15 attempts left Check my work Enter your answer in the provided box. Guided Solution Sports trainers treat sprains and soreness with ethyl bromide. It is manufactured by reacting ethylene with hydrogen bromide: 1 points --- Bri + H References H. Use bond energies to find the enthalpy change for this reaction. kJ Average Bond Energies Bond H-H C-C C=C |Bond Enthalpy (kJ/mol) 432 347 614 839 C=C C-H C-Br Br-Br H-Br 413 276 193 363
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
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In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
![**Exercise: Calculating Enthalpy Change Using Bond Energies**
**Objective:**
Calculate the enthalpy change for the reaction where ethylene and hydrogen bromide react to form ethyl bromide.
**Instructions:**
Enter your answer in the provided box.
**Context:**
Sports trainers often treat sprains and soreness with ethyl bromide, which is manufactured by reacting ethylene with hydrogen bromide.
**Chemical Reaction:**
H2C=CH2 + HBr → H3C-CH2Br
**Task:**
Use bond energies to find the enthalpy change for this reaction.
**Enter your answer:**
\[ \_\_\_\_ \text{kJ} \]
**Bond Energies Table:**
| Bond | Bond Enthalpy (kJ/mol) |
|--------|------------------------|
| H—H | 432 |
| C—C | 347 |
| C=C | 614 |
| C≡C | 839 |
| C—H | 413 |
| C—Br | 276 |
| Br—Br | 193 |
| H—Br | 363 |
**Guided Solution:**
Use the average bond energies provided to calculate the total energy required to break the original bonds and the total energy released when new bonds form. Determine the enthalpy change by subtracting the energy required from the energy released.
**Do you need help?** Click on "Guided Solution" for a step-by-step walkthrough.
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**Note to students:**
Understanding bond energies and their application in calculating reaction enthalpies is crucial for mastering thermodynamics in chemistry. Practice using the given data and approach to gain confidence in these calculations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F728e70e5-602c-40ad-8198-449db4e3e647%2Fe82a0c9d-4d5f-4b33-95ea-5b5adbf6ee36%2F16yf4gi_processed.jpeg&w=3840&q=75)
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