Question

how many protons, neutrons, and electrons are in this ion? 33 16 s - 2 16 p ^ { + }, 17 n ^ { 0 }, 18 e ^ { - } 16 p ^ { + }, 17 n ^ { 0 }, 16 e ^ { - } 16 p ^ { + }, 33 n ^ { 0 }, 16 e ^ { - } 33 p ^ { + }, 16 n ^ { 0 }, 35 e ^ { - }

Explanation:

Step1: Determine the number of protons

The atomic number (subscript) of sulfur (\(S\)) is \(16\). The number of protons (\(p^{+}\)) is equal to the atomic number. So, \(p^{+}=16\).

Step2: Determine the number of neutrons

The mass number (superscript) is \(33\). The formula for the number of neutrons (\(n^{0}\)) is \(n^{0}=\text{Mass number}-\text{Atomic number}\). So, \(n^{0}=33 - 16=17\).

Step3: Determine the number of electrons

The ion has a charge of \(- 2\). For a neutral atom, the number of electrons (\(e^{-}\)) is equal to the number of protons. Since the ion has a charge of \(-2\) (it has gained \(2\) electrons), \(e^{-}=16 + 2=18\).

Answer:

\(16\ p^{+},17\ n^{0},18\ e^{-}\) (the first option)