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Chapter 11: Problem 51

What type of structure must each atom in a compound usually exhibit for the compound to be stable?

Short Answer

Expert verified
Each atom in a compound must usually exhibit a structure that follows the octet rule (or duet rule for hydrogen and helium) to be stable. This means that atoms need to have a full set of eight valence electrons (or two for hydrogen and helium) in their outermost electron shell. Atoms achieve this by forming chemical bonds, such as covalent or ionic bonds, with other atoms in the compound to share, lose, or gain electrons and complete their electron shells.

Step by step solution

01

Rule for atom stability #

In most compounds, atoms follow the octet rule to achieve a stable configuration. The octet rule states that atoms are most stable when they have a full set of eight valence electrons in their outermost electron shell. This is because having a full outer electron shell minimizes the atom's potential energy and makes it less reactive. Exceptions to the rule exist for elements with less than eight electrons in total, like hydrogen and helium, which follow the duet rule, meaning they become stable with two electrons in their outer shell. #
02

Structure for compounds #

In order for a compound to be stable, each atom in the compound must achieve the stable configuration following the octet rule (or duet rule for hydrogen and helium). Atoms form chemical bonds, such as covalent or ionic bonds, with other atoms in the compound so that each atom can complete its valence electron shell and become stable. Consequentially, the type of structure that each atom must exhibit within a stable compound is one where each atom shares, loses, or gains electrons to fulfill its electron shell according to the octet or duet rule. #

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Most popular questions from this chapter

Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. a. nitrate ion b. carbonate ion c. ammonium ion

What do we mean by the bond energy of a chemical bond?

For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. a. \(\mathrm{C}-\mathrm{F}\) b. \(\mathrm{Si}-\mathrm{C}\) c. \(\mathrm{C}-\mathrm{O}\) d. \(\mathrm{B}-\mathrm{C}\)

Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those molecules that exhibit resonance, draw the various possible resonance forms. a. \(\mathrm{SO}_{2}\) b. \(\mathrm{N}_{2} \mathrm{O}(\mathrm{N}\) in center) c. \(O_{3}\)

Explain how the atoms in covalent molecules achieve configurations similar to those of the noble gases. How does this differ from the situation in ionic compounds?
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