CHM 103 003 General Chemistry I C OWLV2 | Online teaching and learning resource from Cengage Learning 8. [References) pt Use the References to access important values if needed for this question. pt Using average bond enthalpies (linked above), estimate the enthalpy change for the following reaction: pt CH (g) + 2F2(g)-CH,F2(g) + 2HF(g) pt kJ pt pt Submit Answer Try Another Version 5 item attempts remaining pt pt pt pt
Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
![**Title: Estimating Enthalpy Change Using Average Bond Enthalpies**
**Objective:**
Learn how to estimate the enthalpy change for a chemical reaction using average bond enthalpies.
**Reaction:**
\[ \text{CH}_4(g) + 2\text{F}_2(g) \rightarrow \text{CH}_2\text{F}_2(g) + 2\text{HF}(g) \]
**Instructions:**
Using average bond enthalpies provided in your references, estimate the enthalpy change for the reaction above.
**Calculation Steps:**
1. **Identify Bonds Broken and Formed:**
- Reactants: Break bonds in \(\text{CH}_4\) and \(\text{F}_2\).
- Products: Form bonds in \(\text{CH}_2\text{F}_2\) and \(\text{HF}\).
2. **Calculate Total Energy for Bonds Broken:**
Use the average bond enthalpies to calculate the energy required to break the bonds in the reactants.
3. **Calculate Total Energy for Bonds Formed:**
Use the average bond enthalpies to calculate the energy released when forming the bonds in the products.
4. **Determine Enthalpy Change (\(\Delta H\)):**
\[ \Delta H = \text{Energy required to break bonds} - \text{Energy released in forming bonds} \]
**Additional Information:**
- Bond enthalpies are typically given in kJ/mol.
- Enthalpy changes provide insights into whether a reaction is endothermic (absorbs energy) or exothermic (releases energy).
**Answer Submission:**
Enter your calculated enthalpy change in kJ. You have 5 attempts remaining to submit your answer accurately.
**Tools:**
- Submit Answer
- Try Another Version
This exercise helps you understand the concept of bond energies and their role in determining the energy profile of chemical reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf5b27fc-182c-458d-bf52-a3d5fb8d4e7e%2Facf59e67-5db6-48da-aaae-8c94158f2b8d%2Flk40kjp_processed.jpeg&w=3840&q=75)
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