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Chapter 8: Problem 24

Does the octet rule mean that a diatomic molecule must have 16 valence electrons?

Short Answer

Expert verified
No, the octet rule does not imply that a diatomic molecule must have 16 valence electrons. The rule states that atoms are most stable when they have a full valence shell of eight electrons. It requires that each atom in the diatomic molecule achieves a stable electron configuration by potentially sharing electrons with the other atom in the bond. The total number of valence electrons in the diatomic molecule may not necessarily be 16 and can vary, as demonstrated by examples such as hydrogen molecules (H2) and nitrogen molecules (N2).

Step by step solution

01

Understanding the octet rule

The octet rule states that atoms are most stable when they have a full valence shell of eight electrons, which usually means having eight electrons in their outermost energy level. This rule is based on the fact that atoms in molecules tend to have the same electron configuration as noble gases, which are known to be very stable.
02

Applying the octet rule to diatomic molecules

A diatomic molecule consists of two atoms bonded together. In order to satisfy the octet rule, each atom in the diatomic molecule might try to achieve a stable configuration by sharing electrons with the other atom in the bond. The total number of valence electrons in a diatomic molecule is the sum of the valence electrons of the two individual atoms.
03

Analyzing if the octet rule requires 16 valence electrons in a diatomic molecule

The octet rule does not explicitly state that a diatomic molecule must have 16 valence electrons. It simply requires that each atom in the molecule have a stable electron configuration with a full valence shell of eight electrons. This might be achieved through sharing electrons with the other atom in the bond, but it does not mean that the diatomic molecule itself must have 16 valence electrons.
04

Counterexamples to having 16 valence electrons

There are several examples of diatomic molecules that do not have 16 valence electrons but still follow the octet rule. For example, in a hydrogen molecule (H2), each hydrogen atom has one valence electron, and they share these electrons forming a covalent bond, satisfying the octet rule as both hydrogen atoms achieve the stable electron configuration of helium, which has two electrons in its only shell. Similarly, a nitrogen molecule (N2) has a total of 10 valence electrons (5 from each nitrogen atom), and each nitrogen atom shares three electrons with the other nitrogen atom, forming a triple bond. Both nitrogen atoms achieve a full octet by sharing these electrons, even though the total number of valence electrons in the molecule is not 16.
05

Conclusion

The octet rule does not mean that a diatomic molecule must have 16 valence electrons. Instead, it requires that each atom in the diatomic molecule have a stable electron configuration with a full valence shell of eight electrons. This can be achieved through sharing electrons with the other atom in the bond, and the total number of valence electrons in the diatomic molecule may not necessarily be 16.

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Key Concepts

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

Valence Electrons
Valence electrons are the electrons in the outermost shell of an atom. These electrons play a key role in chemical bonding. They are the ones involved in forming chemical bonds with other atoms. Atoms are most stable when their valence shell is full.
For most elements, this means having eight valence electrons, satisfying the octet rule. However, hydrogen is an exception, as it is stable with just two valence electrons, mimicking the noble gas helium.
To predict how an atom will bond, one must know how many valence electrons it has:
  • Sulfur has six valence electrons, so it typically forms two covalent bonds to get a full octet.
  • Carbon has four valence electrons, allowing it to form four bonds.
Recognizing the number of valence electrons helps explain why atoms bond in specific ways and enables predictions about molecule formation.
Diatomic Molecules
A diatomic molecule consists of two atoms. These two atoms can be of the same element or different elements. Oxygen ( O_2 ) and hydrogen ( H_2 ) are common diatomic molecules composed of identical atoms, while hydrogen chloride ( HCl ) is made of different elements.
In diatomic molecules, each atom attempts to achieve a full valence shell by sharing electrons. This sharing results in each atom achieving its octet, leading to a more stable configuration.
  • For example, nitrogen ( N_2 ) consists of two nitrogen atoms each sharing three electrons, forming a strong triple bond.
  • In water vapor, ( H_2 ), each hydrogen atom shares its single electron with the oxygen atom, which has six valence electrons, to complete its octet.
Thus, not all diatomic molecules require 16 total valence electrons. Instead, they follow the octet rule, ensuring each atom achieves a filled valence shell through sharing.
Covalent Bonds
Covalent bonds form when two atoms share pairs of valence electrons. Sharing allows each participating atom to attain a stable electron configuration, often resembling the nearest noble gas.
With covalent bonding, the focus is on sharing to achieve stability:
  • Single bonds involve one pair of shared electrons. An example is hydrogen gas ( H_2 ), where each hydrogen shares its electron with the other.
  • Double bonds involve two pairs of shared electrons, as seen in oxygen ( O_2 ), where the atoms share four electrons.
  • Triple bonds involve three pairs of shared electrons, like in nitrogen ( N_2 ).
By understanding covalent bonds, students grasp how atoms can fill their valence shells by electron sharing, rather than by taking or donating, which is typical of ionic bonds. This mutual sharing makes the chemical bond significant and leads to the formation of stable molecular structures.

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Most popular questions from this chapter

Are these two skeletal structures resonance forms: \(\mathrm{X}-\mathrm{X}-\mathrm{O}\) and \(\mathrm{X}-\mathrm{O}-\mathrm{X} ?\) Explain.

Spectroscopic analysis of the linear molecule \(\mathrm{N}_{4} \mathrm{O}\) reveals that the nitrogen-oxygen bond length is \(135 \mathrm{pm}\) and that there are three nitrogen-nitrogen bond lengths: 148,127 and \(115 \mathrm{pm} .\) Draw the Lewis structure for \(\mathrm{N}_{4} \mathrm{O}\) consistent with these observations.

Use formal charges to determine which resonance form of each of the following ions is preferred: CNO"; NCO"; \(\mathrm{CON}^{-}\).

Why is the oxygen-oxygen bond length in \(\mathrm{O}_{3}\) not the same as in \(\mathrm{O}_{2} ?\)

Explain on the basis of atomic structure why trends in electronegativity are related to trends in atomic size.
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