The covalency of carbon in the carbon monoxide (CO) molecule is three primarily due to its ability to form multiple bonds with other atoms. Let's break down the options to understand why this is the case.
Understanding Carbon's Valence Electrons
Carbon has four valence electrons, which allows it to form bonds with other elements. In CO, carbon shares electrons with oxygen to achieve a stable configuration.
Analyzing the Options
- A. An unexcited carbon has two unpaired electrons: This is true, but it doesn't explain the covalency in CO.
- B. The carbon atom can be an acceptor of an electron pair: This is relevant, as carbon can accept electrons to form bonds.
- C. The carbon has four valence electrons: Correct, but it doesn't directly address the covalency in CO.
- D. Maximum covalency of carbon is three: This is incorrect; carbon can have a maximum covalency of four.
Conclusion on Covalency in CO
The correct reasoning lies in the fact that carbon can form a triple bond with oxygen in CO, which involves sharing three pairs of electrons. Thus, the covalency of carbon in CO is three, allowing it to achieve a stable electronic configuration.
