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Chapter 7: Problem 94

Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. a. \(1 s^{2} 2 s^{2} 3 p^{1}\) b. \(1 s^{2} 2 s^{2} 2 p^{6}\) c. \(1 s^{2} 2 s^{2} 2 p^{4} 3 s^{1}\) d. \([\mathrm{Ar}] 4 s^{2} 3 d^{5} 4 p^{1}\) How many unpaired electrons are present in each of these species?

Short Answer

Expert verified
The excited-state configurations are for Boron (\(1s^2 2s^2 3p^1\)), Fluorine (\(1s^2 2s^2 2p^4 3s^1\)), and Iron (\([\text{Ar}] 4s^2 3d^5 4p^1\)), with 1, 2, and 6 unpaired electrons, respectively. The ground-state configuration is for Neon (\(1s^2 2s^2 2p^6\)), which has no unpaired electrons.

Step by step solution

01

Determine Atomic Number

For each electron configuration, count the total number of electrons present. It will be the atomic number of the atom. a. \(1s^2 2s^2 3p^1\): 5 electrons b. \(1s^2 2s^2 2p^6\): 10 electrons c. \(1s^2 2s^2 2p^4 3s^1\): 9 electrons d. \([\text{Ar}] 4s^2 3d^5 4p^1\): 18 (from Ar) + 8 = 26 electrons
02

Identify the Elements

Identify the elements using the atomic numbers found in step 1 by referring to the periodic table. a. 5 electrons: Boron (B) b. 10 electrons: Neon (Ne) c. 9 electrons: Fluorine (F) d. 26 electrons: Iron (Fe)
03

Determine Ground-state or Excited-state Configurations

Compare the given electron configurations with the ground-state configurations according to the Aufbau principle. a. Boron ground-state configuration: \(1s^2 2s^2 2p^1\) (given configuration is in excited state) b. Neon ground-state configuration: \(1s^2 2s^2 2p^6\) (given configuration is in ground state) c. Fluorine ground-state configuration: \(1s^2 2s^2 2p^5\) (given configuration is in excited state) d. Iron ground-state configuration: \([\text{Ar}] 4s^2 3d^6\) (given configuration is in excited state)
04

Count Unpaired Electrons

Count the number of unpaired electrons in each electron configuration. a. Excited Boron: 1 unpaired electron (in 3p) b. Ground-state Neon: 0 unpaired electrons c. Excited Fluorine: 2 unpaired electrons (1 in 2p and 1 in 3s) d. Excited Iron: 6 unpaired electrons (2 in 4s, 5 in 3d, and 1 in 4p) In conclusion, the excited-state configurations are for Boron, Fluorine, and Iron, with 1, 2, and 6 unpaired electrons, respectively. The ground-state configuration is for Neon, which has no unpaired electrons.

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Most popular questions from this chapter

Consider the following ionization energies for aluminum: $$ \begin{aligned} \mathrm{Al}(g) \longrightarrow \mathrm{Al}^{+}(g)+\mathrm{e}^{-} & I_{1}=580 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{Al}^{+}(g) \longrightarrow \mathrm{Al}^{2+}(g)+\mathrm{e}^{-} & I_{2}=1815 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ $$ \begin{array}{ll} \mathrm{Al}^{2+}(g) \longrightarrow \mathrm{Al}^{3+}(g)+\mathrm{e}^{-} & I_{3}=2740 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{Al}^{3+}(g) \longrightarrow \mathrm{Al}^{4+}(g)+\mathrm{e}^{-} & I_{4}=11,600 \mathrm{~kJ} / \mathrm{mol} \end{array} $$ a. Account for the trend in the values of the ionization energies. b. Explain the large increase between \(I_{3}\) and \(I_{4}\). c. Which one of the four ions has the greatest electron affinity? Explain. d. List the four aluminum ions given in order of increasing size, and explain your ordering. (Hint: Remember that most of the size of an atom or ion is due to its electrons.)

An excited hydrogen atom emits light with a wavelength of \(397.2 \mathrm{~nm}\) to reach the energy level for which \(n=2\). In which principal quantum level did the electron begin?

Three elements have the electron configurations \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}\), \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}\), and \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}\). The first ionization energies of these elements (not in the same order) are \(0.419,0.735\), and \(1.527 \mathrm{MJ} / \mathrm{mol}\). The atomic radii are \(1.60,0.98\), and \(2.35 \AA\). Identify the three elements, and match the appropriate values of ionization energy and atomic radius to each configuration.

Octyl methoxycinnamate and oxybenzone are common ingredients in sunscreen applications. These compounds work by absorbing ultraviolet (UV) B light (wavelength \(280-320 \mathrm{~nm}\) ), the UV light most associated with sunburn symptoms. What frequency range of light do these compounds absorb?

Assume that a hydrogen atom's electron has been excited to the \(n=5\) level. How many different wavelengths of light can be emitted as this excited atom loses energy?
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