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Chapter 6: Problem 10

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

Short Answer

Expert verified
(a) Elements with the valence-shell electron configuration \(n s^{2} n p^{5}\) are located in Group 17, known as halogens. (b) Elements with three unpaired p electrons (\(np^{3}\)) are located in Group 15, known as the nitrogen group or pnictogens. (c) An element with valence electrons \(4s^{2} 4p^{1}\) is Gallium (Ga), which is in Period 4 and Group 13. (d) The d-block elements are located in the center of the periodic table and comprise Groups 3 through 12, including Transition Metals.

Step by step solution

01

(a) Valence-shell electron configuration of \(n s^{2}np^{5}\) elements

To locate elements with this valence-shell electron configuration, remember that elements in the periodic table are arranged in periods and groups. A period is denoted by the principal quantum number n, and groups represent elements that have similar electron configurations. Elements with the electron configuration \(ns^{2}np^{5}\) belong to Group 17, known as halogens.
02

(b) Elements with three unpaired p electrons

Having three unpaired p electrons means that the element's electron configuration in the p orbital is \(np^{3}\). These elements are located in Group 15 of the periodic table, known as the nitrogen group or pnictogens.
03

(c) Valence electrons are \(4s^{2} 4p^{1}\)

To determine the element with these valence electrons, consider both the period and the group it belongs to. Here, the principal quantum number n is 4, indicating that the element is in Period 4. Also, its electron configuration indicates that it belongs to Group 13. Consequently, the element is Gallium (Ga).
04

(d) The d-block elements

The d-block elements are located in the center of the periodic table and comprise Groups 3 through 12, including Transition Metals. In these elements, d orbitals are progressively filled from left to right across the block.

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Most popular questions from this chapter

(a) What is the frequency of radiation whose wavelength is \(5.0 \times 10^{-5} \mathrm{~m} ?\) (b) What is the wavelength of radiation that has a frequency of \(2.5 \times 10^{8} \mathrm{~s}^{-1} ?(\mathrm{c})\) Would the radiations in part (a) or part (b) be detected by an X-ray detector? (d) What distance does electromagnetic radiation travel in \(10.5 \mathrm{fs}\) ?

Microwave ovens use microwave radiation to heat food. The energy of the microwaves is absorbed by water molecules in food and then transferred to other components of the food. (a) Suppose that the microwave radiation has a wavelength of \(11.2 \mathrm{~cm} .\) How many photons are required to heat \(200 \mathrm{~mL}\) of coffee from \(23^{\circ} \mathrm{C}\) to \(60^{\circ} \mathrm{C} ?\) (b) Suppose the microwave's power is \(900 \mathrm{~W}\) ( 1 Watt \(=1\) joule-second). How long would you have to heat the coffee in part (a)?

The electron microscope has been widely used to obtain highly magnified images of biological and other types of materials. When an electron is accelerated through a particular potential field, it attains a speed of \(8.95 \times 10^{6} \mathrm{~m} / \mathrm{s}\). What is the characteristic wavelength of this electron? Is the wavelength comparable to the size of atoms?

(a) Calculate the energies of an electron in the hydrogen atom for \(n=1\) and for \(n=\infty .\) How much energy does it require to move the electron out of the atom completely (from \(n=1\) to \(n=\infty),\) according to Bohr? Put your answer in \(\mathrm{kJ} / \mathrm{mol}\). (b) The energy for the process \(\mathrm{H}+\) energy \(\rightarrow \mathrm{H}^{+}+\mathrm{e}^{-}\) is called the ionization energy of hydrogen. The experimentally determined value for the ionization energy of hydrogen is \(1310 \mathrm{~kJ} / \mathrm{mol}\). How does this compare to your calculation?

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 \(0.529 \AA,(\mathrm{c})\) from the \(n=6\) to the \(n=9\) state.
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