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Chapter 6: Problem 65

Explain the octet rule. Why are hydrogen and helium exceptions to the octet rule?

Short Answer

Expert verified
The octet rule states that main-group element atoms tend to achieve a stable configuration with eight electrons in their outermost energy level through gaining, losing, or sharing electrons in chemical bonding. Hydrogen and helium are exceptions because they aim for a "duet" configuration, with only two electrons in their outermost energy level. This is because hydrogen can only accommodate two electrons in its 1s subshell, and helium already has a stable, full configuration with two electrons in its outermost energy level.

Step by step solution

01

Explaining the Octet Rule

The octet rule is a chemical rule of thumb that states that atoms of main-group elements tend to combine in such a way that they each have eight electrons in their valence shell, which is the outermost electron energy level. This gives the atom a stable configuration similar to that of a noble gas. Atoms can achieve an octet by losing, gaining, or sharing electrons through chemical bonding.
02

Hydrogen and the Octet Rule

Hydrogen is an exception to the octet rule because it only has one electron in its outermost energy level. The stable configuration for hydrogen is the same as that of the noble gas helium, with two electrons in its outermost energy level. Because hydrogen can only accommodate two electrons in its 1s subshell, it can only gain, lose, or share one electron to achieve stability. Thus, hydrogen will strive for a filled 1s subshell or a "duet" of electrons, which is not the same as the octet rule's eight-electron configuration.
03

Helium and the Octet Rule

Helium is another exception to the octet rule because it already has a stable, full configuration with two electrons in its outermost energy level. Since the first energy level can only hold two electrons, helium doesn't need to gain, lose, or share electrons. Its complete valence shell is referred to as a "duet" instead of an octet. Helium, being a noble gas, is unreactive with other elements due to its stable configuration.
04

Summary

In summary, the octet rule explains that atoms try to achieve a stable configuration with eight electrons in their outermost energy level, usually by gaining, losing, or sharing electrons in chemical bonding. Hydrogen and helium are exceptions because their stable configurations consist of two electrons in their outermost energy level, which is called a "duet" instead of an octet. These elements achieve stability with fewer electrons in their valence shells than what the octet rule suggests for other main-group elements.

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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 found in the outermost shell of an atom. They play a critical role in determining how an atom can interact with others. These electrons are involved in forming chemical bonds, as they can be shared, gained, or lost in interactions with other atoms.

Atoms aim to have their valence shell either completely filled or empty, resembling the stable electron configurations of noble gases. Having a full shell generally means eight electrons, hence the name valence octet. The tendency of atoms to complete this shell is the basis for many chemical reactions and bonds.
Chemical Bonding
Chemical bonding occurs when atoms connect with one another to achieve more stable electron configurations. In most cases, this involves interactions between valence electrons. There are several types of chemical bonds:
  • Covalent Bonds: Where atoms share valence electrons.
  • Ionic Bonds: Where electrons are transferred from one atom to another, forming ions with opposite charges that attract each other.
  • Metallic Bonds: Where electrons flow freely around a lattice of metal atoms.

Through these bonds, atoms can obtain a noble gas configuration. This often involves completing their valence shell to emulate the stability seen in noble gases, usually achieving an octet.
Noble Gas Configuration
A noble gas configuration refers to the electron arrangement in the outer shell of noble gases, such as neon and argon. These gases have complete valence shells, usually with eight valence electrons (except for helium, which has two). This full shell makes them incredibly stable and mostly unreactive.

Other elements aim to achieve this same stable configuration, either by gaining, losing, or sharing electrons through chemical bonding. The quest for this relaxed state explains why many chemical reactions occur, resulting in the achievement of an octet or duet (as in helium and hydrogen).
Hydrogen Exception
Hydrogen is unique in that it does not follow the octet rule. Instead of aiming for eight electrons in its valence shell, hydrogen strives for two, as seen in helium. This is known as a "duet" rule. Hydrogen achieves stability with just two electrons in its 1s orbital, a configuration that is the same as helium's.

This unique goal reflects hydrogen's simple electron structure, having only one valence electron to start with. Thus, it can either lose, gain, or share a single electron to reach a stable state, making it an exception to the general pursuit of an eight-electron configuration.
Helium Exception
Helium is another exception to the octet rule, not because it fails to seek a stable electron configuration, but because it already maintains one. With only two electrons filling its 1s orbital, helium's valence shell is fully occupied, forming what is known as a "duet."

Since helium's first energy level only requires two electrons to be complete, helium is inherently stable and does not need to participate in chemical bonding. This stability is why helium, as with other noble gases, is inert and less likely to form compounds.

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Most popular questions from this chapter

Interpret Data A company plans to make an electronic device. They need to use an element that has chemical behavior similar to that of silicon (Si) and lead (Pb). The element must have an atomic mass greater than that of sulfur (S), but less than that of cadmium (Cd). Use the periodic table to determine which element the company could use.

Make and Use Graphs Graph the atomic radii of the representative elements in periods 2, 3, and 4 versus their atomic numbers. Connect the points of elements in each period, so that there are three separate curves on the graph. Summarize the trends in atomic radii shown on your graph. Explain.

New Heavy Element If scientists discovered an element with 117 protons, what would be the its group and period? Would it be a metal, a metalloid, or a nonmetal?

Explain why the s-block of the periodic table is two-groups wide, the p-block is six-groups wide, and the d-block is ten-groups wide.

Explain why each successive ionization of an electron requires a greater amount of energy.
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