Explain how you would get an enthalpy of formation that is greater than zero using the magnitudes of the bond enthalpies and equation 9.3 (given in the image attached)
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.
Explain how you would get an enthalpy of formation that is greater than zero using the magnitudes of the bond enthalpies and equation 9.3 (given in the image attached)
![The equation presented here represents the calculation for the change in enthalpy (\(\Delta H^\circ\)) during a chemical reaction, based on bond enthalpies:
\[
\Delta H^\circ = \Sigma \text{BE (reactants)} - \Sigma \text{BE (products)}
\]
\[
= \text{total energy input} - \text{total energy released}
\]
Where:
- \(\Sigma\) stands for the summation sign, indicating the summation of bond enthalpies.
- \(\text{BE}\) represents the bond enthalpy.
- The equation expresses that the change in enthalpy is the difference between the total bond energies required to break the bonds in the reactants and the total energy released when bonds are formed in the products.
There are no graphs or diagrams accompanying this equation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F03fa78cd-6ce9-4582-bb7c-dbeac4c245c8%2Fb6eaa790-8825-43b3-b02c-8e7617294b6d%2F23n2ors_processed.jpeg&w=3840&q=75)
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