Question

One of an atom shows eight electrons in the ringside representative for energy levels. How many electrons are in each energy level

Answer 1

The distribution of electrons in energy levels (or shells) around an atom follows a specific pattern based on the quantum model of the atom. Each energy level can hold a maximum number of electrons given by the formula \(2n^2\), where \(n\) is the energy level number (or shell).

Here is how the first few energy levels are filled:

1. **First energy level (n=1)**:
- Maximum electrons: \(2(1^2) = 2\)
- Electrons: 2

2. **Second energy level (n=2)**:
- Maximum electrons: \(2(2^2) = 8\)
- Electrons: 8

3. **Third energy level (n=3)**:
- Maximum electrons: \(2(3^2) = 18\)
- Electrons: Typically has 8 before moving to the fourth level.

4. **Fourth energy level (n=4)**:
- Maximum electrons: \(2(4^2) = 32\)
- Electrons: Additional electrons will fill this level after the third level.

If there are a total of 8 electrons indicated for an atom, they would be distributed as follows:

- The **first energy level** would hold its maximum of **2 electrons**.
- The **second energy level** would hold the **next 6 electrons** (since it can hold 8, but we only need to place 6 more to reach a total of 8).

In summary:
- **First energy level:** 2 electrons
- **Second energy level:** 6 electrons
- **Third energy level:** 0 electrons

Thus, for an atom with a total of **8 electrons**, this is the distribution: **2 in the first level and 6 in the second.**