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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

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

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