what element has the following electron configuration: 1s22s22p63s23p64s13d5
What element has the following electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵?
Answer:
To determine which element corresponds to the given electron configuration, we need to count the total number of electrons and match this number to its atomic number on the periodic table.
Step 1: Electron Configuration Breakdown
The electron configuration provided is:
1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵
Let’s break it down by counting the electrons in each sub-shell:
- 1s²: 2 electrons
- 2s²: 2 electrons
- 2p⁶: 6 electrons
- 3s²: 2 electrons
- 3p⁶: 6 electrons
- 4s¹: 1 electron
- 3d⁵: 5 electrons
Now, we sum these electrons to find the total number:
2 (1s²) + 2 (2s²) + 6 (2p⁶) + 2 (3s²) + 6 (3p⁶) + 1 (4s¹) + 5 (3d⁵) = 25 electrons
Step 2: Identifying the Element
The element with 25 electrons is manganese (Mn), which has the atomic number 25 on the periodic table.
Step 3: Confirmation
You can confirm this by looking at the position of manganese in the periodic table:
- Manganese is in the 4th period (row) and part of the transition metals.
- The electron configuration for elements in this area often shows the filling of the 3d sub-shell after the 4s sub-shell has primary electrons, which aligns with the configuration provided in the problem.
Final Answer:
The element with the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵ is manganese (Mn).