Answer :
To determine the name of an element based on its electron configuration, we need to carefully analyze the given electron configuration and match it with the correct element. Here is the step-by-step process:
1. Write Down the Given Electron Configuration:
[tex]\[ 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^5 \][/tex]
2. Total the Number of Electrons:
- \(1s^2\): 2 electrons
- \(2s^2\): 2 electrons
- \(2p^6\): 6 electrons
- \(3s^2\): 2 electrons
- \(3p^6\): 6 electrons
- \(4s^2\): 2 electrons
- \(3d^{10}\): 10 electrons
- \(4p^6\): 6 electrons
- \(5s^2\): 2 electrons
- \(4d^{10}\): 10 electrons
- \(5p^5\): 5 electrons
3. Add the Electrons:
[tex]\[ 2 + 2 + 6 + 2 + 6 + 2 + 10 + 6 + 2 + 10 + 5 = 53 \text{ electrons} \][/tex]
4. Determine the Element:
- The element with 53 electrons in its neutral state has an atomic number of 53.
5. Identify the Element on the Periodic Table:
- The element with atomic number 53 is iodine (I).
Therefore, based on the electron configuration, the element is iodine. The answer is:
[tex]\[ \boxed{\text{iodine}} \][/tex]
1. Write Down the Given Electron Configuration:
[tex]\[ 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^5 \][/tex]
2. Total the Number of Electrons:
- \(1s^2\): 2 electrons
- \(2s^2\): 2 electrons
- \(2p^6\): 6 electrons
- \(3s^2\): 2 electrons
- \(3p^6\): 6 electrons
- \(4s^2\): 2 electrons
- \(3d^{10}\): 10 electrons
- \(4p^6\): 6 electrons
- \(5s^2\): 2 electrons
- \(4d^{10}\): 10 electrons
- \(5p^5\): 5 electrons
3. Add the Electrons:
[tex]\[ 2 + 2 + 6 + 2 + 6 + 2 + 10 + 6 + 2 + 10 + 5 = 53 \text{ electrons} \][/tex]
4. Determine the Element:
- The element with 53 electrons in its neutral state has an atomic number of 53.
5. Identify the Element on the Periodic Table:
- The element with atomic number 53 is iodine (I).
Therefore, based on the electron configuration, the element is iodine. The answer is:
[tex]\[ \boxed{\text{iodine}} \][/tex]
