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Chapter 3: Problem 82

Explain why argon does not form either (a) ionic bonds or (b) covalent bonds.

Short Answer

Expert verified
Argon does not form ionic or covalent bonds because it already has a stable, full valence shell.

Step by step solution

01

Understanding Argon's Electron Configuration

Argon is a noble gas with the atomic number 18. Its electron configuration is \(1s^2 2s^2 2p^6 3s^2 3p^6\), showing that argon has a full outer shell with 8 electrons in its valence shell. This full valence shell makes argon chemically inert.
02

Exploring Ionic Bond Formation

Ionic bonds are formed when atoms transfer electrons to achieve a full valence shell, typically between metals and non-metals. Since argon already has a full valence shell, it neither needs to lose nor gain electrons. Thus, it does not have a tendency to form ionic bonds.
03

Examining Covalent Bond Formation

Covalent bonds involve the sharing of electrons between atoms to achieve full valence shells. Argon already has a complete set of 8 electrons in its outer shell, so it does not need to share electrons with other atoms to achieve stability. As a result, argon does not form covalent bonds.

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Key Concepts

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

Electron Configuration
Electron configuration describes how electrons are distributed in an atom's orbitals. For argon, this configuration is written as \(1s^2 2s^2 2p^6 3s^2 3p^6\). This notation indicates that argon has a total of 18 electrons arranged into specific energy levels and orbitals. The outermost shell, which is also known as the valence shell, contains 8 electrons for argon.
  • The valence shell is crucial for chemical bonding as it determines an atom's ability to bind with other atoms.
  • For noble gases like argon, having a full outer shell (octet) means that they are highly stable and do not readily react with other elements.
Understanding electron configuration is key to grasping why argon and other noble gases exhibit non-reactive behavior.
Ionic Bonds
Ionic bonds are formed through the transfer of electrons between atoms, typically between metals and nonmetals. This transfer occurs so that both atoms involved can achieve a full valence shell, known as the octet rule.
  • In an ionic bond, one atom donates electrons to another atom, leading to the creation of ions: one positively charged (cation) and one negatively charged (anion).
  • This results in a strong electrostatic attraction between the oppositely charged ions, forming the ionic bond.
Argon does not form ionic bonds because it already possesses a complete valence shell. With all its orbitals in the outer shell filled, argon neither needs to accept nor donate electrons to achieve stability, thus showing no tendency to form such bonds.
Covalent Bonds
Covalent bonds involve the sharing of electrons between atoms to allow each participating atom to achieve a full outer electron shell. This type of bonding usually occurs between nonmetals.
  • Covalent bonds enable atoms to share their electrons in such a way that both achieve a complete outer shell, or satisfy the octet rule.
  • The shared electrons count towards the valence shell of each involved atom, helping them reach a stable electronic state.
Argon does not engage in covalent bonding because it naturally has a complete octet. This optimal electron arrangement means there is no need for argon to partake in sharing electrons, rendering it inert in the context of covalent bonding.
Chemical Inertness
Chemical inertness refers to an element's lack of reactivity with other substances. Noble gases, like argon, are excellent examples of chemically inert elements.
  • The full valence shells of noble gases make them stable and nonreactive.
  • This stability is due to the lack of available electrons for bonding, both through ionic or covalent means.
Argon's complete outer shell with eight electrons results in minimal chemical reactivity, making it one of the least likely elements to form bonds under normal conditions. This inherent inertness is why argon does not form ionic or covalent bonds easily, fulfilling its role as a noble gas.

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Most popular questions from this chapter

How many covalent bonds are normally formed by each element? (a) \(\mathrm{N}\) (b) \(\mathrm{F}\) (c) \(\mathrm{C}\) (d) \(\mathrm{Br}\) (e) \(\mathrm{O}\)

Ozone, \(\mathrm{O}_{3}\), is an unstable blue gas with a characteristic pungent odor. In an ozone molecule, the connectivity of the atoms is \(\mathrm{O}-\mathrm{O}-\mathrm{O}\) and both \(\mathrm{O}-\mathrm{O}\) bonds are equivalent. (a) How many valence electrons must be present in an acceptable Lewis structure for an ozone molecule? (b) Write two equivalent resonance contributing structures for ozone. Be certain to show any positive or negative charges that may be present in your contributing structures. By equivalent contributing structures, we mean that each has the same pattern of bonding. (c) Show by the use of curved arrows how the first of your contributing structures may be converted to the second. (d) Based on your contributing structures, predict the \(\mathrm{O}-\mathrm{O}-\mathrm{O}\) bond angle in ozone (e) Explain why the following is not an acceptable contributing structure for an ozone molecule:

(Chemical Connections \(3 \mathrm{B}\) ) What is a medical use of barium sulfate?

Write the formula for the most stable ion formed by each element. (a) Mg (b) F (c) A (d) S {e} K (f) Br

Complete the chart by writing formulas for the compounds formed: \(\mathrm{Br}^{-} \quad \mathrm{MnO}_{4}^{-} \quad \mathrm{O}^{2-} \quad \mathrm{NO}_{3}^{-} \quad \mathrm{SO}_{4}^{2-} \quad \mathrm{PO}_{4}^{3-} \quad \mathrm{OH}^{-}\) \(\mathbf{L i}^{+}\) \(\mathrm{Ca}^{2+}\) \(\mathrm{Co}^{3+}\) \(\mathrm{K}^{+}\) \(\mathrm{Cu}^{2}\)
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