Question

for each nonmetal below, identify how many covalent bonds (shared electron pairs) it forms with other atoms to fill its valence shell. element number of covalent bonds h c n 1 o 2 f 3 4 show periodic table

Explanation:

• Hydrogen (\(H\)) has \(1\) valence electron. It needs \(1\) more electron to fill its valence shell (duet rule, as the first shell can hold a maximum of \(2\) electrons). So, it forms \(1\) covalent bond.
• Carbon (\(C\)) has \(4\) valence electrons. It needs \(4\) more electrons to fill its valence shell (octet rule, as the second - shell can hold a maximum of \(8\) electrons). So, it forms \(4\) covalent bonds.
• Nitrogen (\(N\)) has \(5\) valence electrons. It needs \(3\) more electrons to fill its valence shell (octet rule). So, it forms \(3\) covalent bonds.
• Oxygen (\(O\)) has \(6\) valence electrons. It needs \(2\) more electrons to fill its valence shell (octet rule). So, it forms \(2\) covalent bonds.
• Fluorine (\(F\)) has \(7\) valence electrons. It needs \(1\) more electron to fill its valence shell (octet rule). So, it forms \(1\) covalent bond.

Answer:

Element	Number of covalent bonds
\(C\)	\(4\)
\(N\)	\(3\)
\(O\)	\(2\)
\(F\)	\(1\)