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Chapter 8: Problem 88

The following electron configurations correspond to the ground states of certain elements. Name each element. (a) \([\mathrm{Ar}] 3 d^{10} 4 s^{2} 4 p^{3} ;\) (b) \([\mathrm{Ne}] 3 s^{2} 3 p^{4} ;\) (c) \([\mathrm{Ar}] 3 d^{1} 4 s^{2}\) (d) \([\mathrm{Kr}] 4 d^{6} 5 s^{2} ;\) (e) \([\mathrm{Xe}] 4 f^{12} 6 s^{2}\)

Short Answer

Expert verified
The corresponding elements are (a) Arsenic (As), (b) Sulfur (S), (c) Scandium (Sc), (d) Molybdenum (Mo), and (e) Lutetium (Lu)

Step by step solution

01

Identify Elements

Use the last part of the electron configuration to identify the group and period to which an element belongs. For example, with the electron configuration \([\mathrm{Ar}] 3 d^{10} 4 s^{2} 4 p^{3}\), the last part, or highest energy level, is 4p^3. This shows it belongs to the p-block, specifically Group 15 and period 4. The element with this electron configuration is Arsenic (As).
02

Solve for all

Using the same process, identify all the elements. Here are the elements under each letter: \(a) \([\mathrm{Ar}] 3 d^{10} 4 s^{2} 4 p^{3}\); Arsenic (As) \(b) \([\mathrm{Ne}] 3 s^{2} 3 p^{4}\); Sulfur (S) \(c) \([\mathrm{Ar}] 3 d^{1} 4 s^{2}\); Scandium (Sc) \(d) \([\mathrm{Kr}] 4 d^{6} 5 s^{2}\); Molybdenum (Mo) \(e) \([\mathrm{Xe}] 4 f^{12} 6 s^{2}\); Lutetium (Lu)

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Most popular questions from this chapter

Use the Balmer equation (8.2) to determine (a) the frequency, in \(s^{-1}\), of the radiation corresponding to \(n=5\) (b) the wavelength, in nanometers, of the line in the Balmer series corresponding to \(n=7\) (c) the value of \(n\) corresponding to the Balmer series line at \(380 \mathrm{nm}\)

Draw an energy-level diagram that represents all the possible lines in the emission spectrum of hydrogen atoms produced by electron transitions, in one or more steps, from \(n=5\) to \(n=1\).

Calculate the wavelengths, in nanometers, of the first four lines of the Balmer series of the hydrogen spectrum, starting with the longest wavelength component.

In everyday usage, the term "quantum jump" describes a change of a very significant magnitude compared to more gradual, incremental changes; it is similar in meaning to the term "a sea change." Does quantum jump have the same meaning when applied to events at the atomic or molecular level? Explain.

In the ground state of a hydrogen atom, what is the probability of finding an electron anywhere in a sphere of radius (a) \(a_{0},\) or \(\left(\text { b) } 2 a_{0} ?\right.\)
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