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Chapter 6: Problem 103

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 predicted condensed electron configuration for element 126 is \[ \text{Rn} \ 7s^2 \ 5f^14 \ 6d^10 \ 7p^14. \]

Step by step solution

01

Identify the Previous Noble Gas

Before we can start building the electron configuration, we need to determine which noble gas element comes before element 126 in the periodic table. This will be the starting point for our electron configuration. The last noble gas with a lower atomic number than 126 is Radon (Rn), which has atomic number 86. So our starting point will be Rn.
02

Build the Electron Configuration

Starting with Rn as our base, we will add electrons one at a time, following the Aufbau principle. This principle states that electrons are added to orbitals of lower energy first, then orbitals of higher energy.
03

Step 2.1: Add Electrons to the 7s Orbital

After Rn, the next lowest energy orbital is the 7s orbital. A maximum of two electrons can occupy an s orbital. Thus, we add two electrons to the 7s orbital: Rn 7s^2
04

Step 2.2: Add Electrons to the 5f Orbital

The 5f orbital has a capacity for 14 electrons. After filling the 7s orbital, we add 14 electrons to the 5f orbital: Rn 7s^2 5f^14
05

Step 2.3: Add Electrons to the 6d Orbital

Moving on to the 6d orbital, it has a capacity for 10 electrons. We add 10 electrons to the 6d orbital: Rn 7s^2 5f^14 6d^10
06

Step 2.4: Add Electrons to the 7p Orbital

Finally, we reach the 7p orbital. Up to this point, we have already assigned (86 + 2 + 14 + 10) = 112 electrons. Since element 126 has 126 electrons, we need to add 14 more electrons to complete its electron configuration: Rn 7s^2 5f^14 6d^10 7p^14 In conclusion, the predicted condensed electron configuration for element 126 is \[ \text{Rn} \ 7s^2 \ 5f^14 \ 6d^10 \ 7p^14. \]

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Most popular questions from this chapter

One of the emission lines of the hydrogen atom has a wavelength of 93.07 nm. (a) In what region of the elertromagnetic spectrum is this emission found? (b) Determine the initial and final values of \(n\) associated with this emission.

Consider a transition of the electron in the hydrogen atom from \(n=4\) to \(n=9 .\) (a) Is \(\Delta E\) for this process positive or negative? (b) Determine the wavelength of light that is associated with this transition. Will the light be absorbed or emitted? (c) In which portion of the electromagnetic spectrum is the light in part (b)?

It is possible to convert radiant energy into electrical energy using photovoltaic cells. Assuming equal efficiency of conversion, would infrared or ultraviolet radiation yield more electrical energy on a per-photon basis?

The speed of sound in dry air at \(20^{\circ} \mathrm{C}\) is 343 \(\mathrm{m} / \mathrm{s}\) and the lowest frequency sound wave that the human ear can detect is approximately 20 \(\mathrm{Hz}\) (a) What is the wavelength of such a sound wave? (b) What would be the frequency of electromagnetic radiation with the same wavelength? (c) What type of electromagnetic radiation would that correspond to? [Section 6.1]

Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (a) \(1 s^{2} 2 s^{2},(\mathbf{b}) 1 s^{2} 2 s^{2} 2 p^{4}\) (c) \([\operatorname{Ar}] 4 s^{1} 3 d^{5},(\mathbf{d})[\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{4}\)
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