Question

Carbon shows tetravalency due to: (a) Dsp \(^{2}\) hybridisation (b) \(\mathrm{Sp}^{3}\) hybridisation (c) \(\mathrm{S}^{2} \mathrm{p}^{2}\) hybridisation (d) \(\mathrm{D}^{3} \mathrm{p}\) hybridisation

Short answer

Carbon shows tetravalency due to \\(\mathrm{sp}^{3}\\) hybridisation.

Step-by-step solution

Understanding Tetravalency

Tetravalency refers to the ability of an atom to form four covalent bonds. Carbon typically forms four covalent bonds to achieve a stable electronic configuration resembling that of a noble gas.

Identifying Carbon's Electronic Configuration

Carbon has an atomic number of 6, with an electronic configuration of \(1s^2 2s^2 2p^2\). The four valence electrons (two in the 2s subshell and two in the 2p subshell) are involved in bonding.

Hybridization Concept

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals. These hybrid orbitals have properties that are intermediate between the original orbitals and are used to form covalent bonds.

Determining the Correct Hybridization

Carbon exhibits \( ext{sp}^3\) hybridization when all four valence orbitals (one 2s and three 2p orbitals) mix to form four equivalent \( ext{sp}^3\) hybrid orbitals, each containing one electron for bonding. This accounts for carbon's tetravalency.

Key concepts

sp3 Hybridization

Carbon is a versatile element known for its ability to form four stable bonds. This property is due to a concept known as sp^3 hybridization. In this process, one s orbital and three p orbitals in carbon's outer shell mix together. The result of this blending is the formation of four equivalent sp^3 hybrid orbitals. Each of these orbitals contains one electron which can be shared with other atoms. This sharing leads to the formation of covalent bonds.
The idea of hybridization helps explain carbon's ability to form complex structures, such as chains and rings in organic compounds. It provides the flexibility for carbon to connect with various elements, creating diverse chemical compounds. By understanding sp^3 hybridization, students can begin to appreciate the central role carbon plays in chemistry and life itself.

Covalent Bonding

Covalent bonding is at the heart of carbon's chemistry. This type of bond involves the sharing of electron pairs between atoms. Carbon, with its four valence electrons, aims to complete its outer shell by sharing electrons with other atoms. In this way, it satisfies the octet rule, whereby atoms strive for an electronic arrangement similar to that of a noble gas.
Through covalent bonding, carbon can form strong stable connections. This is why many carbon-containing compounds, such as hydrocarbons and proteins, are so stable in nature. The number of covalent bonds an atom forms depends on how many electrons it can share or accept to complete its outer electron shell. Carbon's ability to establish four covalent bonds is due to its tetravalency, allowing it to form a variety of complex compounds. Understanding covalent bonding is essential to grasp how carbon forms diverse and essential chemical structures.

Electronic Configuration

Electronic configuration gives a detailed account of an atom's electron arrangement within its orbitals. For carbon, the electronic configuration is denoted as 1s^2 2s^2 2p^2. This means:

• The 1s energy level holds two electrons.
• The 2s energy level also holds two electrons.
• Finally, there are two electrons in the 2p orbitals.

This configuration highlights the four electrons carbon has available for bonding in its second shell, which is crucial for its chemical behavior. During chemical reactions, these valence electrons can be shared or exchanged to form bonds with other atoms. Carbon strives to reach a full outer shell similar to noble gases by engaging in covalent bonding. Mastering electronic configuration enables students to predict how atoms like carbon will interact to form chemical bonds and structures.

Valence Electrons

Valence electrons are the electrons found in the outermost shell of an atom and are significant in forming chemical bonds. For carbon, it has four valence electrons, located in the second shell: two in the 2s orbital and two in the 2p orbitals. These electrons are vital for chemical reactions because they can be shared or transferred to other atoms to form bonds.
Carbon aims to use its valence electrons to fill its outer shell, achieving a configuration like a noble gas with eight electrons. This action results in the formation of covalent bonds, which are fundamental to the structure of molecules like carbohydrates and DNA. The behavior of these valence electrons underpins much of carbon's chemistry, making it versatile and capable of forming a vast array of complex structures. By understanding the role of valence electrons in this context, students can better comprehend the mechanisms of chemical bonding and predict the interactions of carbon atoms within molecules.