The number of unpaired electrons and the element for [Xe]6s24f145d7:
I know the element is Iridium but I cannot figure out the unpaired electrons!
The number of unpaired electrons is 5.
To determine the number of unpaired electrons in an element, we need to look at the electron configuration. The electron configuration of iridium (Ir) is [Xe]6s24f145d7.
To find the number of unpaired electrons, we'll analyze the 5d subshell. The 5d subshell can contain a maximum of 10 electrons.
In this case, there are 7 electrons in the 5d subshell, which means 7 electrons are paired. The remaining 3 electrons in the 5d subshell are unpaired.
Therefore, the number of unpaired electrons in iridium (Ir) is 3.
To determine the number of unpaired electrons in an atom, you need to know its electron configuration. The electron configuration for Iridium (Ir) is [Xe]6s24f145d7, as you correctly stated.
To find the number of unpaired electrons, you need to consider the last energy level (principal quantum number) that contains electrons. In this case, it is the 5d orbital. The 5d orbital can hold a maximum of 10 electrons.
Since there are 7 electrons in the 5d orbital, we can determine the number of unpaired electrons by subtracting the number of electrons from the maximum capacity. Therefore, 10 - 7 = 3.
Hence, the number of unpaired electrons in Iridium is 3.