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Chapter 6: Problem 71

Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (a) \(1 s^{2} 2 s^{2},\) (b) \(1 s^{2} 2 s^{2} 2 p^{4}\), (c) \([\mathrm{Ar}] 4 s^{1} 3 d^{5}\) (d) \([\mathrm{Kr}] 5 s^{2} 4 d^{10} 5 p^{4}\).

Short Answer

Expert verified
(a) Beryllium (Be) has 0 unpaired electrons. (b) Oxygen (O) has 2 unpaired electrons. (c) Chromium (Cr) has 6 unpaired electrons. (d) Tellurium (Te) has 2 unpaired electrons.

Step by step solution

01

Determine the total number of electrons

Count the total number of electrons in the given configuration (a) \(1s^2 2s^2\). There are 2 electrons in the first shell (1s) and 2 electrons in the second shell (2s). So, the total number of electrons is 4.
02

Identify the element

With 4 electrons, the element has an atomic number of 4. Using the periodic table, we can see that this corresponds to the element Beryllium (Be). #Step 2: Determine the number of unpaired electrons in configuration (a)#
03

Check for unpaired electrons in each subshell

Both 1s and 2s subshells are full, with no capacity for additional electrons, so there are 0 unpaired electrons in this configuration. #Step 3: Repeat the process for the electron configuration (b)#
04

Electron configuration (b)

Count the total electrons in the configuration (b) \(1s^2 2s^2 2p^4\). There are 2 electrons in the 1s shell/1s-subshell, 2 electrons in the 2s-subshell, and 4 electrons in the 2p-subshell. There are a total of 8 electrons, so the element corresponding to this configuration is Oxygen (O). For unpaired electrons, as 2p has 4 electrons, 2 are paired and the other 2 are unpaired. #Step 4: Repeat the process for electron configuration (c)#
05

Electron configuration (c)

The given configuration (c) is [\(\mathrm{Ar}\)] \(4s^1 3d^5\). As Ar (Argon) has 18 electrons, the element now has a total of 18 (Ar) + 1 (4s) + 5 (3d) = 24 electrons. The element with 24 electrons is Chromium (Cr). In this configuration, the 4s subshell has 1 unpaired electron, and the 3d subshell has 5 unpaired electrons, making a total of 6 unpaired electrons. #Step 5: Repeat the process for electron configuration (d)#
06

Electron configuration (d)

The given configuration (d) is [\(\mathrm{Kr}\)] \(5s^2 4d^{10} 5p^4\). As Kr (Krypton) has 36 electrons, the element now has a total of 36 (Kr) + 2 (5s) + 10 (4d) + 4 (5p) = 52 electrons. The element with 52 electrons is Tellurium (Te). In this configuration, the 5p subshell has 4 electrons, with 2 being paired and the other 2 unpaired. The rest of the subshells are full, leaving a total of 2 unpaired electrons. #Solution# Here are the results for each electron configuration: (a) Element: Beryllium (Be) - Unpaired electrons: 0 (b) Element: Oxygen (O) - Unpaired electrons: 2 (c) Element: Chromium (Cr) - Unpaired electrons: 6 (d) Element: Tellurium (Te) - Unpaired electrons: 2

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