Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 106

What is the octet rule, and what is the justification behind it?

Short Answer

Expert verified
The octet rule states that atoms tend to combine in such a way that they each have eight electrons in their valence shell, resulting in a more stable electron configuration through ionic or covalent bonds. This rule is justified by the increased stability provided by having a full outer shell, corresponding to the electron configuration of a noble gas that is unreactive. Atoms achieve this stable configuration through ionic and covalent bonding, donating, accepting, or sharing electrons with other atoms to meet the octet rule. Examples include the formation of NaCl and H2O, demonstrating the importance of the octet rule in predicting and explaining chemical behavior.

Step by step solution

01

Definition of the Octet Rule

The octet rule is a chemical rule that states that atoms tend to combine in such a way that they each have eight electrons in their valence shell, which results in a more stable electron configuration. This is often achieved through the forming of ionic or covalent bonds.
02

Justification: Electron Stability

The justification behind the octet rule lies in the stability that it provides for the resulting chemical compounds. Atoms seek to have a stable electron configuration, and in most cases, this stability can be achieved by having eight electrons in their outer shell, corresponding to the electron configuration of a noble gas. These noble gases tend to be unreactive and have little tendency to gain or lose electrons, making them more stable.
03

Justification: Ionic and Covalent Bonds

Atoms strive to achieve an electron configuration of a noble gas by participating in chemical bonding - either ionic bonding or covalent bonding. In ionic bonding, atoms donate or accept electrons to/from other atoms to achieve a full outer shell. In covalent bonding, atoms share electron pairs with other atoms to achieve a stable electron configuration. Both types of bonding result in the formation of chemical compounds that obey the octet rule, thus providing the necessary stability.
04

Justification: Examples

Some examples of the octet rule in action include the formation of NaCl (sodium chloride), where sodium (Na) donates one electron to chlorine (Cl), and the two elements form an ionic bond. In the case of the covalent bond, H2O (water) is formed when oxygen (O) shares its electrons with two hydrogen (H) atoms. Overall, the octet rule is an essential principle in chemistry that helps predict and explain the behavior of atoms in the formation of stable chemical compounds.

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

Regarding primary quantum number \(n\), which representative elements have valence electrons with an \(n\) value that is three times the \(n\) value of lithium's valence electrons? What period are they in?

Electromagnetic radiation emitted by magnesium has a wavelength of \(285.2 \mathrm{~nm}\). (a) Is this radiation visible to the eye? (b) What is the energy of this radiation?

Identify the period 2 element that is described by the ionization data below. \(\mathrm{M}(\mathrm{g}) \rightarrow \mathrm{M}^{+} 1 \mathrm{e}^{-} \quad \mathrm{IE}(1)=1.40 \times 10^{3} \mathrm{~J} / \mathrm{mol}\) \(\mathrm{M}^{+}(\mathrm{g}) \rightarrow \mathrm{M}^{2+} 1 \mathrm{e}^{-} \mathrm{IE}(2)=2.86 \times 10^{3} \mathrm{~J} / \mathrm{mol}\) \(\mathrm{M}^{2+}(\mathrm{g}) \rightarrow \mathrm{M}^{3+} 1 \mathrm{e}^{-} \mathrm{IE}(3)=4.58 \times 10^{3} \mathrm{~J} / \mathrm{mol}\) \(\mathrm{M}^{3+}(\mathrm{g}) \rightarrow \mathrm{M}^{4+} 1 \mathrm{e}^{-} \mathrm{IE}(4)=7.48 \times 10^{3} \mathrm{~J} / \mathrm{mol}\) \(\mathrm{M}^{4+}(\mathrm{g}) \rightarrow \mathrm{M}^{5+} 1 \mathrm{e}^{-} \mathrm{IE}(5)=9.44 \times 10^{3} \mathrm{~J} / \mathrm{mol}\) \(\mathrm{M}^{5+}(\mathrm{g}) \rightarrow \mathrm{M}^{6+} 1 \mathrm{e}^{-} \mathrm{IE}(6)=5.33 \times 10^{4} \mathrm{~J} / \mathrm{mol}\) \(\mathrm{M}^{6+}(\mathrm{g}) \rightarrow \mathrm{M}^{7+} 1 \mathrm{e}^{-} \mathrm{IE}(7)=6.44 \times 10^{4} \mathrm{~J} / \mathrm{mol}\)

According to Bohr, what is so special about the valence shell of an atom?

According to Bohr's model, energy must be put into an atom to move an electron from a low-energy shell to a higher-energy shell. How do you calculate the amount of energy needed for the move?
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

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.

Sign-up for free