Final answer:
Methane, ethene, ethyne, and benzene are hydrocarbons where each carbon atom has four covalent bonds, accordingly fulfilling carbon's bonding requirements. They exemplify single, double, triple, and resonance bonds respectively, each maintaining the overall stability of the molecule by following the octet rule.
Step-by-step explanation:
The question asks about carbon bonding in organic molecules, specifically which molecules show an appropriate number of bonds around each carbon atom. Carbon is renowned for its ability to form four covalent bonds due to its four electrons in the outer shell, satisfying the octet rule. This allows it to bond with other atoms, including hydrogen, to form stable compounds.
Methane (CH4), ethene (C2H4), ethyne (C2H2), and benzene (C6H6) are all examples of hydrocarbons that feature carbon atoms with four bonds each, correctly adhering to carbon's bonding rule.
However, these molecules exhibit different types of bonds; methane has four single bonds, ethene contains a double bond between the two carbon atoms, ethyne includes a triple bond between its carbon atoms, and benzene presents a unique case with alternating single and double bonds in a ring structure, known as resonance.
Each of these molecules satisfies the condition that every carbon atom makes four bonds, which could be a combination of single, double, and triple bonds. Therefore, methane, ethene, ethyne, and benzene indeed show an appropriate number of bonds around each carbon atom. They all obey the octet rule, where each carbon atom is involved in four bonds, achieving a stable configuration.