Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical-radical combination reaction is the formation of a new electron-pair bond. Consider the formation of hydrogen peroxide. 2 OH(g) H,O,g) Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons.
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.
![Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical–radical combination reaction is the formation of a new electron-pair bond.
Consider the formation of hydrogen peroxide.
\[ 2 \text{OH(g)} \rightarrow \text{H}_2\text{O}_2\text{(g)} \]
Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons.
### Diagrams:
**OH(g):**
- **Lewis Structure:** The diagram shows a hydroxyl radical (OH) with three lone pairs of electrons on the oxygen atom, and a single bond between oxygen and hydrogen.
**H₂O₂(g):**
- **Lewis Structure:** The diagram represents hydrogen peroxide with each oxygen atom bonded to a hydrogen atom. The two oxygen atoms are connected by a single bond. Both oxygen atoms have two lone pairs of electrons. The hydrogen atoms are bonded through single bonds to the oxygen atoms.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F726ba96a-8f61-467f-b06f-8b424ce252fa%2F5077013a-97e5-4b0a-b201-4da4a46184f2%2Fincslvi_processed.jpeg&w=3840&q=75)
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