The electron configuration below represents a ground-state atom of which element? 1s22s22p63s23p4
Answer:
Sulfur
Explanation:
There are two ways to get the answer.
1. Count the electrons.
The electron configuration is 1s² 2s²2p⁶ 3s²3p⁴.
The numbers in the superscripts tell you how many electrons are in each subshell.
They add up to 16, and element 16 is sulfur.
2. Look at the outermost shell.
The outermost shell has the electron configuration 3s²3p⁴.
This tells you that the element is in Period 3 and has six valence electrons.
Start at the left of Period 3 (Na). Count six places to the right, and you come to sulfur.
The given electronic configuration has been representing the ground state of sulfur atom.
The electronic configuration has been the electron address in an atom. It has been the representation of the number of electrons present in the quantum subshell of each shell.
The number of electrons has been calculated with the superscript of each quantum level. The number of electrons in the given electronic configuration has been given as:
[tex]\rm Electrons=2+2+6+2+4\\Electrons=16[/tex]
The number of electrons in the sample has been a representation of the atomic number of the element. The number of electrons in the given sample has been 16. Thus, the atomic number of the sample has been 16.
The element with 16 atomic number is Sulfur. Thus, the given electronic configuration has been representing the ground state of sulfur atom.
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