The fourth row of the periodic table has transition metals ranging from scandium (21) to zinc (30).Īhh, the transition metals. Remember that the first eight were placed during our trip through the third period/row. For the fourth period/row, all of these electrons build the third shell to a maximum of 18 electrons. This element is one of the transition elements that doesn't place the additional electrons in the outer shell, but in the one underneath. So remember when you look at our breakdown that the electrons aren't always in a nice neat order as shown here. They are found in clouds that can have different shapes that include spheres and dumbbell-like shapes. As you learn more about atomic structure, you will learn that the electrons don't stay in defined areas around the nucleus. The electrons like to be in separate shells/orbitals. In an atom, the electrons spin around the center, also called the nucleus. Each of those colored balls is an electron. If you think this is a little over your head, go back and look at the elements 1-18 that have organizations that are a little more simple. Let's take a look at the arrangements of electrons in the basic elements (left and right sides of the table) of period four and the more complex arrangements of the transition elements (in the middle of the row). You may have an easy way to know the number of electrons in a neutral atom, but the placement of those electrons gets a little more complex.

Now we're working with the fourth period/row in the table of elements. It tells you the mass of one atom, how many pieces are inside, and where it should be placed on the periodic table. That box on the left has all of the information you need to know about one element.

Sc electron configuration