Write the electron configuration of Sn and Sn2+
Give the electron configuration of Cu+ and Cu2+
Write the electron configuration for Sn2+.
Same response as before. If you still have a question, explain what it is that you don't undrestand.
What I don't understand is where I get the number of dots from and what is the electron configuration
You get the number of dots from the periodic table. For example, Na is Na. and Ba is Ba: (because Na is in group I and has 1 electrons in its outside shell and Ba is in group II and has 2 electrons in its outside shell). Cl is in group VII (or 17 depending upon which system you are using) and has 7 electrons in its outside shell.
The electron configuration is done following two rules.
2 s electrons, 6 p electrons, 10 d electrons, and 14 f electrons. The ORDER of filling is
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 which will get you through element 38. There are two exceptions in this chain; one is Cr and the other is Cu. The ground state of both Cr and Cu have 1 fewer electron in the 4s and 1 more electron in the 3d than the above scheme provides. Let me know if you still have questions about this but please be specific.
To find the electron configuration of an element and its ions, we need to understand the distribution of electrons in different energy levels and orbitals.
The electron configuration of Sn (Tin) is obtained by following the Aufbau principle, which states that electrons fill the lowest energy level available before moving to higher energy levels. The atomic number of Sn is 50, which means it has 50 electrons.
The electron configuration of Sn is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^2
To determine the electron configuration of Sn2+ (Tin ion with a +2 charge), we need to remove two electrons from the neutral Sn atom. We start removing electrons from the highest energy level, following the Aufbau principle. Therefore, the electron configuration for Sn2+ is: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 3d^10 4p^6.
Moving on to Cu (Copper), the atomic number is 29, which means it has 29 electrons.
The electron configuration of Cu is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^10
To find the electron configuration of Cu+ (Copper ion with a +1 charge), we need to remove one electron from the neutral Cu atom. We start removing electrons from the highest energy level, which is the 4s orbital. Therefore, the electron configuration for Cu+ is: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10.
Finally, we can determine the electron configuration of Cu2+ (Copper ion with a +2 charge) by removing two electrons from the neutral Cu atom. Similar to Cu+, we start removing electrons from the highest energy level, which is the 4s orbital. Therefore, the electron configuration for Cu2+ is: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^9.