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Chapter 7: Problem 106

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 electron configurations a, c, and d represent excited states. The respective atoms and ground-state configurations are: a) Boron (B) with 1\(s^{2} 2 s^{2} 2 p^{1}\), c) Fluorine (F) with 1\(s^{2} 2 s^{2} 2 p^{5}\), and d) Gallium (Ga) with \([\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{1}\). Configuration b represents a Neon (Ne) atom in the ground state. The number of unpaired electrons in each configuration is: a) 1, b) 0, c) 3, and d) 6.

Step by step solution

01

Ground state rules check:

Remember the three rules: -Aufbau principle: electrons occupy the lowest energy orbitals available -Pauli exclusion principle: no two electrons in the same atom can have the same four quantum numbers -Hund's rule: electrons will occupy orbitals with the same energy (degenerate orbitals) singly before pairing up Verify that the given electron configurations follow the rules above. **Step 2: Identify the atoms represented by each configuration and write the ground-state electron configuration if appropriate**
02

Identifying atoms:

Use the periodic table and electron configuration patterns to identify which atom corresponds to each given electron configuration. If any of the configurations don't correspond to a ground state, find the correct ground-state electron configuration. **Step 3: Calculate the number of unpaired electrons in each configuration**
03

Count unpaired electrons:

Count how many electrons remain unpaired (i.e., do not have a partner with an opposite spin) in each configuration. This will give us the number of unpaired electrons for each electron configuration specified. Now let's implement these steps for each given electron configuration: a. 1\(s^{2} 2 s^{2} 3 p^{1}\)
04

Excited or ground state:

This configuration does not follow the Aufbau principle since it skips the 2\(p\) subshell. It is an excited state.
05

Atom and ground-state configuration:

The ground-state configuration should be 1\(s^{2} 2 s^{2} 2 p^{1}\), which corresponds to the Boron (B) atom.
06

Unpaired electrons:

There is one unpaired electron in the 3\(p\) subshell. b. 1\(s^{2} 2 s^{2} 2 p^{6}\)
07

Excited or ground state:

This configuration follows all rules and is the ground state.
08

Atom and ground-state configuration:

The configuration corresponds to a Neon (Ne) atom in its ground state.
09

Unpaired electrons:

There are no unpaired electrons in this configuration. c. 1\(s^{2} 2 s^{2} 2 p^{4} 3 s^{1}\)
10

Excited or ground state:

This configuration does not follow the Aufbau principle since it skips the 2\(p\) subshell. It is an excited state.
11

Atom and ground-state configuration:

The ground-state configuration should be 1\(s^{2} 2 s^{2} 2 p^{5}\), which corresponds to the Fluorine (F) atom.
12

Unpaired electrons:

There are two unpaired electrons in the 2\(p\) subshell and one unpaired electron in the 3\(s\) subshell, making a total of three unpaired electrons. d. \([\mathrm{Ar}] 4 s^{2} 3 d^{5} 4 p^{1}\)
13

Excited or ground state:

This configuration does not follow the Aufbau principle since it skips the 3\(d^{10}\) subshell. It is an excited state.
14

Atom and ground-state configuration:

The ground-state configuration should be \([\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{1}\), which corresponds to the Gallium (Ga) atom.
15

Unpaired electrons:

There are five unpaired electrons in the 3\(d\) subshell and one unpaired electron in the 4\(p\) subshell, making a total of six unpaired electrons.

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