**Anomalous Electron Configurations**Some atoms, such as certain transition metals and elements in the lanthanide and actinide series, do not strictly follow Hund's rule. The anomalies are due to the unusual stability of both half-filled and completely filled subshells. This can be illustrated with the example of the chromium atom. Using Hund’s rule and Pauli’s principle, the expected electron configuration of a chromium atom can be written as:1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁴However, by moving an electron from the 4s orbital to the 3d orbital, you obtain a half-filled 3d orbital. This half-filled orbital is more stable than the combination of a filled 4s orbital and a partially filled 3d orbital. Thus, the observed electron configuration of a Cr atom is:1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵---**Part D**Ag has an anomalous electron configuration. Write the observed electron configuration of Ag.Express your answer in complete form in order of orbital filling. For example, 1s² 2s² should be entered as 1s^2 2s^2.- View Available Hint(s)[Answer Box]

Ag has an anomalous electron configurationWe have to write the observed electron configuration of Ag…

Anomalous electron configurations Some atoms, such as some transition metals and some elements in the lanthanide and actinide series, do not adhere strictly to Hund's rule. The reason the anomalies are observed is the unusual stability of both half-filled and completely filled subshells. This behavior can be explained with an example of the chromium atom. Using Hund's rule and Pauli's principle, you can write the expected electron configuration of the Cr atom that strictly follows these rules as I orbital you obtain a half-filled 3d orbital. This half-filled orbital is more stable than the combination of the filled 4s orbital and the partially filled 3G 18² 28² 2p 38² 3p6 48² 3d. However, by moving an electron from the 4s orbital to the orbital. Thus, the observed electron configuration of the Cr atom is 18²2 28² 2p 3s 3p 4s¹ 3d5. Y Part D Ag has an anomalous electron configuration. Write the observed electron configuration of Ag. Express your answer in complete form in order of orbital filling. For example, 182 2s2 should be entered as 1s^22s^2. bls Hinte)

Anomalous electron configurations Some atoms, such as some transition metals and some elements in the lanthanide and actinide series, do not adhere strictly to Hund's rule. The reason the anomalies are observed is the unusual stability of both half-filled and completely filled subshells. This behavior can be explained with an example of the chromium atom. Using Hund's rule and Pauli's principle, you can write the expected electron configuration of the Cr atom that strictly follows these rules as I orbital you obtain a half-filled 3d orbital. This half-filled orbital is more stable than the combination of the filled 4s orbital and the partially filled 3G 18² 28² 2p 38² 3p6 48² 3d. However, by moving an electron from the 4s orbital to the orbital. Thus, the observed electron configuration of the Cr atom is 18²2 28² 2p 3s 3p 4s¹ 3d5. Y Part D Ag has an anomalous electron configuration. Write the observed electron configuration of Ag. Express your answer in complete form in order of orbital filling. For example, 182 2s2 should be entered as 1s^22s^2. bls Hinte)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: us, the observed eléctron configuration of the Cr atom is 1s 2s 2p" 3s Part D Mo has an anomalous…

A: Electronic configuration of molybdenum

Q: Which substance has the larger first ionization energy, sodium or rubidium? Why?

A: Sodium has the larger first ionization enegy as compare to rubidium

Q: If we consider atoms of Si and Ge, say which has the largest atomic ray. Justify your answer (be…

A: We need to predict the element having highest atomic radius among Si and Ge. This question belongs…

Q: please answer question 4.

A: Given:Velocity (Δv) = 50.0 m/s.Mass of hydrogen atom = 1 amu = 1.66 x 10-27 Kg.

Q: State the exclusion principle. What does it imply about the number and spin of electrons in an…

Q: 6. Write the condensed electron configuration for C, Si, Ge, Sn, and Pb using the appropriate…

Q: When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as…

A: Rules for filling of electrons in orbitals: (1) Aufbau principle: Orbitals are filled in order of…

Q: Consider the element osmium (Os): a. Draw the ground state orbital diagram of the highest occupied…

A: The atomic no of Os is 75

Q: The Pauli Exclusion Principle requires that

A: According to the Pauli Exclusion Principle, no two electrons can have same set of all four quantum…

Q: Label the orbitals below by dragging the purple text onto the appropriote graph. Use the concepts…

A: We are to discuss which of given graphs represent 1s, 2s, 2p, 3p orbitals.

Q: Explain these exceptions to the general trend. Match the items in the left column to the appropriate…

Q: Show the orbital-filling diagram for BrBr (bromine). Order subshells by energy, with the…

A: Atomic number of a neutral atom is equal to the number of the electrons present in it. As atomic no.…

Q: When a voltage is applied and current passes through sodium vapor, electrons are raised from the 3s…

A: When a voltage is applied and current passes through sodium vapor, electrons are raised from the…

Q: Which of the following represents the complete electron configuration for nickel? 1s2 2s2 2p6 3s1…

A: The distribution of electrons in different orbitals of an atom is known as its electronic…

Q: In Universe L, recently discovered by an intrepid team of chemists who also happen to have studied…

Q: please answer the questions in the images (part of the same question) thank you

A: The Hund’s rule state that the pairing of electrons in orbitals does not occur until all orbitals…

Q: How does the Pauli exclusion principle limit the possible electron configurations of an atom? The…

A: Answer:Pauli's exculsion principleHund's rule of maximum multiplicityAfbau principle

Q: ive the “COMPLETE” electron configuration for antimony. Is it paramagnetic or diamagnetic? If there…

A: Antimony electronic configuration 1s22s22p63s23p64s23d104p65s24d105p3

Q: Use the periodic table to identify the elements with the following electron configurations.…

Q: Assuming perfect Aufbau filling, how many electrons would be present in the highest energy subshell…

A: Aufbau is a German word meaning Building up. Aufbau principle states that lowest energy orbitals…

Q: Write the ground state electron configurations for the Zn, Cu, Co, Fe, and Cr atoms. You can write…

Q: hich statement about electrons and orbitals is false? In an atom with many electrons, 3d orbitals…

A: An atom is made up of nucleus that consist of protons and neutrons.

Q: Which of these electron configurations represents the ground state electron configuration of a d…

A: There are various types of sub levels - 1- s sub level 2- p sub level 3- d sub level 4- f sub level

Q: Define the Aufbau Principle, the Pauli Exclusion Principle, and Hund's Rule. Demonstrate how they…

Q: Write the ground-state electron configuration and draw an orbital diagram for a neutral atom…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Concept explainers

Atomic Structure

The basic structure of an atom is defined as the component-level of atomic structure of an atom. Precisely speaking an atom consists of three major subatomic particles which are protons, neutrons, and electrons. Many theories have been stated for explaining the structure of an atom.

Shape of the D Orbital

Shapes of orbitals are an approximate representation of boundaries in space for finding electrons occupied in that respective orbital. D orbitals are known to have a clover leaf shape or dumbbell inside where electrons can be found.

Question

**Anomalous Electron Configurations**

Some atoms, such as certain transition metals and elements in the lanthanide and actinide series, do not strictly follow Hund's rule. The anomalies are due to the unusual stability of both half-filled and completely filled subshells. This can be illustrated with the example of the chromium atom. Using Hund’s rule and Pauli’s principle, the expected electron configuration of a chromium atom can be written as:

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁴

However, by moving an electron from the 4s orbital to the 3d orbital, you obtain a half-filled 3d orbital. This half-filled orbital is more stable than the combination of a filled 4s orbital and a partially filled 3d orbital. Thus, the observed electron configuration of a Cr atom is:

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵

---

**Part D**

Ag has an anomalous electron configuration. Write the observed electron configuration of Ag.

Express your answer in complete form in order of orbital filling. For example, 1s² 2s² should be entered as 1s^2 2s^2.

- View Available Hint(s)

[Answer Box]

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: Introduce the problem

VIEW

Step 2: write the observed electron configuration of Ag

VIEW

Solution

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

As you have seen, the periodic table is a result of empirical observation (i.e., the periodic law), but quantum-mechanical theory explains why the table is so arranged. Suppose that, in another universe, quantum theory was such that there were one s orbital but only two p orbitals (instead of three) and only three d orbitals (instead of five). Draw out the first four periods of the periodic table in this alternative universe. Which elements would be the equivalent of the noble gases? Halogens? Alkali metals?
List the values of all four quantum numbers for each of the valence electrons of radium (Ra). State how these two sets of quantum numbers satisfy Pauli exclusion principle. List all the possible values of magnetic quantum number for the electrons in praseodymium? How many magnetic quantum number values are possible for the electrons in the energy level that is closest to the nucleus of praseodymium? List the values.
What is the electron configuration of a neutral atom with 35 electrons? Assume that this electron configuration obeys the Aufbau principle. 1s22s22p63s23p64s23d104p5 1s²2s22p63s²3p64s24p5 1s 2s22p63 p63d104s24p5
use the photon energies (Li E = 178.428 KJ/mol) to determine the valence orbital energies for both Li and Na. For lithium, the transition is from the 2p- to the 2s-orbital, and the 2s-orbital energy is –520.3 kJ/mol. Use this to find the energy of the 2p-orbitals in Li. For sodium, the higher-energy photon is emitted when the electron drops from one of the 3p-orbitals to the 3s-orbital, while the lower energy photon is emitted when the electron drops from one of the 3d-orbitals to one of the 3p-orbitals. Use these facts, along with the known energy of the 3s-orbital (–495.8 kJ/mol), to find the energies of the 3p- and 3d-orbitals.
In Universe L, recently discovered by an intrepid team of chemists who also happen to have studied interdimensional travel, quantum mechanics works just as it does in our universe, except that there are four d orbitals instead of the usual number we observe here. Use these facts to write the ground-state electron configurations of the seventh and eighth elements in the first transition series in Universe L. Note: you may use [X] to stand for the electron configuration of the noble gas at the end of the row before the first transition series. seventh transition metal: eighth transition metal:
Imagine a universe where there are three spin states for the electron instead of two (for example, spin up, spin down, and spin cray-cray). The number of subshells per shell and number of orbitals per subshell stay the same, but an orbital now holds three electrons instead of two. The names of the elements stay the same. Draw the top three rows of what this new periodic table would look like, indicating which elements are in which groups in our new universe, and show the electron configurations of each of the elements of these three rows.
How many electrons can be removed from element 71 before it is reduced to its core electron configuration? For the purposes of this question, the core electron configuration is the configuration of the next lightest rare gas atom.
Select the statement(s) that explain(s) the relationship between the arrangement of elements by size and first ionization energy. 1. The first set of paired electrons in a pp subshell experience a large amount of electron-electron repulsion, making the fourth electron in a pp subshell easy to remove. 2. The third unpaired electron in a pp subshell causes a lot of electron-electron repulsion among the orbitals, making the third electron in a pp subshell easy to remove. 3. A pp subshell with only one unpaired electron is extremely stable, making the fifth electron in a pp subshell easy to remove. 4. The two arrangements are the same because IE of elements increases from left to right and the radii of elements decreases from left to right. 5. A full ss subshell is able to shield a newly filled pp subshell from the nucleus, making the first electron in a pp subshell easy to remove.