Below is the Lewis structure of the bicarbonate (HCO3) ion. :0: H:O:C:0: Count the number of bonding pairs and the number of lone pairs around the right oxygen atom in this molecule. bonding pairs: lone pairs: X
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.
![Below is the Lewis structure of the bicarbonate (\( \text{HCO}_3^- \)) ion.
\[
\begin{array}{c}
\quad & :\text{O}: & \\
\text{H} & ::\text{O}:\text{C}:\text{O}: & \\
\quad & \quad & \\
\end{array}
\]
Count the number of bonding pairs and the number of lone pairs around the right oxygen atom in this molecule.
**Explanation of the Diagram:**
The Lewis structure for the bicarbonate ion shows the arrangement of electrons around the atoms in the molecule. In this structure:
- Oxygen atoms are denoted with "\(:\text{O}:\)" where the dots represent the electron pairs.
- The central atom is carbon, shown as "\text{C}".
- The hydrogen atom is written as "\text{H}" bonded to one of the oxygens.
- The structure is enclosed in square brackets to indicate it is an ion with a negative charge.
**Task:**
Count the bonding pairs and lone pairs of electrons around the right oxygen atom.
- **Bonding pairs:** The number of shared electron pairs connecting atoms.
- **Lone pairs:** The number of electron pairs not involved in bonding on the right oxygen atom.
Boxes are provided to input your answer for bonding pairs and lone pairs.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0f3ffac2-6c59-474a-a434-564154eba462%2F54873683-40f1-4d6d-8984-8e3f7bd6a11f%2Fiovfhp_processed.jpeg&w=3840&q=75)
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