The electron configuration of \(A_{1}^{3-}\) is \(1s^2 2s^2 2p^6\). \(A_{1}\) atom belongs to row 2, column 16. The atom and ion have different electron configurations. When \(A_{1}\) (6 valence electrons) reacts with Cl (17 electrons), they form an ionic bond, resulting in \(A_{1}^{3-}Cl^{-}\).
1) The electron configuration of \(A_{1}^{3-}\) is given as \(K^2, L^{3}\). Let's break this down:
- \(K^2\) represents the electron configuration of the K shell (the first shell), which has 2 electrons.
- \(L^{3}\) represents the electron configuration of the L shell (the second shell), which has 3 electrons.
So, combining these, the electron configuration of \(A_{1}^{3-}\) is \(1s^2 2s^2 2p^6\).
Now, to find the electron configuration of \(A_{1}\) (neutral atom), you would simply remove the three extra electrons. Therefore, the electron configuration of \(A_{1}\) is \(1s^2 2s^2 2p^4\).
2) Let's evaluate the statements:
a. \(A_{1}\) atom belongs to row 2, column 18.
This statement is false. Elements in row 2 are the second period elements (having electron shells numbered 1 and 2), and column 18 corresponds to the noble gases. However, \(A_{1}\) is not a noble gas. The element \(A_{1}\) would be found in row 2, column 16, as it would be in group 16 (or VIA) of the periodic table.
b. \(A_{1}\) atom and its corresponding ion have the same electron configuration.
This statement is false. \(A_{1}\) atom has an electron configuration of \(1s^2 2s^2 2p^4\). If \(A_{1}\) loses three electrons to form \(A_{1}^{3-}\), the electron configuration of the ion becomes \(1s^2 2s^2 2p^6\), as mentioned in the previous answer.
3) When \(A_{1}\) atom and Cl (with an atomic number of 17) combine to form a compound, they will likely form an ionic bond. \(A_{1}\) (with 6 valence electrons in the outer shell) tends to lose 3 electrons to achieve a stable electron configuration, while Cl tends to gain 1 electron to achieve a stable electron configuration.
The resulting compound would be \(A_{1}^{3-}Cl^{-}\). The \(A_{1}^{3-}\) ion has lost 3 electrons, and Cl has gained 1 electron. This combination results in a compound where there is an electrostatic attraction between the positively charged \(A_{1}^{3-}\) ion and the negatively charged Cl ion, forming an ionic bond.