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Chapter 6: Problem 3

Explain why \(\mathrm{C}_{2} \mathrm{H}_{4}\) has fewer hydrogen atoms than \(\mathrm{C}_{2} \mathrm{H}_{6}\).

Short Answer

Expert verified
The double bond in \(\mathrm{C}_{2} \mathrm{H}_{4}\) restricts the hydrogen count compared to the single bonds in \(\mathrm{C}_{2} \mathrm{H}_{6}\), leading to fewer hydrogen atoms.

Step by step solution

01

Understand the Chemical Formula

The chemical formula is a way to represent how many atoms of each element are present in a compound. - For \(\mathrm{C}_{2} \mathrm{H}_{4}\), there are 2 carbon (\mathrm{C}) atoms and 4 hydrogen (\mathrm{H}) atoms.- For \(\mathrm{C}_{2} \mathrm{H}_{6}\), there are 2 carbon (\mathrm{C}) atoms and 6 hydrogen (\mathrm{H}) atoms.
02

Atom Count Comparison

Look at the number of hydrogen atoms in each compound:- For \(\mathrm{C}_{2} \mathrm{H}_{4}\), there are 4 hydrogen atoms.- For \(\mathrm{C}_{2} \mathrm{H}_{6}\), there are 6 hydrogen atoms.- Compare the two, and you will see that \(\mathrm{C}_{2} \mathrm{H}_{4}\) has 2 fewer hydrogen atoms than \(\mathrm{C}_{2} \mathrm{H}_{6}\).
03

Understanding the Molecular Structure

In \(\mathrm{C}_{2} \mathrm{H}_{4}\), the carbon atoms form a double bond (\(\mathrm{C=C}\)), which affects the number of hydrogen atoms that can bond with the carbons because double bonds limit the number of hydrogen atoms that can attach.- In \(\mathrm{C}_{2} \mathrm{H}_{6}\), the carbon atoms form single bonds (\(\mathrm{C-C}\)), allowing for more hydrogen atoms to be bonded, so each carbon is attached to 3 hydrogen atoms, making 6 hydrogen atoms in total for the molecule.
04

Conclusion

The presence of a double bond in \(\mathrm{C}_{2} \mathrm{H}_{4}\) reduces the number of hydrogen atoms compared to the single bonds in \(\mathrm{C}_{2} \mathrm{H}_{6}\), resulting in fewer hydrogen atoms in \(\mathrm{C}_{2} \mathrm{H}_{4}\). This structural difference is the reason for the difference in the hydrogen atom count.

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Key Concepts

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

Molecular Structure
When we talk about molecular structure, we mean how the atoms in a molecule are arranged in relation to one another. This involves not only counting atoms but understanding how they connect.
In a molecule like ethylene (\(\mathrm{C}_2 \mathrm{H}_4\)), the molecular structure includes carbon atoms that share a double bond. This affects how many other atoms, like hydrogens, can bond to each carbon.
  • Double bonds tend to reduce the number of total atoms connected to each carbon.
  • Bond angles and hybridization also contribute to the molecular shape and structure.
  • This differs from molecules with only single bonds, which can allow for more surrounding atoms due to having more available bonding spots.
Understanding the molecular structure helps us predict not just appearances but reactivity and properties.
Chemical Formula
A chemical formula is a shorthand way of showing what elements make up a molecule and how many atoms there are of each. For instance, in \(\mathrm{C}_2 \mathrm{H}_4\), it shows there are 2 carbon and 4 hydrogen atoms.
This formula is like a recipe, providing a precise count of elements but not detailing how they connect. However, by counting atoms, we can infer a lot about the molecule itself.
  • Helps in identifying the particular compound.
  • Assists in balancing chemical reactions.
  • Allows for calculation of molar mass, useful in quantitative chemistry.
Learning to read and understand a chemical formula is a fundamental skill in chemistry.
Double Bond
A double bond involves two pairs of electrons shared between two atoms, typically carbon atoms. In chemical structures, double bonds are denoted by two lines (=).
In our example, \(\mathrm{C}_2 \mathrm{H}_4\) has a carbon-carbon double bond. This double bond significantly influences the properties of a molecule and its ability to bind with other atoms, as electrons are occupied in forming the double bond.
  • Double bonds restrict rotation around the bond axis, leading to different isomers.
  • They are stronger than single bonds but not twice as strong.
  • Double bonds contribute to the molecule's stability and rigidity.
Molecules with double bonds often participate in different chemical reactions than those with only single bonds. Understanding the impact of double bonds is crucial for predicting chemical behavior.
Single Bond
Single bonds involve the sharing of one pair of electrons between two atoms, such as in ethane (\(\mathrm{C}_2 \mathrm{H}_6\)).
These bonds enable more hydrogens to attach to the carbons compared to double bonds; therefore, each carbon in \(\mathrm{C}_2 \mathrm{H}_6\) bonds with three hydrogen atoms via single bonds.
  • Single bonds allow for free rotation about the bond axis, unlike double bonds.
  • They are simpler and generally weaker than double or triple bonds.
  • Molecules with single bonds are typically more flexible.
The simplicity and flexibility provided by single bonds often result in different physical properties, such as lower boiling points compared to double-bonded compounds.

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