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Chapter 29: Problem 15

Write out the electron configuration \(\left(1 s^{2} 2 s^{2},\right.\) and so on \()\) for \(\mathrm{Ne}\) Ar, and Kr. (b) How many electrons does each of these atoms have in its outer shell? (c) Predict the chemical behavior of these three atoms. Explain your reasoning.

Short Answer

Expert verified
Ne, Ar, and Kr are noble gases with full outer shells (8 electrons) and show low reactivity due to their stable electron configurations.

Step by step solution

01

Understand the Problem

We need to write the electron configurations for Ne (Neon), Ar (Argon), and Kr (Krypton). After that, we determine how many electrons are in each atom鈥檚 outer shell (valence electrons), and finally, predict their chemical behavior.
02

Write Electron Configuration for Neon

Neon (Ne) has an atomic number of 10, which means it has 10 electrons. The electron configuration is constructed starting from the lowest energy level. We fill the 1s orbital with 2 electrons, then the 2s orbital with 2 electrons, and lastly, the 2p orbital with the remaining 6 electrons: \[ 1s^2 \, 2s^2 \, 2p^6 \]
03

Write Electron Configuration for Argon

Argon (Ar) has an atomic number of 18, implying it has 18 electrons. The electron configuration starts filling the 1s orbital, then 2s, 2p, 3s, and 3p orbitals: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \]
04

Write Electron Configuration for Krypton

Krypton (Kr) has an atomic number of 36. Its electron configuration involves filling up to 4p: \[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^6 \]
05

Determine Valence Electrons

The outer shell (valence shell) corresponds to the highest energy level. For Ne: 2p (8 electrons), for Ar: 3p (8 electrons), and for Kr: 4p (8 electrons). Thus, each atom has 8 electrons in its outer shell.
06

Predict Chemical Behavior

Ne, Ar, and Kr all have full valence shells (8 electrons) and belong to the group of noble gases. This makes them very stable and unreactive under normal conditions, as they do not seek to gain or lose electrons to achieve a full outer shell, unlike other elements.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Noble Gases
Noble gases are a special group of elements found in Group 18 of the periodic table. They include elements such as Neon (Ne), Argon (Ar), and Krypton (Kr).
These gases are unique because they have a complete set of electrons in their outermost shell. This full shell makes them very stable, as they don't need to gain or lose electrons, a typical behavior seen in other elements to achieve stability.
Their lack of reactivity is why they are termed "noble," as in "noble" or "inert."
Understanding noble gases is crucial because they set a benchmark for what most atoms attempt to achieve through chemical reactions鈥攕tability through a full valence shell.
Valence Electrons
Valence electrons are the electrons located in the outermost shell of an atom. They play a vital role in an atom's chemical properties and its ability to form bonds with other atoms.
Neon, Argon, and Krypton each have 8 valence electrons, filling their outermost energy level completely.
  • Neon's valence electrons are in the 2p orbital.
  • Argon's valence electrons are in the 3p orbital.
  • Krypton's valence electrons are in the 4p orbital.
These electrons determine the reactivity of an element. Since noble gases have full outer shells, their valence electrons are pleased, and they don't participate in bonding or reactions readily.
Atomic Structure
Atomic structure refers to the arrangement of electrons around the nucleus of an atom. Electrons occupy energy levels or shells, around the nucleus, and each level can hold a specific number of electrons.
In noble gases like Ne, Ar, and Kr, electron configurations are built by filling lower energy levels first. This process results in:
  • Neon: \[ 1s^2 \, 2s^2 \, 2p^6 \]
  • Argon:\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \]
  • Krypton:\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^6 \]
These configurations show how filled each outer shell is, which is crucial in determining the atoms' stability and reactivity.
Chemical Stability
Chemical stability of an element relates to its electronic configuration. When an element's outermost shell is filled with electrons, it is considered stable. It has little tendency to engage in chemical reactions.
For noble gases like Ne, Ar, and Kr, having 8 electrons in their valence shell means they are exceptionally stable.
  • This stability is why they are commonly found in their elemental form rather than in compounds.
  • Their full shells secure them against the usual electron loss or gain seen in active elements.
This natural resistance to change or react influences the way we use noble gases in technology, such as neon lights and argon welding, where their inertness is a significant advantage.

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Most popular questions from this chapter

The dissociation energy of the hydrogen molecule (i.e., the energy required to separate the two atoms) is \(4.48 \mathrm{eV}\). In the gas phase (treated as an ideal gas), at what temperature is the average translational kinetic energy of a molecule equal to this energy?

An ionic bond. (a) Calculate the electric potential energy for a \(\mathrm{K}^{+}\) ion and a \(\mathrm{Br}^{-}\) ion separated by a distance of \(0.29 \mathrm{nm}\), the equilibrium separation in the KBr molecule. Treat the ions as point charges. (b) What is the ratio of this energy to the ionization energy of the hydrogen atom?

Atoms of unusual size. In photosynthesis in plants, light is absorbed in light-harvesting complexes consisting of protein and pigment molecules. The energy absorbed is then transported to a specialized complex called the reaction center. Scientists believe that quantum mechanical effects may play an important role in this energy transfer. In a recent experiment, researchers used rubidium atoms cooled to a very low temperature to study a similar energy-transfer process in the laboratory. Laser light was used to excite an electron in each atom to a very highly excited state (large \(n\) ). The excited electron behaves very much like the single electron in a hydrogen atom, with an effective \(Z=1,\) but because \(n\) is so large, the excited electron is quite far from the atomic nucleus, with an orbital radius of approximately \(1 \mu \mathrm{m},\) and is weakly bound. Using these so-called Rydberg atoms, the researchers were able to study how energy is transported from one atom to the next in a process that may be a helpful model in understanding energy transport in photosynthesis. How many different possible electron states are there in the \(n=100, l=2\) subshell? A. 2 B. 100 C. 10,000 D. 10

(a) Write out the ground-state electron configuration \(\left(1 s^{2} 2 s^{2},\right.\) and so on) for the carbon atom. (b) What element of next-larger \(Z\) has chemical properties similar to those of carbon? (See Example 29.3.) Give the ground-state electron configuration for this element.

The \(z\) component of the angular momentum of an atom, \(L_{z}\), is measured as a function of the angle that the angular momentum vector \(\vec{L}\) makes with the positive \(z\) axis, \(\theta .\) The resulting data are given in the table, where the angular momentum is measured in units of \(\hbar\). $$ \begin{array}{cc} \hline \boldsymbol{\theta}\left({ }^{\circ}\right) & \boldsymbol{L}_{z}(\hbar) \\\ \hline 63.7 & 1.97 \\ 79.2 & 1.05 \\ 90.4 & -0.03 \\ 102 & -0.95 \\ 118 & -2.02 \\ \hline \end{array} $$ Make a plot of \(L_{z}\) as a function of \(\cos \theta\). Using a linear "best fit" to the data, determine (a) the magnitude of the angular momentum vector in units of \(\hbar\) and (b) the corresponding angular momentum quantum number.
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