To determine which element corresponds to the electron configuration [tex]\(1s^2 2s^2 2p^6 3s^2 3p^4\)[/tex], let's break down the configuration step-by-step:
1. Count the electrons:
- [tex]\(1s^2\)[/tex]: The 1s orbital contains 2 electrons.
- [tex]\(2s^2\)[/tex]: The 2s orbital contains 2 electrons.
- [tex]\(2p^6\)[/tex]: The 2p orbitals collectively contain 6 electrons.
- [tex]\(3s^2\)[/tex]: The 3s orbital contains 2 electrons.
- [tex]\(3p^4\)[/tex]: The 3p orbitals collectively contain 4 electrons.
2. Sum the electrons:
[tex]\[
2 (from \, 1s) + 2 (from \, 2s) + 6 (from \, 2p) + 2 (from \, 3s) + 4 (from \, 3p) = 16 \, electrons
\][/tex]
3. Identify the element:
Elements are defined by their atomic number, which is equal to the number of protons in their nucleus. Since a neutral atom has an equal number of electrons and protons, we can determine the element by looking at its atomic number. An element with 16 electrons must have an atomic number of 16.
4. Match the atomic number to the element:
- Atomic Number 16 corresponds to Sulfur (S).
Therefore, the element with the electron configuration [tex]\(1s^2 2s^2 2p^6 3s^2 3p^4\)[/tex] is Sulfur.
The correct answer is:
B. [tex]\( S \)[/tex]
