Acetic acid (shown below) has a Ka that is much smaller, 1.8x10-º. Why is dichloroacetic acid a stronger acid than acetic acid? This statement is not true, acetic acid is a stronger acid than dichloroacetic acid. The chlorine atoms in dichloroacetic acid are very electronegative, withdrawing electrons from the rest of the molecule ultimately making the O-H bond weaker. The chlorine atoms withdraw electrons, ultimately from the O atoms making them positive which then repel H*. The chlorine atoms have more electrons than the hydrogen atoms and can donate these electrons to the rest of the molecule, weakening the O-H bond in dichloroacetic acid compared to acetic acid.
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.
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