/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 24 Does the octet rule mean that a ... [FREE SOLUTION] | 魅影直播

魅影直播

Log out

Learning Materials

Features

Discover

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.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 魅影直播!

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.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

When left at room temperature, mixtures of \(\mathrm{BF}_{3}\) and \(\mathrm{BCl}_{3}\) are found to contain significant amounts of \(\mathrm{BF}_{2} \mathrm{Cl}\) and BFCl \(_{2} .\) Using Lewis structures, explain the origin of the latter two compounds..

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

What structural features do all the resonance forms of a molecule or ion have in common?

Does the number of valence electrons in a neutral atom ever equal the atomic number?

How do the electronegativities of the elements change across a period and down a group?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.