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[tex]\[1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^{10} \, 4p^5\][/tex]

Which element is this?

\begin{tabular}{|l|}
\hline
fluorine [tex]\((F)\)[/tex] \\
bromine [tex]\((Br)\)[/tex] \\
chlorine [tex]\((Cl)\)[/tex] \\
krypton [tex]\((Kr)\)[/tex] \\
\hline
\end{tabular}



Answer :

GinnyAnswer
To determine which element corresponds to the electron configuration provided, we need to carefully analyze it step-by-step:

[tex]\[ 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^5 \][/tex]

This configuration indicates the distribution of electrons in various orbitals. Let's summarize the given configuration:

1. 1st Energy Level:
- [tex]\( 1s^2 \)[/tex]: 2 electrons

2. 2nd Energy Level:
- [tex]\( 2s^2 \)[/tex]: 2 electrons
- [tex]\( 2p^6 \)[/tex]: 6 electrons

3. 3rd Energy Level:
- [tex]\( 3s^2 \)[/tex]: 2 electrons
- [tex]\( 3p^6 \)[/tex]: 6 electrons
- [tex]\( 3d^{10} \)[/tex]: 10 electrons

4. 4th Energy Level:
- [tex]\( 4s^2 \)[/tex]: 2 electrons
- [tex]\( 4p^5 \)[/tex]: 5 electrons

To find the element, we add up all the electrons:

[tex]\[ 2 + 2 + 6 + 2 + 6 + 2 + 10 + 5 = 35 \][/tex]

This total indicates that we are dealing with an element that has an atomic number of 35. Looking at the periodic table, the element with atomic number 35 is bromine (Br).

Thus, the correct answer to which element the given electron configuration corresponds is:

[tex]\[ \boxed{\text{bromine (Br)}} \][/tex]

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