To identify the element based on the given electron configuration, we need to carefully count the total number of electrons that occupy the various subshells.
Here is a detailed breakdown of the configuration provided:
1. \(1s\): The \(\uparrow\downarrow\) symbol indicates that the 1s subshell is filled with 2 electrons.
2. \(2s\): The \(\uparrow\downarrow\) symbol indicates that the 2s subshell is filled with 2 electrons.
3. \(2p\): The \(\uparrow\downarrow \uparrow\downarrow \uparrow\downarrow\) symbol indicates that the 2p subshell is filled with 6 electrons.
4. \(3s\): The \(\uparrow\downarrow\) symbol indicates that the 3s subshell is filled with 2 electrons.
5. \(3p\): The \(\uparrow\downarrow \uparrow\downarrow \uparrow\) symbol indicates that the 3p subshell has 5 electrons.
Next, we sum up the number of electrons in each subshell:
[tex]\[
2 \text{ (from 1s)} + 2 \text{ (from 2s)} + 6 \text{ (from 2p)} + 2 \text{ (from 3s)} + 5 \text{ (from 3p)} = 17 \text{ electrons}
\][/tex]
An element with 17 electrons has an atomic number of 17. By referring to the periodic table, the element with atomic number 17 is Chlorine.
Finally, we need to match the element Chlorine with the given options:
- Astatine
- Bromine
- Chlorine
- Fluorine
The correct choice is Chlorine. Thus, the element with the given electron configuration is Chlorine.
