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Chapter 8: Problem 86

What is the expected ground-state electron configuration for each of the following elements? (a) tellurium; (b) cesium; (c) selenium; (d) platinum; (e) osmium; (f) chromium.

Short Answer

Expert verified
The electron configurations are: (a) Tellurium (\( Te \)): [Kr] 5s\(^2\) 4d\(^{10}\) 5p\(^4\), (b) Cesium (\( Cs \)): [Xe] 6s\(^1\), (c) Selenium (\( Se \)): [Ar] 4s\(^2\) 3d\(^{10}\) 4p\(^4\), (d) Platinum (\( Pt \)): [Xe] 6s\(^1\) 4f\(^{14}\) 5d\(^{9}\), (e) Osmium (\( Os \)): [Xe] 6s\(^2\) 4f\(^{14}\) 5d\(^6\), (f) Chromium (\( Cr \)): [Ar] 4s\(^1\) 3d\(^5\).

Step by step solution

01

Identify Element's Atomic Number

Observe the periodic table and identify the atomic number (number of protons) of each element. The atomic number is also equal to the number of electrons in an atomic ground state.
02

Applying the Aufbau principle

Follow the Aufbau Principle (which states electrons fill the lowest energy levels first), and the Pauli Exclusion Principle (no two electrons can occupy the same quantum state simultaneously). Apply these principles to fill the electron shells. Electron filling order is typically 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p.
03

Write the Electron Configuration

Write the electron configuration for the respective atomic number based on the filling order, for example, element with atomic number 2 would have electronic configuration of 1s\(^2\).

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Most popular questions from this chapter

Concerning the concept of subshells and orbitals, (a) How many subshells are found in the \(n=3\) level? (b) What are the names of the subshells in the \(n=3\) level? (c) How many orbitals have the values \(n=4\) and \(\ell=3 ?\) (d) How many orbitals have the values \(n=3, \ell=2\) and \(m_{\ell}=-2 ?\) (e) What is the total number of orbitals in the \(n=4\) level?

What must be the velocity, in meters per second, of a beam of electrons if they are to display a de Broglie wavelength of \(1 \mu \mathrm{m} ?\)

What type of orbital (i.e., \(3 s, 4 p, \ldots)\) is designated by these quantum numbers? (a) \(n=5, \ell=1, m_{\ell}=0\) (b) \(n=4, \ell=2, m_{\ell}=-2\) (c) \(n=2, \ell=0, m_{\ell}=0\)

Infrared lamps are used in cafeterias to keep food warm. How many photons per second are produced by an infrared lamp that consumes energy at the rate of \(95 \mathrm{W}\) and is \(14 \%\) efficient in converting this energy to infrared radiation? Assume that the radiation has a wavelength of \(1525 \mathrm{nm}\).

Which must possess a greater velocity to produce matter waves of the same wavelength (such as \(1 \mathrm{nm}\) ), protons or electrons? Explain your reasoning.
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