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Chapter 6: Problem 98

Scientists have speculated that element 126 might have a moderate stability, allowing it to be synthesized and characterized. Predict what the condensed electron configuration of this element might be.

Short Answer

Expert verified
The condensed electron configuration of element 126 is: [Rn] \(7s^2 5f^{14} 6d^{10} 7p^4\).

Step by step solution

01

Determine the number of electrons

Element 126 will have 126 protons and, since it is neutral, 126 electrons. We will be placing these 126 electrons in the respective atomic orbitals according to the rules of electron configuration.
02

Recall the order of orbital filling

Following the Aufbau principle, we will place electrons in orbitals in this order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
03

Fill the orbitals with electrons

We will fill the orbitals with electrons, keeping in mind that each orbital can hold a maximum of 2 electrons, each subshell (s, p, d, f) can hold 2, 6, 10, or 14 electrons, respectively: 1. 1s: 2 2. 2s: 2 3. 2p: 6 4. 3s: 2 5. 3p: 6 6. 4s: 2 7. 3d: 10 8. 4p: 6 9. 5s: 2 10. 4d: 10 11. 5p: 6 12. 6s: 2 13. 4f: 14 14. 5d: 10 15. 6p: 6 16. 7s: 2 17. 5f: 14 18. 6d: 10 19. 7p: 4 (We only have 4 electrons left to place)
04

Write out the complete electron configuration

Writing out the electron configuration using the number of electrons assigned to each orbital: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^{10} 6p^6 7s^2 5f^{14} 6d^{10} 7p^4\)
05

Condense the electron configuration

To express this in condensed electron configuration form, we find the nearest noble gas with a lower atomic number than element 126. In this case, it is the noble gas with the electron configuration that comes before 7p - Radon (Rn). Radon electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^{10} 6p^6\) Now we can replace the electron configuration of Radon (Rn) in our full electron configuration with [Rn]: \(\text{Element 126 condensed electron configuration:}\) [Rn] \(7s^2 5f^{14} 6d^{10} 7p^4\)

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Most popular questions from this chapter

For each element, count the number of valence electrons, core electrons, and unpaired electrons in the ground state: (a) carbon, (b) phosphorus, (c) neon.

What is the maximum number of electrons that can occupy each of the following subshells: (a) \(3 p\), (b) \(5 d\), (c) 2 s, (d) 4 ?

Sodium metal requires a photon with a minimum energy of \(4.41 \times 10^{-19} \mathrm{~J}\) to emit electrons. (a) What is the minimum frequency of light necessary to emitelectrons from sodium via the photoelectric effect? (b) What is the wavelength of this light? (c) If sodium is irradiated with light of \(439 \mathrm{~nm}\), what is the maximum possible kinetic energy of the emitted electrons? (d) What is the maximum number of electrons that can be freed by a burst of light whose total energy is \(1.00 \mu] ?\)

Is energy emitted or absorbed when the following electronic transitions occur in hydrogen: (a) from \(n=4\) to \(n=2,(\mathrm{~b})\) from an orbit of radius \(2.12 \AA\) to one of radius \(8.46 \AA\), (c) an electron adds to the \(\mathrm{H}^{+}\) ion and ends up in the \(n=3\) shell?

Indicate whether energy is emitted or absorbed when the following electronic transitions occur in hydrogen: (a) from \(n=2\) to \(n=6,(b)\) from an orbit of radius \(4.76 \AA\) to one of radius \(0.529 \AA,(c)\) from the \(n=6\) to the \(n=9\) state.
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