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Chapter 7: Problem 3

Why is the ratio between the empirical formula and the molecular formula a whole number?

Short Answer

Expert verified
The ratio between empirical and molecular formula is a whole number because the molecular formula is made up of integer multiples of the empirical formula.

Step by step solution

01

Define Empirical and Molecular Formula

Empirical formula is the simplest whole number expression of a compound whereas the molecular formula gives the actual number of atoms of each element in a molecule of the compound.
02

Describe Relationship

Molecular formula is a multiple of the empirical formula. This is because a molecular formula could represent multiple molecules of the empirical formula.
03

Explain Ratio Nature

The ratio between the empirical formula and the molecular formula is therefore always a whole number because the molecular formula is composed of integer multiples of the empirical formula.

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Key Concepts

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

Empirical Formula
An empirical formula is like the simplest form of a chemical formula. It shows the basic ratio of each type of atom in a compound. This doesn't tell you the exact number of atoms, but it does show the simplest whole number ratio of different elements in a compound.

For instance, in hydrogen peroxide, the empirical formula is HO, indicating a 1:1 ratio of hydrogen to oxygen. In its most reduced form, it shows the core relationship between the elements.

Empirical formulas are useful because they provide a simplified perspective which can be especially helpful in determining key chemical properties and conducting laboratory analyses.
  • Represents the simplest ratio of atoms.
  • Does not show the exact count of atoms in a molecule.
  • Simplifies complex chemical compositions.
Molecular Formula
The molecular formula reveals the actual number of atoms of each element in a molecule of a compound. It builds on the empirical formula by showing how many of each type of atom actually exist in a real molecule.

Using the hydrogen peroxide example from before, its molecular formula is \( \text{H}_2\text{O}_2 \). This shows it has 2 hydrogen atoms and 2 oxygen atoms, distinguishing it from the simpler empirical formula "HO."

While empirical formulas give a simplified ratio, molecular formulas ensure specificity by representing the precise make-up of a compound. This can be vital for understanding how a compound will react or interact with other substances.
  • Gives the exact atom count in a molecule.
  • Displays the true structure of the compound.
  • Important for predicting chemical behaviors.
Whole Number Ratio
The relationship between an empirical formula and a molecular formula can be understood through the concept of a whole number ratio. This connection is because the molecular formula is an integer multiple of the empirical formula.

Essentially, multiplying the empirical formula by a whole number, known as the "n-factor," will yield the molecular formula. For example, if the empirical formula is CH, like in benzene, the whole number multiple would be 6 to get the molecular formula \( \text{C}_6\text{H}_6 \).

The reason it is always a whole number stems from the requirements of atomic structure and stability, meaning complete and consistent integration of atoms in a compound.
  • Molecular formula is a whole number multiple of the empirical formula.
  • Shows proportional consistency between empirical and molecular compositions.
  • Helps in precisely identifying chemical substances.

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Most popular questions from this chapter

A compound of silver has the following analytical composition: \(63.50 \% \mathrm{Ag}, 8.25 \%\) \(\mathrm{N},\) and 28.25\(\%\) O. Calculate the empirical formula.

When you calculate the percentage composition of a compound from both the empirical formula and the molecular formula, why are the two results identical?

How would you determine the number of molecules in 3 mol of oxygen, \(\mathrm{O}_{2} ?\)

A 1.344 g sample of a compound contains 0.365 g \(N a, 0.221 \mathrm{g} \mathrm{N},\) and 0.758 \(\mathrm{g}\) O. What is its percentage composition? Calculate its empirical formula.

Calculating the Molar Mass of a Compound The graphing calculator can run a program that calculates the molar mass of a compound given the chemical formula for the compound. This program will prompt for the number of elements in the formula, the number of atoms of each element in the formula, and the atomic mass of each element in the formula. It then can be used to find the molar masses of various compounds. Go to Appendix \(C\) . If you are using a TI-83 Plus, you can download the program MOLMASS and data sets and run the application as directed. If you are using another calculator, your teacher will provide you with the keystrokes and data sets to use. After you have graphed the data, answer the questions below. a. What is the molar mass of \(\mathrm{BaTiO}_{3} ?\) b. What is the molar mass of \(\mathrm{PbCl}_{2} ?\) c. What is the molar mass of \(\mathrm{NH}_{4} \mathrm{NO}_{3} ?\)
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