If an element has the electronic configuration 1s\(^2\), 2s\(^2\), 2p\(^6\), 3s\(^2\), 3p\(^4\), it is
If an element has the electronic configuration 1s\(^2\), 2s\(^2\), 2p\(^6\), 3s\(^2\), 3p\(^4\), it is
- A) metal
- B) An alkaline earth metal
- C) An S-block element
- D) A P-block element
Correct Answer: D) A P-block element
Explanation
First, let's understand the electronic configuration given: 1s\(^2\), 2s\(^2\), 2p\(^6\), 3s\(^2\), 3p\(^4\). This configuration shows the distribution of electrons in the energy levels and sublevels of the element's atom.
To identify the element, we can add up the total number of electrons: 2 + 2 + 6 + 2 + 4 = 16 electrons. The element with 16 electrons is sulfur (S).
Now, let's analyze the options:
Option A: metal - Sulfur is a non-metal, so this option is incorrect.
Option B: An alkaline earth metal - Alkaline earth metals belong to Group 2 of the periodic table and have their outer electrons in the S sublevel (specifically, in the form of ns\(^2\). Sulfur does not fit this description, so this option is incorrect.
Option C: An S-block element - S-block elements are found in Groups 1 and 2 of the periodic table, and their outer electrons are in the S sublevel. Sulfur's outer electrons are in the 3p sublevel, so this option is incorrect.
Option D: A P-block element (Correct) - P-block elements are found in Groups 13-18 of the periodic table, and their outer electrons are in the P sublevel. Sulfur is in Group 16, and its outer electrons are in the 3p sublevel, so this option is correct.
In summary, an element with the electronic configuration 1s\(^2\), 2s\(^2\), 2p\(^6\), 3s\(^2\), 3p\(^4\) is sulfur, which is a P-block element.