This section probably won't make much sense if you haven't read Electron Shells and Electron Configuration. This will also help explain why certain members of the d-block aren't classified as transition metals.
We'll start with their electron configuration as atoms, and then look at how this changes as they form ions. Electron configuration of transition metals The transition metals can be found in groups 3-12 and periods 4-7, although what's more crucial is that they can be easily located in the periodic table. The highest energy subshell in the d-block is always a d-subshell. You can find the transition metals in the middle of the d-block section of the periodic table, which acts as a link between the s- and p-blocks. However, for this article, we will be focusing solely on the elements highlighted in blue above, as defined by IUPAC. Additionally, there are two other groups of elements called the lanthanides and actinides, with atomic numbers 57-71 and 89-103 respectively, which are sometimes referred to as inner transition metals.
The reason for this will be discussed later on. It's important to note that not all elements in the d-block are transition metals, despite the term being used interchangeably. Periodic table of elements with transition metals highlighted
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