In what group of the periodic table is the element with the following configuration [Ar] 4s2 3d10 4p3
the number of electrons is 15 greater than Ar
... so the atomic number is also
I supposed the valence electron is 3 so it should be in the group 13 or 3A
you might want to find the element and check
Electrons feel an empty shell before they pair up with another electron; maybe that should help you figure out the correct group. You are close but not quite right.
If I look at the exact element it goes under group 5A. Then if I consider the valence electron it will be under group 3A. Im still confused.
To determine the group of an element in the periodic table based on its electron configuration, we need to focus on the outermost energy level, which is known as the valence shell.
The given electron configuration [Ar] 4s2 3d10 4p3 corresponds to the element chlorine (Cl). To identify its group, we need to consider the configuration of the outermost electrons, which in this case is 4s2 3d10 4p3.
The 4s2 part indicates that chlorine has two electrons in the 4s subshell. The 3d10 4p3 part means that it has ten electrons in the 3d subshell and three electrons in the 4p subshell.
Now, let's look at the periodic table. Chlorine is located in the third period (row) and belongs to Group 17 (also known as Group VIIA or Group 7). This group is called the halogens and includes elements such as fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At).
So, the element with the given electron configuration [Ar] 4s2 3d10 4p3 belongs to Group 17 (Group VIIA or Group 7) of the periodic table, which is the halogens.