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Chapter 7: Problem 76

The ground-state electron configurations listed here are incorrect. Explain what mistakes have been made in each and write the correct electron configurations. Al: \(1 s^{2} 2 s^{2} 2 p^{4} 3 s^{2} 3 p^{3}\) \(\mathrm{B}: 1 s^{2} 2 s^{2} 2 p^{5}\) \(\mathrm{F}: 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6}\)

Short Answer

Expert verified
The correct electron configurations are: Aluminium: \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}\), Boron: \(1 s^{2} 2 s^{2} 2 p^{1}\), Fluorine: \(1 s^{2} 2 s^{2} 2 p^{6}\).

Step by step solution

01

Correcting the Configuration for Aluminium

For Aluminium (Al), it's given as \(1 s^{2} 2 s^{2} 2 p^{4} 3 s^{2} 3 p^{3}\). However, if you check the periodic table, you'll find that Aluminium has an atomic number of 13, which means it has 13 electrons. The given configuration adds up to \(2+2+4+2+3=13\) electrons. Therefore, the initial count is correct but the placement of the electrons in \(2 p^{4}\) is not accurate. The configuration should be \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}\) following the rule that p-orbitals can at maximum hold 6 electrons.
02

Correcting the Configuration for Boron

For Boron (B), the configuration provided is \(1 s^{2} 2 s^{2} 2 p^{5}\). Boron has an atomic number of 5 indicating 5 electrons. The given configuration adds up to 9 electrons which is incorrect. The correct electron configuration for Boron is \(1 s^{2} 2 s^{2} 2 p^{1}\).
03

Correcting the Configuration for Fluorine

Lastly, the presented configuration for Fluorine(F) is \(1 s^{2} 2 s^{2} 2 p^{6}\). Fluorine has an atomic number of 9 and the given configuration satisfies this with a total of \(2+2+5=9\) electrons. Therefore, the configuration for Fluorine is correct and no changes are required.

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Most popular questions from this chapter

Photodissociation of water \(\mathrm{H}_{2} \mathrm{O}(l)+h \nu \longrightarrow \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g)\) has been suggested as a source of hydrogen. The \(\Delta H_{\mathrm{xn}}^{\circ}\) for the reaction, calculated from thermochemical data, is \(285.8 \mathrm{~kJ}\) per mole of water decomposed. Calculate the maximum wavelength (in \(\mathrm{nm}\) ) that would provide the necessary energy. In principle, is it feasible to use sunlight as a source of energy for this process?

What are the inadequacies of Bohr's theory?

What is the maximum number of electrons in an atom that can have the following quantum numbers? Specify the orbitals in which the electrons would be found. (a) \(n=2, m_{\mathrm{s}}=+\frac{1}{2}\) (b) \(n=4, m_{e}=+1\) (c) \(n=3, \ell=2 ;\) (d) \(n=2, \ell=0, m_{\mathrm{s}}=-\frac{1}{2} ;\) (e) \(n=4\) \(\ell=3, m_{\ell}=-2\)

Calculate the energies needed to remove an electron from the \(n=1\) state and the \(n=5\) state in the \(\mathrm{Li}^{2+}\) ion. What is the wavelength (in \(\mathrm{nm}\) ) of the emitted photon in a transition from \(n=5\) to \(n=1 ?\) The Rydberg constant for hydrogen like ions is \((2.18 \times\) \(\left.10^{-18} \mathrm{~J}\right) Z^{2},\) where \(Z\) is the atomic number.

Describe the characteristics of the following groups of elements: transition metals, lanthanides, actinides.
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