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Chapter 7: Problem 159

Identify the following three elements. a. The ground-state electron configuration is \([\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{4}\). b. The ground-state electron configuration is \([\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{2} .\) c. An excited state of this element has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{4} 3 s^{1}\).

Short Answer

Expert verified
The elements corresponding to the given electron configurations are: a. Tellurium (Te) with the ground-state electron configuration \([\mathrm{Kr}] 5s^2 4d^{10} 5p^4\). b. Germanium (Ge) with the ground-state electron configuration \([\mathrm{Ar}] 4s^2 3d^{10} 4p^2\). c. Fluorine (F) in an excited state with the electron configuration \(1s^2 2s^2 2p^4 3s^1\).

Step by step solution

01

Calculate the atomic number of each element

For each given configuration, we will count the total number of electrons. a. \([\mathrm{Kr}] 5s^2 4d^{10} 5p^4\) b. \([\mathrm{Ar}] 4s^2 3d^{10} 4p^2\) c. Excited State: \(1s^2 2s^2 2p^4 3s^1\)
02

Identify the elements corresponding to the atomic numbers

Match the calculated atomic numbers to their corresponding elements on the periodic table. a. The ground-state electron configuration is \([\mathrm{Kr}] 5s^2 4d^{10} 5p^4\): The total number of electrons is \(36+2+10+4=52\). The element with the atomic number of 52 is Tellurium (Te). b. The ground-state electron configuration is \([\mathrm{Ar}] 4s^2 3d^{10} 4p^2\): The total number of electrons is \(18+2+10+2=32\). The element with the atomic number of 32 is Germanium (Ge). c. An excited state of this element has the electron configuration \(1s^2 2s^2 2p^4 3s^1\): The total number of electrons is \(2+2+4+1=9\). The element with the atomic number of 9 is Fluorine (F). Note that this configuration is an excited state, meaning that at least one electron has moved to a higher energy level temporarily. Answers: a. Tellurium (Te) b. Germanium (Ge) c. Fluorine (F) in an excited state

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Atomic Number
The atomic number is a fundamental property of an element and it indicates the number of protons found in the nucleus of an atom. Since atoms are electrically neutral, this number also reflects the number of electrons orbiting the nucleus under normal circumstances.

For example, the atomic number of Tellurium (Te) is 52, which means it has 52 protons and, when in the ground state, an equal number of electrons. Atomic numbers are sequential and are assigned based on increasing number of protons in the elements, making it a unique identifier for each element.
Periodic Table
The periodic table is an organized chart of elements, arrayed by increasing atomic number, electron configurations, and recurring chemical properties. Elements are placed in specific rows (periods) and columns (groups) which are indicative of the element's electron configuration and the behavior of its electrons.

Different blocks within the periodic table (s, p, d, and f) correspond to the highest energy level of electron orbitals that are being filled. For instance, Germanium (Ge) resides in the p-block, period 4 of the table, which correlates with its valence electron configuration of \(4s^2 3d^{10} 4p^2\).
Ground-State Configuration
Ground-state configuration of an element refers to the most stable, low energy arrangement of electrons in an atom when it is not excited. This configuration can be predicted using principles like the Aufbau principle, Pauli exclusion principle, and Hund's rule.

The ground-state electron configurations provided in the exercise for Tellurium is \(\left[\mathrm{Kr}\right] 5s^2 4d^{10} 5p^4\), and for Germanium is \(\left[\mathrm{Ar}\right] 4s^2 3d^{10} 4p^2\). In these notations, the part in brackets, \(\left[\mathrm{Kr}\right]\) and \(\left[\mathrm{Ar}\right]\), represents the electron configuration of the noble gas from the previous period, signifying a stable electron configuration that the elements鈥� electrons are building upon.
Excited State
An excited state occurs when one or more electrons in an atom absorb energy and move to a higher energy orbital, which is not the case in ground-state configurations. These excited configurations are usually unstable and the excited electrons will eventually return to their ground-state configurations, releasing energy in the process.

In the exercise, Fluorine (F) \(1s^2 2s^2 2p^4 3s^1\) is in an excited state because one electron has moved to a 3s orbital, which is a higher energy level than expected for its ground-state. The ground-state configuration for Fluorine would be \(1s^2 2s^2 2p^5\), without the \(3s^1\) electron.

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Most popular questions from this chapter

For each of the following pairs of elements \(\begin{array}{ll}(\mathrm{Mg} \text { and } \mathrm{K}) & (\mathrm{F} \text { and } \mathrm{Cl})\end{array}\) pick the atom with a. more favorable (exothermic) electron affinity. b. higher ionization energy. c. larger size.

An ion having a \(4+\) charge and a mass of \(49.9\) amu has 2 electrons with principal quantum number \(n=1,8\) electrons with \(n=2\), and 10 electrons with \(n=3\). Supply as many of the properties for the ion as possible from the information given. (Hint: In forming ions for this species, the \(4 s\) electrons are lost before the \(3 d\) electrons.) a. the atomic number b. total number of \(s\) electrons c. total number of \(p\) electrons d. total number of \(d\) electrons e. the number of neutrons in the nucleus f. the ground-state electron configuration of the neutral atom

Give the maximum number of electrons in an atom that can have these quantum numbers: a. \(n=4\) b. \(n=5, m_{\ell}=+1\) c. \(n=5, m_{s}=+\frac{1}{2}\) d. \(n=3, \ell=2\) e. \(n=2, \ell=1\)

Photogray lenses incorporate small amounts of silver chloride in the glass of the lens. When light hits the \(\mathrm{AgCl}\) particles, the following reaction occurs: $$ \mathrm{AgCl} \stackrel{\mathrm{hv}}{\longrightarrow} \mathrm{Ag}+\mathrm{Cl} $$ The silver metal that is formed causes the lenses to darken. The enthalpy change for this reaction is \(3.10 \times 10^{2} \mathrm{~kJ} / \mathrm{mol}\). Assuming all this energy must be supplied by light, what is the maximum wavelength of light that can cause this reaction?

It takes \(476 \mathrm{~kJ}\) to remove 1 mole of electrons from the atoms at the surface of a solid metal. How much energy (in kJ) does it take to remove a single electron from an atom at the surface of this solid metal?
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