Which of the following molecules contains the fewest covalent bonds?
A.
Chlorine molecule
B.
Ammonia molecule
C.
Methane molecule
D.
Water molecule
The correct answer and Explanation is :
The molecule that contains the fewest covalent bonds is A. Chlorine molecule (Cl₂).
Explanation:
To determine which molecule has the fewest covalent bonds, let’s analyze each option:
- Chlorine molecule (Cl₂): This diatomic molecule consists of two chlorine atoms bonded together by a single covalent bond. Each chlorine atom contributes one electron to form this bond, resulting in a total of one covalent bond.
- Ammonia molecule (NH₃): Ammonia consists of one nitrogen atom bonded to three hydrogen atoms. The nitrogen atom forms three single covalent bonds with the three hydrogen atoms, leading to a total of three covalent bonds.
- Methane molecule (CH₄): Methane has one carbon atom bonded to four hydrogen atoms. The carbon forms four single covalent bonds, one with each hydrogen, resulting in a total of four covalent bonds.
- Water molecule (H₂O): Water consists of one oxygen atom bonded to two hydrogen atoms. The oxygen forms two single covalent bonds, one with each hydrogen atom, resulting in a total of two covalent bonds.
When comparing these molecules, it’s clear that the chlorine molecule (Cl₂) has the least number of covalent bonds, with just one bond. In contrast, ammonia has three, methane has four, and water has two.
Covalent bonds are formed when atoms share pairs of electrons, and the number of bonds typically correlates with the number of atoms involved and their bonding preferences. In this case, Cl₂ is unique as a diatomic molecule with a simple bond formation, making it the simplest in terms of bonding complexity among the options provided.