1. Write the electron configuration for each atom or ion. Then explain the distribution of electrons among energy levels.
Ca, Be2+, and Br-
I already found the electron configurations but I don't understand the second part of the question.(Then explain the distribution of electrons among energy levels.)
The electron configuration refers to the arrangement of electrons in an atom or ion. Each electron occupies an energy level, also known as an electron shell. The distribution of electrons among energy levels is determined by the order of filling according to the Aufbau principle, which states that electrons fill the lowest energy levels first before moving to higher ones. The specific distribution for each atom or ion is as follows:
1) Calcium (Ca):
The electron configuration for calcium (Ca) is 1s2 2s2 2p6 3s2 3p6 4s2. This indicates that the first energy level (n = 1) contains 2 electrons, the second energy level (n = 2) contains 8 electrons, and the third energy level (n = 3) contains 8 electrons. The last two electrons occupy the 4s orbital.
2) Beryllium ion (Be2+):
Beryllium (Be) has an electron configuration of 1s2 2s2. When it loses two electrons to become a Be2+ ion, the electron configuration becomes 1s2. As a result, the Be2+ ion only has electrons in the first energy level (n = 1), which contains 2 electrons.
3) Bromide ion (Br-):
Bromine (Br) has an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5. When it gains one electron to become a Br- ion, the electron configuration becomes 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6. The last electron gained occupies the 4p orbital, resulting in a full set of electrons in the fourth energy level (n = 4), with a total of 18 electrons.
In summary, the distribution of electrons among energy levels follows the Aufbau principle, filling the lowest energy levels first before moving to higher ones.
To understand the distribution of electrons among energy levels, it is essential to have a basic understanding of electron configuration. Electron configuration refers to the arrangement of electrons within an atom or ion in its ground state, indicating how they occupy various energy levels, sublevels, and orbitals.
In terms of the distribution of electrons among energy levels, we can consider the principle energy levels, also known as shells. These are represented by the numbers 1, 2, 3, and so on. Each energy level can hold a specific maximum number of electrons, given by the formula 2n^2, where "n" represents the principal energy level.
1. Calcium (Ca) has an electron configuration of 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2. In this case, the electron distribution can be understood as follows:
- The first shell (n = 1) can hold a maximum of 2 electrons, which are found in the 1s orbital.
- The second shell (n = 2) can hold a maximum of 8 electrons, which are split between the 2s and 2p orbitals.
- The third shell (n = 3) can also hold a maximum of 8 electrons, with the 3s and 3p orbitals filled.
- Finally, in the fourth shell (n = 4), we find the remaining 2 electrons in the 4s orbital.
2. Beryllium ion (Be2+) has an electron configuration of 1s^2. Here, the electron distribution can be explained as follows:
- The first shell (n = 1) still holds a maximum of 2 electrons, which are found in the 1s orbital in the ground state Be atom.
- However, the Be2+ ion has lost two electrons, which means it now only has the two electrons filling the 1s orbital.
3. Bromide ion (Br-) has an electron configuration of 1s^2 2s^2 2p^6 3s^2 3p^6. Let's understand the electron distribution:
- Starting from the first shell (n = 1), there are 2 electrons in the 1s orbital.
- In the second shell (n = 2), there are 2 electrons in the 2s orbital and 6 electrons in the 2p orbitals.
- In the third shell (n = 3), there are 2 electrons in the 3s orbital and 6 electrons in the 3p orbitals.
By understanding the electron configurations, we can see how the available energy levels (shells) are occupied by electrons, following the principle that they fill up from lower to higher energy levels and from lower to higher sublevels within the same energy level.