Question

Carbon burns in air and forms two oxides $ CO $ and $ C{O_2} $ .This shows that carbon has:
A. Two allotropic forms
B. Two oxidation states
C. Two isotopes
D. $ 4 $ electrons in valence shell

Answer 1

Hint: Oxides are binary chemicals formed when oxygen reacts with other elements. In nature, oxygen is a highly reactive gas. They form oxides when they react with metals and non-metals. The carbon group elements of the modern periodic table are also known as group 14 elements. In their outermost shell, these elements have four valence electrons.

Complete answer:
 $ C(s) + {O_2} \to C{O_2} $
Here oxidation state of carbon is $ + 4 $
Carbon burns in oxygen to form carbon dioxide.
When the oxygen supply is limited, combustion is incomplete, and carbon monoxide is produced.
 $ 2C + {O_2} \to 2CO $
Here the oxidation state of carbon is $ + 2 $ .
Hence, the correct option is B. Two oxidation states.

Additional Information:
Carbon monoxide ( $ CO $ ) is a poisonous gas. It is colourless and odourless. It's a combustible gas that's used to make a variety of inorganic and organic compounds. Carbon monoxide is an essential industrial gas since it is used in the production of a variety of organic and inorganic chemicals. It keeps packed meat fresh in modified environment packaging methods.
In nature, carbon dioxide is a colourless and odourless gas. It is critical to the survival of life on the planet. Although this gas is only found in tiny amounts in the environment, it is extremely important.
Carbon dioxide is used in a variety of industries, including the oil and food industries, as well as the chemical industry. It is used in the production of urea in a variety of chemical processes.

Note:
When certain substances react with oxygen, they generate oxides that are neither acidic nor basic. The term "neutral oxygen compounds" refers to such substances. Carbon monoxide is a neutral compound.