Calculate the ΔHrxn using bond enthalpies for the balanced equation below (Lewis structures also provided). Bond Enthalpy Values: Bond ΔH (kJ/mol) C=C 611 C–H 414 H–H 436 C–C 347 Group of answer choices -219 kJ -128 kJ 286 kJ -564 kJ
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.
Calculate the ΔHrxn using bond enthalpies for the balanced equation below (Lewis structures also provided).
| Bond Enthalpy Values: | |
|
Bond |
ΔH (kJ/mol) |
|
C=C |
611 |
|
C–H |
414 |
|
H–H |
436 |
|
C–C |
347 |
![### Bond Enthalpy Calculation for Reaction
**Calculate the ΔH_rxn** using bond enthalpies for the balanced equation below (Lewis structures also provided).
#### Chemical Reaction:
\[ \text{C}_2\text{H}_4(g) + \text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g) \]
- **C₂H₄ (g) Structure**:
- An ethene molecule with a double bond between two carbon atoms. Each carbon is also single-bonded to two hydrogen atoms.
```
H H
\ /
C=C
/ \
H H
```
- **H₂ (g) Structure**:
- A hydrogen molecule with a single bond.
```
H—H
```
- **C₂H₆ (g) Structure**:
- An ethane molecule with a single bond between two carbon atoms. Each carbon is also single-bonded to three hydrogen atoms.
```
H H
| |
H—C—C—H
| |
H H
```
#### Bond Enthalpy Values:
| Bond | ΔH (kJ/mol) |
|-------|-------------|
| C=C | 611 |
| C—H | 414 |
| H—H | 436 |
| C—C | 347 |
#### Possible Answers for ΔH_rxn:
- -219 kJ
- -128 kJ
- 286 kJ
- -564 kJ
Choose the correct enthalpy change for the reaction given the bond enthalpies.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F840f535b-f075-49f5-9fe8-c5a30f6f8dd7%2Fa0243da7-f814-4855-a724-f792beac5746%2F17dbe8i_processed.png&w=3840&q=75)
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