CH3CH=CH2 + 4.50=0 ---> з0-С-С + ЗН-О-Н using the following bond enthalpy values: Bond Bond Energy C-C C=C C-H C=O O=0 O-H 347 611 414 736 498 464 REMINDER: AH = E Ereactant bonds broken - I Eproduct bonds broken AH = -1517 kJ AH = - 7200 kJ None of these AH = 1517 kJ AH = 5683 kJ AH = 7200 kJ Ο ΔΗ-0
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.
Polarity Of Water
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.
![**Determining the Enthalpy Change of a Reaction**
**Reaction:**
\[ \text{CH}_3\text{CH}=\text{CH}_2 + 4.5\text{O}=\text{O} \rightarrow 3\text{O}=\text{C}=\text{O} + 3\text{H}-\text{O}-\text{H} \]
**Bond Enthalpy Values:**
| Bond | Bond Energy (kJ/mol) |
|--------|----------------------|
| C–C | 347 |
| C=C | 611 |
| C–H | 414 |
| C=O | 736 |
| O=O | 498 |
| O–H | 464 |
**Formula for Enthalpy Change:**
\[
\Delta H = \Sigma E_{\text{reactant bonds broken}} - \Sigma E_{\text{product bonds broken}}
\]
**Options for \(\Delta H\):**
- \( \Delta H = -1517 \text{ kJ} \)
- \( \Delta H = -7200 \text{ kJ} \)
- None of these
- \( \Delta H = 1517 \text{ kJ} \)
- \( \Delta H = 5683 \text{ kJ} \)
- \( \Delta H = 7200 \text{ kJ} \)
- \( \Delta H = 0 \)
**Explanation:**
To find the enthalpy change, you need to calculate the total bond energies for the reactants and the products, and then apply the formula above. Determine which bonds are broken in the reactants and which bonds are formed in the products, using the given bond energies.
This calculation will help in understanding how energy is absorbed or released in a chemical reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1c9a3da8-b443-4c7b-9ddb-d4ba4f71dd14%2Fd4eddd62-eefa-45d9-90ae-fd2d233253f6%2Fe7euvp7_processed.png&w=3840&q=75)
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