Question

which statement best explains why carbon bonds to four hydrogen atoms to form methane but to only two oxygen atoms to form carbon dioxide? (1 point) hydrogen shares electrons with carbon, but oxygen transfers its electrons. the carbon in carbon dioxide is stable, with fewer valence electrons than the carbon in methane. hydrogen shares one valence electron with carbon, and oxygen shares two valence electrons. the carbon in methane has more valence electrons to share than the carbon in carbon dioxide.

Explanation:

Carbon has four valence electrons. In methane ($CH_4$), each hydrogen atom shares one valence electron with carbon. Since hydrogen has one valence electron, four hydrogen atoms are needed (1×4 = 4) to complete carbon's valence shell (carbon's four valence electrons + four from hydrogen = eight, achieving a stable octet). In carbon dioxide ($CO_2$), each oxygen atom shares two valence electrons with carbon. Oxygen has six valence electrons and needs two more to complete its octet. Carbon shares two electrons with each oxygen atom (2×2 = 4, and carbon's four valence electrons are all used). So the number of atoms carbon bonds with depends on how many valence electrons the other atom shares. Option A is wrong because both hydrogen and oxygen share electrons (covalent bonds in $CH_4$ and $CO_2$). Option B is wrong as carbon in both $CH_4$ and $CO_2$ has a full valence shell (eight electrons). Option D is wrong as carbon has four valence electrons in both compounds.

Answer:

C. Hydrogen shares one valence electron with carbon, and oxygen shares two valence electrons.