Textbook Question
True or false? c. S2− is larger than K+.
Ch.7 - Periodic Properties of the Elements
Chapter 7, Problem 38
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+
Verified step by step guidance1
Step 1: Determine the electron configuration of the neutral atom for each element. This involves knowing the atomic number and filling the orbitals according to the Aufbau principle, Hund's rule, and the Pauli exclusion principle.
Step 2: For each ion, adjust the electron configuration by adding or removing electrons. For cations (positive ions), remove electrons starting from the outermost shell. For anions (negative ions), add electrons to the outermost shell.
Step 3: Write the electron configuration for each ion after adjusting for the gain or loss of electrons. Use the noble gas shorthand notation where applicable.
Step 4: Compare the electron configuration of each ion to the nearest noble gas configuration. Noble gases have full outer electron shells, typically ending in s²p⁶.
Step 5: Identify which ions have achieved a noble-gas configuration by having a full outer shell similar to that of a noble gas. This typically means having the same electron configuration as one of the noble gases.>
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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 follows the Aufbau principle, which states that electrons fill lower-energy orbitals first, and is represented using a notation that indicates the energy levels and sublevels occupied by electrons. Understanding electron configurations is essential for predicting chemical behavior and reactivity.
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Electron Configuration Example
Ionic Charge and Electron Loss/Gain
Ionic charge refers to the net electrical charge an atom has after losing or gaining electrons. Cations are positively charged ions formed by the loss of electrons, while anions are negatively charged ions formed by the gain of electrons. The charge of an ion directly influences its electron configuration, as it alters the number of electrons present compared to the neutral atom.
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Noble Gas Configuration
Noble gas configuration refers to an electron arrangement that mirrors that of the nearest noble gas, characterized by a full outer electron shell. Atoms or ions with noble gas configurations are generally more stable and less reactive. Identifying whether an ion has a noble gas configuration helps in understanding its stability and potential chemical behavior.
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Related Practice
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. 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 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?
Textbook Question
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
Textbook Question
a. Write an equation for the second electron affinity of chlorine.
b. Would you predict a positive or a negative quantity for this process?