Question

oxygen has _ valence electrons, therefore it always forms _ bonds.
o a 2 valence electrons, 6 bonds
o b 8 valence electrons, 0 bonds
o c 2 valence electrons, 2 bonds
o d 6 valence electrons, 2 bonds

Explanation:

Oxygen has an atomic number of 8. Its electron configuration is \(1s^{2}2s^{2}2p^{4}\). The valence electrons are in the \(n = 2\) shell. The number of valence electrons is \(2 + 4=6\). Oxygen needs 2 more electrons to complete its octet (following the octet rule). So, it forms 2 covalent bonds (by sharing electrons) to achieve a stable electron configuration.

Answer:

d. 6 valence electrons, 2 bonds