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.