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Why does carbon make a stable compound?
Due to big size carbon forms strong bonds.
Due to small size carbon forms strong bonds.
Due to higher electronegativity carbon forms strong bonds.
Due to higher enthalpy carbon forms strong bonds.
Due to small size carbon forms strong bonds.
Carbon forms stable compounds primarily because of its small atomic size, which allows its valence electrons to be held strongly by the nucleus, facilitating strong covalent bonding. This compact structure leads to a high degree of orbital overlap, resulting in very stable and robust single, double, and triple bonds.
Carbon forms stable compounds primarily because of its small atomic size, which allows its valence electrons to be held strongly by the nucleus, facilitating strong covalent bonding. This compact structure leads to a high degree of orbital overlap, resulting in very stable and robust single, double, and triple bonds.
Think of a handshake between two people with short arms; they can hold onto each other much more tightly and securely than two people with very long, lanky arms, where the grip is easier to break.
SMALL: Strong, Mighty, And Long-lasting Linkage
EbondтАЛтИЭr21тАЛ тАФ where EbondтАЛ is bond energy and r is the bond length
CnтАЛH2n+2тАЛ тАФ the general formula for stable alkanes
In a covalent bond, stability is determined by the extent of orbital overlap. Because carbon has a small atomic radius, the bonding electrons are closer to the nucleus, creating a strong electrostatic attraction. This leads to shorter bond lengths and higher bond dissociation energies, such as the C-C bond energy being approximately 347┬аkJ/mol, which is significantly higher than that of larger group 14 elements like silicon.
Small atomic size permits effective overlapping of atomic orbitals.
Carbon's unique ability to form catenation is linked to the stability of its C-C bond.
Strong covalent bonds are a result of the high electron density between the bonded nuclei.
High thermal stability of organic molecules
Diversity of chemical structures due to catenation
Requires high energy to break bonds in chemical reactions
Formation of long-chain hydrocarbons (polymers)
Biological structural integrity in proteins and DNA
Bond dissociation energy of C-C is тЙИ347┬аkJ/mol, while Si-Si is тЙИ226┬аkJ/mol.
Option A is incorrect because large size decreases orbital overlap, weakening the bond.
Option C is incorrect because while electronegativity matters, the primary physical driver for stability in this context is the bond length/size relationship.
Option D is incorrect as higher enthalpy usually refers to the system state, not the bond stability itself.
B is correct тАФ Carbon's small size allows for closer proximity between bonding nuclei, resulting in stronger orbital overlap and more stable covalent bonds.
Always remember: In periodic trends, smaller atoms in the same group generally form stronger covalent bonds with themselves because the bonding electrons are closer to both nuclei.
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