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Chapter 17: Problem 51

Are \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{H}_{2} \mathrm{O}_{2}\) isomers? Explain.

Short Answer

Expert verified
No, H2O and H2O2 are not isomers because they have different molecular formulas: H2O has one oxygen atom while H2O2 has two. Their structural arrangements are also different: H2O has two hydrogen atoms bonded to one oxygen atom (H-O-H), while H2O2 has each hydrogen atom bonded to a separate oxygen atom (H-O-O-H).

Step by step solution

01

Molecular Formula of H2O and H2O2

According to the given exercise, we have two compounds: 1. H2O: It has two hydrogen atoms (H) and one oxygen atom (O). 2. H2O2: It has two hydrogen atoms (H) and two oxygen atoms (O).
02

Structural Arrangement of H2O

In the case of H2O (Water), the oxygen atom forms two single covalent bonds with two hydrogen atoms. The structure looks like this: H-O-H.
03

Structural Arrangement of H2O2

For H2O2 (Hydrogen Peroxide), each oxygen atom forms a single bond with a hydrogen atom and also forms a single bond with the other oxygen atom. The structure of hydrogen peroxide can be represented as: H-O-O-H.
04

Comparing Molecular Formulas and Structures

Upon comparing the molecular formulas of H2O and H2O2, we notice that they are different, with H2O having one oxygen atom while H2O2 has two. Also, their structural arrangements are different. In H2O, two hydrogen atoms are bonded to one oxygen atom, while in H2O2, each hydrogen atom is bonded to a separate oxygen atom.
05

Conclusion

Based on the comparison of their molecular formulas and structural arrangements, we can conclude that H2O and H2O2 are not isomers because they have different molecular formulas and structural arrangements.

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Key Concepts

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

Molecular Formula
Understanding the molecular formula is essential to identifying substances and predicting their chemical behavior. The molecular formula gives a count of each type of atom present in a molecule. For example, in water (H2O), the formula indicates there are two hydrogen atoms and one oxygen atom. In contrast, hydrogen peroxide (H2O2) is composed of two hydrogen atoms and two oxygen atoms.

These formulas are concise methods of describing molecular composition. They are crucial when comparing substances to determine their identity or when discerning different compounds. However, it鈥檚 important to note that molecular formulas do not provide structural information about how these atoms are arranged and bonded.
Covalent Bonds
Covalent bonds are the glue that holds molecules together. They form when atoms share pairs of electrons to attain a stable electron configuration. In the water molecule (H2O), each hydrogen atom shares an electron with the oxygen atom, forming two single covalent bonds.

In hydrogen peroxide (H2O2), each oxygen atom forms a single bond with one hydrogen atom. Furthermore, the two oxygen atoms share a pair of electrons, resulting in a single covalent bond between them, which holds the entire molecule together.
  • Covalent bonds involve electron sharing.
  • They contribute to the molecule's stability.
  • They determine the molecule鈥檚 structure.
Hydrogen Peroxide
Hydrogen peroxide is a compound with interesting structural properties. It is represented by the formula H2O2. The compound's structure consists of two hydrogen atoms each connected to an oxygen atom, and the two oxygen atoms bonded to each other. This defines hydrogen peroxide's distinct arrangement.

Due to the O-O bond, hydrogen peroxide is less stable than some other compounds, such as water, and can readily decompose into water (H2O) and oxygen (O2). Its unique structure also makes it a powerful oxidizing agent used in both industrial and medical applications.
  • Known for its bleaching and disinfecting properties.
  • Unstable due to the O-O bond.
  • Used in dilute form as an antiseptic.
Water Structure
The structure of the water molecule ( H2O) is simple yet fundamental for life as we know it. The oxygen atom in H2O forms two covalent bonds with hydrogen atoms, creating a bent shape due to the electron pair repulsion. This results in a molecule that has a slight negative charge on the oxygen and a slight positive charge on the hydrogens.

This polar nature of water molecules leads to hydrogen bonding, which is responsible for many of water's unique properties:
  • High surface tension.
  • Excellent solvent for ionic and polar substances.
  • Regulating temperature due to its high specific heat capacity.
Water鈥檚 molecular structure gives rise to its critical role in biological, chemical, and environmental processes.

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Most popular questions from this chapter

The common name for ethyne is acetylene. Draw a dot diagram and a line drawing for this compound, and indicate whether it is more or less unsaturated than ethene.

Where do we start numbering carbons on a main chain when both branches and \(C=C\) or \(C \equiv C\) bonds are present?

2-Propanol is quite soluble in water, but 2 -decanol is insoluble in water. Draw both structural formulas and explain why one compound is soluble but the other isn't.

What is wrong with using common names for hydrocarbon molecules?

Although it was not discussed in the chapter, it is possible for a hydrocarbon molecule to have more than one site of unsaturation. One such molecule is 1,3 -butadiene; the \(d i\) - tells us there are two double bonds in the molecule. Give the molecular formula and line drawing for this molecule.
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