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Chapter 7: Problem 93

A certain oxygen atom has the electron configuration \(1 s^{2} 2 s^{2} 2 p_{x}^{2} 2 p_{y}^{2}\). How many unpaired electrons are present? Is this an excited state of oxygen? In going from this state to the ground state would energy be released or absorbed?

Short Answer

Expert verified
The given oxygen atom has \(0\) unpaired electrons, is in an excited state, and energy will be released when it returns to the ground state.

Step by step solution

01

Identify the Oxygen Atom's Electron Configuration

The given electron configuration of the oxygen atom is \(1s^2 2s^2 2p_x^2 2p_y^2\). This notation represents the orbital filling of the electrons.
02

Determine the Number of Unpaired Electrons

In the electron configuration, 1s and 2s orbitals are fully occupied by two electrons each, and both 2px and 2py orbitals have two electrons each. All electrons are paired up, meaning there are \(0\) unpaired electrons.
03

Compare the Given Electron Configuration to the Ground State Configuration of Oxygen

The electron configuration of an oxygen atom in its ground state is given by \(1s^2 2s^2 2p^4\), which is the same as saying \(1s^2 2s^2 2p_x^2 2p_y^1 2p_z^1\). Comparing the ground state configuration to the given configuration, we can see differences in the filling of 2py and 2pz orbitals with one less electron in 2py and one more electron in 2pz.
04

Determine if the Atom is in an Excited State

As the given electron configuration differs from the ground state configuration, we can conclude that the oxygen atom is in an excited state.
05

Determine if Energy is Released or Absorbed in Returning to the Ground State

When an atom transitions from an excited state to the ground state, the excess energy stored in the excited state is released as energy, in various forms such as light, heat, or other rays. Hence, energy is released when the oxygen atom transitions from this excited state to its ground state. In conclusion, the given oxygen atom has 0 unpaired electrons, is in an excited state, and energy will be released when it returns to the ground state.

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Most popular questions from this chapter

Order the atoms in each of the following sets from the least exothermic electron affinity to the most. a. \(\mathrm{N}, \mathrm{O}, \mathrm{F}\) b. \(\mathrm{Al}, \mathrm{Si}, \mathrm{P}\)

Using only the periodic table inside the front cover of the text, write the expected ground-state electron configurations for a. the third element in Group \(5 \mathrm{~A}\). b. element number 116 . c. an element with three unpaired \(5 d\) electrons. d. the halogen with electrons in the \(6 p\) atomic orbitals.

Calculate the wavelength of light emitted when each of the following transitions occur in the hydrogen atom. What type of electromagnetic radiation is emitted in each transition? a. \(n=3 \rightarrow n=2\) b. \(n=4 \rightarrow n=2\) c. \(n=2 \rightarrow n=1\)

How many orbitals in an atom can have the designation \(5 p, 3 d_{z^{2}}\), \(4 d, n=5, n=4 ?\)

How many valence electrons do each of the following elements have, and what are the specific valence electrons for each element? a. \(\mathrm{Ca}\) b. \(\mathrm{O}\) c. element 117 d. In e. Ar f. \(\mathrm{Bi}\)
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