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Chapter 2: Problem 79

Draw two different structural formulas based on the molecular formula \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\). Is the fact that you can have more than one compound with the same molecular formula consistent with Dalton's atomic theory?

Short Answer

Expert verified
Two different structural formulas for the molecular formula \(C_{2}H_{6}O\) could be Ethanol and Methoxymethane. Having more than one compound with the same molecular formula (isomers) is consistent with Dalton's atomic theory, as it does not consider the different arrangement of atoms within a molecule.

Step by step solution

01

Draw the first structural formula

The first way to arrange \(C_{2}H_{6}O\) is by placing the two carbon (C) atoms in the center, surrounded by hydrogen (H) atoms with one of the carbons linked to an oxygen (O) atom, forming an alcohol called Ethanol: \n\nH H H\n| | |\nH-C-C-O-H\n| | |\nH H H
02

Draw the second structural formula

The second way to arrange \(C_{2}H_{6}O\) is by placing the two carbons (C) and one oxygen (O) in the center, surrounded by hydrogen (H) atoms, forming an ether called Methoxymethane. \n\n H H H\n | | |\nH -C - O - C - H\n | |\n H H
03

Analysis According to Dalton's Atomic Theory

While Dalton's atomic theory states that atoms of the same element are identical, it does not conflict with the idea of isomers. This is because Dalton's theory does not consider the arrangement of atoms within a molecule. It simply states that all atoms of a certain element behave the same. In the case of isomers, while the atoms are arranged differently, they are still identical atoms of carbon, hydrogen, and oxygen, behaving as such atoms should.

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Most popular questions from this chapter

Consult a handbook of chemical and physical data (ask your instructor where you can locate a copy of the handbook) to find (a) two metals less dense than water, (b) two metals more dense than mercury, (c) the densest known solid metallic element, (d) the densest known solid nonmetallic element.

Group these elements in pairs that you would expect to show similar chemical properties: \(\mathrm{K}, \mathrm{F}, \mathrm{P}, \mathrm{Na}, \mathrm{Cl}\) and \(N\).

Give an example of each of the following: (a) a monatomic cation, (b) a monatomic anion, (c) a polyatomic cation, (d) a polyatomic anion.

Why do all atoms of an element have the same atomic number, although they may have different mass numbers? What do we call atoms of the same element with different mass numbers? Explain the meaning of each term in the symbol \({ }_{Z}^{A} \mathrm{X}\).

Define these terms: (a) atomic number, (b) mass number. Why does a knowledge of atomic number enable us to deduce the number of electrons present in an atom?
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