For Each Of The Formulas, Classify The Formula As Either An Empirical Formula, A Molecular Formula, Or Both.1. N A H C O 3 NaHCO_3 N A H C O 3 ​ - [ ] Empirical Formula - [ ] Molecular Formula - [ ] Both2. C 2 H 6 C_2H_6 C 2 ​ H 6 ​ - [ ] Empirical Formula - [ ]

Introduction

In chemistry, formulas are used to represent the composition of molecules. Two types of formulas are commonly used: empirical formulas and molecular formulas. Empirical formulas represent the simplest whole-number ratio of atoms in a molecule, while molecular formulas represent the actual number of atoms in a molecule. In this article, we will explore the differences between empirical and molecular formulas and classify several given formulas as either empirical, molecular, or both.

What is an Empirical Formula?

An empirical formula is a chemical formula that represents the simplest whole-number ratio of atoms in a molecule. It is a way of expressing the composition of a molecule in terms of the smallest possible whole-number ratio of atoms. Empirical formulas are often used to represent the composition of molecules that have a simple ratio of atoms.

What is a Molecular Formula?

A molecular formula is a chemical formula that represents the actual number of atoms in a molecule. It is a way of expressing the composition of a molecule in terms of the actual number of atoms present. Molecular formulas are often used to represent the composition of molecules that have a complex ratio of atoms.

Classifying Formulas

Now that we have a basic understanding of empirical and molecular formulas, let's classify the given formulas as either empirical, molecular, or both.

Formula 1: $NaHCO_3$

• Empirical Formula: [ ]
• Molecular Formula: [ ]
• Both: [ ]

To classify this formula, we need to determine the simplest whole-number ratio of atoms in the molecule. The formula $NaHCO_3$ represents a molecule with one sodium atom, one hydrogen atom, one carbon atom, and three oxygen atoms. The simplest whole-number ratio of atoms in this molecule is 1:1:1:3, which is the empirical formula. Therefore, the correct classification for this formula is:

• Empirical Formula: [X]
• Molecular Formula: [ ]
• Both: [ ]

Formula 2: $C_2H_6$

• Empirical Formula: [ ]
• Molecular Formula: [ ]
• Both: [ ]

To classify this formula, we need to determine the simplest whole-number ratio of atoms in the molecule. The formula $C_2H_6$ represents a molecule with two carbon atoms and six hydrogen atoms. The simplest whole-number ratio of atoms in this molecule is 2:6, which can be simplified to 1:3. Therefore, the correct classification for this formula is:

• Empirical Formula: [X]
• Molecular Formula: [X]
• Both: [ ]

Formula 3: $H_2O$

• Empirical Formula: [ ]
• Molecular Formula: [ ]
• Both: [ ]

To classify this formula, we need to determine the simplest whole-number ratio of atoms in the molecule. The formula $H_2O$ represents a molecule with two hydrogen atoms and one oxygen atom. The simplest whole-number ratio of atoms in this molecule is 2:1, which is the empirical formula. Therefore, the correct classification for this formula is:

• Empirical Formula: [X]
• Molecular Formula: [ ]
• Both: [ ]

Formula 4: $CH_4$

• Empirical Formula: [ ]
• Molecular Formula: [ ]
• Both: [ ]

To classify this formula, we need to determine the simplest whole-number ratio of atoms in the molecule. The formula $CH_4$ represents a molecule with one carbon atom and four hydrogen atoms. The simplest whole-number ratio of atoms in this molecule is 1:4, which is the empirical formula. Therefore, the correct classification for this formula is:

• Empirical Formula: [X]
• Molecular Formula: [X]
• Both: [ ]

Formula 5: $C_6H_12O_6$

• Empirical Formula: [ ]
• Molecular Formula: [ ]
• Both: [ ]

To classify this formula, we need to determine the simplest whole-number ratio of atoms in the molecule. The formula $C_6H_12O_6$ represents a molecule with six carbon atoms, twelve hydrogen atoms, and six oxygen atoms. The simplest whole-number ratio of atoms in this molecule is 6:12:6, which can be simplified to 1:2:1. Therefore, the correct classification for this formula is:

• Empirical Formula: [X]
• Molecular Formula: [X]
• Both: [ ]

Conclusion

Introduction

In our previous article, we explored the differences between empirical and molecular formulas and classified several given formulas as either empirical, molecular, or both. In this article, we will answer some frequently asked questions about empirical and molecular formulas.

Q: What is the difference between an empirical formula and a molecular formula?

A: An empirical formula represents the simplest whole-number ratio of atoms in a molecule, while a molecular formula represents the actual number of atoms in a molecule.

Q: How do I determine the empirical formula of a molecule?

A: To determine the empirical formula of a molecule, you need to find the simplest whole-number ratio of atoms in the molecule. This can be done by dividing the number of atoms of each element by the greatest common divisor (GCD) of the numbers.

Q: How do I determine the molecular formula of a molecule?

A: To determine the molecular formula of a molecule, you need to know the actual number of atoms in the molecule. This can be done by using techniques such as mass spectrometry or nuclear magnetic resonance (NMR) spectroscopy.

Q: What is the relationship between empirical and molecular formulas?

A: The empirical formula of a molecule is a factor of the molecular formula. In other words, the molecular formula can be expressed as a multiple of the empirical formula.

Q: Can a molecule have the same empirical and molecular formulas?

A: Yes, a molecule can have the same empirical and molecular formulas. This occurs when the molecular formula is a multiple of the empirical formula.

Q: Can a molecule have different empirical and molecular formulas?

A: Yes, a molecule can have different empirical and molecular formulas. This occurs when the molecular formula is not a multiple of the empirical formula.

Q: How do I classify a formula as empirical, molecular, or both?

A: To classify a formula as empirical, molecular, or both, you need to determine the simplest whole-number ratio of atoms in the molecule (empirical formula) and the actual number of atoms in the molecule (molecular formula). If the two formulas are the same, the formula is both empirical and molecular. If the two formulas are different, the formula is either empirical or molecular.

Q: What are some common examples of empirical and molecular formulas?

A: Some common examples of empirical and molecular formulas include:

• Empirical formula: H2O, Molecular formula: H2O
• Empirical formula: CH4, Molecular formula: CH4
• Empirical formula: C6H12O6, Molecular formula: C6H12O6

Conclusion

In conclusion, empirical and molecular formulas are two types of formulas used to represent the composition of molecules. By understanding the differences between these two types of formulas, we can classify given formulas as either empirical, molecular, or both. We hope this Q&A guide has been helpful in answering your questions about empirical and molecular formulas.

Frequently Asked Questions

Q: What is the difference between an empirical formula and a molecular formula?

A: An empirical formula represents the simplest whole-number ratio of atoms in a molecule, while a molecular formula represents the actual number of atoms in a molecule.

Q: How do I determine the empirical formula of a molecule?

A: To determine the empirical formula of a molecule, you need to find the simplest whole-number ratio of atoms in the molecule. This can be done by dividing the number of atoms of each element by the greatest common divisor (GCD) of the numbers.

Q: How do I determine the molecular formula of a molecule?

A: To determine the molecular formula of a molecule, you need to know the actual number of atoms in the molecule. This can be done by using techniques such as mass spectrometry or nuclear magnetic resonance (NMR) spectroscopy.

Q: What is the relationship between empirical and molecular formulas?

A: The empirical formula of a molecule is a factor of the molecular formula. In other words, the molecular formula can be expressed as a multiple of the empirical formula.

Q: Can a molecule have the same empirical and molecular formulas?

A: Yes, a molecule can have the same empirical and molecular formulas. This occurs when the molecular formula is a multiple of the empirical formula.

Q: Can a molecule have different empirical and molecular formulas?

A: Yes, a molecule can have different empirical and molecular formulas. This occurs when the molecular formula is not a multiple of the empirical formula.

Q: How do I classify a formula as empirical, molecular, or both?

A: To classify a formula as empirical, molecular, or both, you need to determine the simplest whole-number ratio of atoms in the molecule (empirical formula) and the actual number of atoms in the molecule (molecular formula). If the two formulas are the same, the formula is both empirical and molecular. If the two formulas are different, the formula is either empirical or molecular.

Q: What are some common examples of empirical and molecular formulas?

A: Some common examples of empirical and molecular formulas include:

• Empirical formula: H2O, Molecular formula: H2O
• Empirical formula: CH4, Molecular formula: CH4
• Empirical formula: C6H12O6, Molecular formula: C6H12O6