what is the electron configuration for Au+ ?
where does f block fit in?
There is a 4f series and a 5f series. The 4f series (what I call the Lanthanide series) has the first 4f electron (actually two of them) enter at Ce (#58). The 5f series has the first 5f electron (actually two of them) entering at Pa(#91).
To determine the electron configuration for Au+, we first need to know the electron configuration of neutral gold (Au). The electron configuration of neutral gold is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6.
When gold loses one electron to form Au+, one electron is removed from the 6s orbital since it is the outermost orbital. Therefore, the electron configuration for Au+ would be 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^1.
Next, let's talk about the f block. The f block, also known as the inner transition metals, consists of two rows of elements located at the bottom of the periodic table. These elements belong to the lanthanide series (atomic numbers 57-71) and the actinide series (atomic numbers 89-103).
The f block elements have their electron configurations characterized by the filling of the 4f and 5f orbitals. These orbitals are part of the f sublevel, which is one of the seven sublevels (s, p, d, f, g, h, i) that make up the electron arrangement around the nucleus.
In terms of fitting in the periodic table, the f block is typically shown separately at the bottom of the periodic table to conserve space. This allows for a more compact representation of the periodic table while still including all the elements and their information.
To find the electron configuration of elements in the f block, you'll need to know the specific element and its corresponding atomic number. Using the rules for filling orbitals, you can determine the order in which electrons fill the f orbitals to write the electron configuration.