Question

Написать электронные формулы ионов cu(2+) S(2-) Sr(2+)

Answer 1

Cu2+   1s2 2s2 2p6 3s2 3p6 4s0 3d9
S2-      1s2 2s2 2p6 3s2 3p6
Sr2+    1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

Answer 2

Electron Configurations of Cu(2+), S(2-), and Sr(2+)

The electron configurations of ions can be determined by considering the number of electrons gained or lost by the neutral atom. Here are the electron configurations for Cu(2+), S(2-), and Sr(2+):

- Cu(2+): Copper (Cu) has an atomic number of 29, and its neutral atom has the electron configuration 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^10. When it loses two electrons to become Cu(2+), the electron configuration becomes 1s^2 2s^2 2p^6 3s^2 3p^6 3d^9. - S(2-): Sulfur (S) has an atomic number of 16, and its neutral atom has the electron configuration 1s^2 2s^2 2p^6 3s^2 3p^4. When it gains two electrons to become S(2-), the electron configuration becomes 1s^2 2s^2 2p^6 3s^2 3p^6. - Sr(2+): Strontium (Sr) has an atomic number of 38, and its neutral atom has the electron configuration 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2. When it loses two electrons to become Sr(2+), the electron configuration becomes 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 4p^6.

Please note that the electron configurations provided above are based on the information available from the search results.