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प्रश्न
Elements forming ionic compounds attain noble gas configuration by either gaining or losing electrons from their outermost shells. Give reason to explain why carbon cannot attain noble gas configuration in this manner to form its compounds.
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उत्तर
The atomic number of carbon is 6. This means that it has 4 electrons in its outermost shell and it needs 4 more electrons to attain noble gas electronic configuration. It cannot form C4+ cation, as the removal of 4 valence electrons requires a huge amount of energy. The cation formed has 6 protons and 2 electrons. This makes it highly unstable. Carbon cannot form C4− anion, as its nucleus with 6 protons cannot hold 10 electrons. Thus, carbon achieves noble gas electronic configuration by sharing its 4 electrons with other elements—that is, it forms covalent compounds.
संबंधित प्रश्न
State the reason why carbon can neither form C4+ cations nor C4− anions but forms covalent compounds.
What is the difference between ionic compounds and covalent compounds?
State the type of bonding in the following molecule.
Methane
Choose the correct answer from the options given below
Condition favorable for formation of a covalent bond is
Explain the bonding in methane molecule using electron dot structure.
Explain the following:
Polar covalent compounds conduct electricity?
Complete the following activity.
Write the names of the hydrocarbons for the following structural formula.
(isobutylene, cyclohexane, propene, cyclohexene, cyclopentane, benzene, propyne, isobutane, propane)
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Complete the following activity.
Write the names of the hydrocarbons for the following structural formula.
(isobutylene, cyclohexane, propene, cyclohexene, cyclopentane, benzene, propyne, isobutane, propane)
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An element A is soft and can be cut with a knife. This is very reactive to air and cannot be kept open in air. It reacts vigorously with water. Identify the element from the following
The electron dot structure of chlorine molecule is:
