I do not understand anything about electron configuration. How do you figure out if the element is in P,D,S,orF? What do the subscripts represent? What is a subshell? I am so confused!!

You figure it out by using the Aufgau principle, placing electrons in the proper order in orbitals

I suggest a tutoring by another student on this, it is really simple, you are having undoubtably a mental block. It is rather difficult to teach on a text format.

It is really simple..

Here is an interactive site that may be of help. Bob Pursley found this and I saw it yesterday.
http://www.iun.edu/~cpanhd/C101webnotes/modern-atomic-theory/aufbau-principle.html

+WHAT IS THE ELECTRON CONFIGURATION FOR THE FOLLOWING ELEMENTS p,li,ca ga as

Hi i'm not sure if you still need the answers but here they are (in condensed form):

P: [Ne] 3s2 3p3
Li: [He] 2s1
Ca: [Ar] 4s2
Ga: [Ar] 3d10 4s2 4p1
As: [Ar] 3d10 4s2 4p3

Valance Electrons?

I hate chemistry

I understand that electron configuration can be confusing at first. It may take time and practice to fully grasp the concept. However, I can certainly explain the basics to help you understand.

The electron configuration of an element describes the arrangement of electrons in its atomic orbitals. The orbitals are organized into subshells, which are further divided into different types known as s, p, d, and f orbitals.

To determine which subshell an element belongs to, you need to refer to the periodic table. The main energy level or period of the element indicates the principal quantum number (n). For example, elements in the first period (n = 1) belong to the first energy level, elements in the second period (n = 2) belong to the second energy level, and so on.

Next, you determine the type of subshell within the energy level using the azimuthal quantum number (l) values. The l values correspond to different orbitals: s (l = 0), p (l = 1), d (l = 2), and f (l = 3). So, for the first energy level (n = 1), there is only one subshell, which is an s subshell. For the second energy level (n = 2), there are two subshells: an s subshell and a p subshell. And so on.

Now, let's look at the electron configuration for the elements you mentioned:
- P (Phosphorus): P has an atomic number of 15, which means it has 15 electrons. Following the Aufbau principle, you start filling the subshells from the lowest energy level to the highest. P belongs to the third period (n = 3) and its highest energy subshell is the p subshell (l = 1). Therefore, the electron configuration of P is 1s^2 2s^2 2p^6 3s^2 3p^3.

- Li (Lithium): Li has an atomic number of 3, which means it has 3 electrons. Again, following the Aufbau principle, you fill the subshells from the lowest energy level to the highest. Li belongs to the second period (n = 2) and its highest energy subshell is the s subshell (l = 0). Therefore, the electron configuration of Li is 1s^2 2s^1.

- Ca (Calcium): Ca has an atomic number of 20, which means it has 20 electrons. Using the same principles, Ca belongs to the fourth period (n = 4) and its highest energy subshell is the s subshell (l = 0). Therefore, the electron configuration of Ca is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2.

- Ga (Gallium): Ga has an atomic number of 31, which means it has 31 electrons. Following the Aufbau principle, Ga belongs to the fourth period (n = 4) and its highest energy subshell is the p subshell (l = 1). Therefore, the electron configuration of Ga is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^1.

- As (Arsenic): As has an atomic number of 33, which means it has 33 electrons. Using the same principles, As belongs to the fourth period (n = 4) and its highest energy subshell is the p subshell (l = 1). Therefore, the electron configuration of As is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^3.

I hope this helps clarify the concept of electron configuration for you. Remember, practice and repetition will make it easier to understand and determine electron configurations for different elements.