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Chapter 6: Problem 12

State where in the periodic table these elements appear: (a) elements with the valence-shell electron configuration \(n s^{2} n p^{5}\) (b) elements that have three unpaired \(p\) electrons (c) an element whose valence electrons are \(4 s^{2} 4 p^{1}\) (d) the \(d\) -block elements [Section 6.9\(]\)

Short Answer

Expert verified
(a) Elements with the valence-shell electron configuration \(n s^{2} n p^{5}\) appear in Group 17 (the Halogens) of the periodic table. (b) Elements with three unpaired \(p\) electrons can be found in Group 15 (the Nitrogen group) of the periodic table. (c) The element with valence electrons \(4 s^{2} 4 p^{1}\) is Gallium (Ga), which is located in Group 13 and Period 4 of the periodic table. (d) The \(d\)-block elements belong to Groups 3 to 12 (transition metals) and are located in the center of the periodic table, between the s-block and p-block elements.

Step by step solution

01

Part (a): Elements with electron configuration \(n s^{2} n p^{5}\)

These elements have 2 electrons in the s subshell and 5 electrons in the p subshell of the same energy level, which means they are 1 electron short of completing the p subshell. The element in group 17 of the periodic table (the halogens) have this electron configuration. So, the elements with such configuration are located in Group 17 (the Halogens) of the periodic table.
02

Part (b): Elements with three unpaired p electrons

Elements with three unpaired p electrons have the electron configuration \(n p^{3}\), as each p orbital can hold two electrons with opposite spins. These elements can be found in Group 15 of the periodic table, the Nitrogen group. Group 15 elements, such as nitrogen, phosphorus, and arsenic, are known to have three unpaired p-electrons.
03

Part (c): Element with valence electrons \(4 s^{2} 4 p^{1}\)

The given electron configuration indicates that the element has 2 electrons in the 4s subshell and 1 electron in the 4p subshell. To determine the element's position in the periodic table, we can look at the sum of the superscripts, which is 2 + 1 = 3. This sum represents the number of electrons in the outermost energy level or the group number in the periodic table. Therefore, the element with this electron configuration is in Group 13 and Period 4. After locating this position, we can identify the element as Gallium (Ga).
04

Part (d): The d-block elements

The d-block elements are the elements whose outermost electron enters the d-subshell. They are located in the center of the periodic table, between the s-block and p-block elements. The d-block elements belong to Groups 3 to 12 and are commonly referred to as transition metals. Examples of d-block elements include iron (Fe), copper (Cu), and gold (Au).

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Most popular questions from this chapter

What is the maximum number of electrons in an atom that can have the following quantum numbers? (a) \(n=3, m_{l}=-1 ;\) (b) \(n=4, l=2\); (c) \(n=4, l=3, m_{l}=-2 ;\) (d) \(n=5, l=2\), \(m_{l}=0 .\)

The series of emission lines of the hydrogen atom for which \(n_{f}=4\) is called the Brackett series. (a) Determine the region of the electromagnetic spectrum in which the lines of the Brackett series are observed. (b) Calculate the wavelengths of the first three lines in the Brackett series - those for which \(n_{i}=5,6,\) and 7.

Titanium metal requires light with a maximum wavelength of \(286 \mathrm{nm}\) to emit electrons. (a) What is the minimum energy of the photons necessary to emit electrons from titanium via the photoelectric effect? (b) What is the frequency of this radiation? (c) Is it possible to eject electrons from titanium metal using infrared light? (d) If titanium is irradiated with light of wavelength \(276 \mathrm{nm}\), what is the maximum possible kinetic energy of the emitted electrons?

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.

Identify the group of elements that corresponds to each of the following generalized electron configurations and indicate the number of unpaired electrons for each: (a) [noble gas]ns \(^{2} n p^{5}\) (b) \([\) noble gas \(] n s^{2}(n-1) d^{2}\) (c) \([\) noble gas \(] n s^{2}(n-1) d^{10} n p^{1}\) (d) \([\) noble \(\operatorname{gas}] n s^{2}(n-2) f^{6}\)
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