Ch.7 - Periodic Properties of the Elements

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.7 - Periodic Properties of the Elements

Problem 40

Chapter 7, Problem 40

Which of the ions Ni2+, Fe2+, Co3+, and Pt2+ has an electron configuration of 𝑛𝑑6(𝑛=3,4,5,…)?
a. Ni2+
b. Fe2+
c. Co3+
d. Pt2+
e. More than one of these

Verified step by step guidance

insert step 1> Determine the electron configuration of the neutral atoms: Ni, Fe, Co, and Pt. For transition metals, the general order is to fill the 4s orbital before the 3d orbital.

insert step 2> For each ion, remove electrons starting from the outermost shell, which is typically the s orbital, followed by the d orbital if necessary.

insert step 3> Calculate the electron configuration for each ion: Ni^{2+}, Fe^{2+}, Co^{3+}, and Pt^{2+}.

insert step 4> Identify which ion has an electron configuration ending in nd^6.

insert step 5> Compare the electron configurations to determine if more than one ion has the nd^6 configuration.

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Key Concepts

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

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It is represented using a notation that indicates the energy levels and sublevels occupied by electrons. For transition metals, the d-orbitals play a significant role, and understanding how to write and interpret these configurations is essential for predicting chemical behavior and properties.

Oxidation States

Oxidation states indicate the degree of oxidation of an atom in a compound, reflecting the number of electrons lost or gained. Transition metals can exhibit multiple oxidation states, which affects their electron configurations. Knowing the oxidation state of an ion helps in determining its electron configuration, especially for ions like Ni2+, Fe2+, Co3+, and Pt2+.

d-Orbital Filling

The d-orbitals are filled according to specific rules, including the Aufbau principle, Hund's rule, and the Pauli exclusion principle. For transition metals, the filling of d-orbitals is crucial for understanding their chemical properties and electron configurations. The notation 𝑛𝑑6 indicates that there are six electrons in the d-orbitals, which is key to identifying the correct ion from the given options.

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Related Practice

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a. Write an equation for the second electron affinity of chlorine.

b. Would you predict a positive or a negative quantity for this process?

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rue or false: If the electron affinity for an element is a negative number, then the anion of the element is more stable than the neutral atom.

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Write equations that show the processes that describe the first, second, and third ionization energies of an aluminum atom. Which process would require the least amount of energy?

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Textbook Question

In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 2.01 Å (Li–F), 2.82 Å (Na–Cl), 3.30 Å (K–Br), and 3.67 Å (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?

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Textbook Question

Write the electron configurations for the following ions, and determine which have noble-gas configurations.

a. Ru3+

b. As3−

c. Y3+

d. Pd2+

e. Pb2+

f. Au3+

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