electrons.
  • Negative ions (anions) form when an atom gains one or more electrons.
The formation of ions is crucial for various chemical reactions and is a key part of understanding electron configurations. Often, ions seek to achieve a stable electron configuration, similar to noble gases, which is driving many chemical reactions and bonding activities.
The Role of Neutral Atoms
Neutral atoms are atoms with no net charge, meaning they have an equal number of protons and electrons. This balance ensures that the electric charges cancel each other out, resulting in a neutral charge.
In the context of electron configurations:
  • Neutral atoms have all electrons they originally own intact, without loss or gain.
  • The electron configuration of a neutral atom dictates its chemical properties and reactivity.
Understanding the electron configuration of neutral atoms helps predict what ions they might form as they gain or lose electrons to achieve stability.
What Happens During Electron Loss?
Electron loss usually leads to the formation of a positive ion or cation. This process is crucial in getting atoms to mimic the stable electron configuration of noble gases.
  • When an electron is lost, the remaining electrons rearrange to stabilize the atom, often leading to a configuration similar to the nearest noble gas.
  • Electron loss decreases the negative charge, making the atom positively charged.
For example, in the case of \(Sc^{3+}\), losing three electrons results in the electron configuration matching that of argon, a noble gas. This shows the significance of electron loss in achieving stable configurations and highlights how ions often mimic noble gas configurations for stability.
Noble Gas Configuration Explained
Noble gas configurations are the electron structures that are particularly stable. Noble gases like helium, neon, and argon have complete outer electron shells, making them chemically inert and stable.
Achieving a noble gas configuration is a common goal for ions and atoms as they undergo electron gain or loss.
  • Atoms often lose or gain electrons to match the electron configuration of the nearest noble gas, which is a highly stable arrangement.
  • For example, chloride ion \(Cl^{-}\) gains an electron to achieve the electron configuration of argon.
This constant striving for a noble gas configuration significantly influences chemical behavior, as having a full outer electron shell minimizes energy and enhances stability.

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Most popular questions from this chapter

Compare the elements sodium and magnesium with respect to the following properties: (a) electron configuration, (b) most common ionic charge, (c) first ionization energy, (d) reactivity toward water, (e) atomic radius. Account for the differences between the two elements.

Write the electron configurations for the following ions: (a) \(\ln ^{3+}\) (b) \(\mathrm{Sb}^{3+}\) (c) \(\mathrm{Te}^{2-}\), (d) \(\mathrm{Te}^{6+}\) (e) \(\mathrm{Hg}^{2+}\) (f) \(\mathrm{Rh}^{3+}\),

Consider the isoelectronic ions \(\mathrm{F}^{-}\) and \(\mathrm{Na}^{+}\). (a) Which ion is smaller? (b) Using Equation \(7.1\) and assuming that core electrons contribute \(1.00\) and valence electrons contribute \(0.00\) to the screening constant, \(S\), calculate \(Z_{\text {efi }}\) for the \(2 \mathrm{p}\) electrons in both ions. (c) Repeat this calculation using Slater's rules to estimate the screening constant, \(S\). (d) For isoelectronic ions, how are effective nuclear charge and ionic radius related?

In Chapter 1 we learned that silicon is the second most abundant element in Earth's crust, accounting for more than one-fourth of the mass of the crust (Figure 1.6). Yet we see that silicon is not among the elements that have been known since ancient times (Figure \(7.2\) ), whereas iron, which accounts for less than \(5 \%\) of Earth's crust, has been known since prehistoric times. Given silicon's abundance how do you account for its relatively late discovery?

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