How do you figure out the Noble Gas Configuration? Also, why do you not put in the "p" level and when do you( if you even do) put it in?
You need to be more specific about your question. Elements that lose electrons (Na, Ca, Al, etc) gain the noble gas structure of the noble gas preceding them in the periodic table. For example, Na (11 total electrons) loses 1 electron to become th Na^+ ion and with 10 electrons now is isoelectronic I(isoelectronic means same number of electrons) as Ne(element #10). Mg and Al lose two and three electrons respectively making them isoelectronic with Ne, also. On the other hand, elements that gain electrons to fill their outer shells, gain the noble gas structure of the noble gas following them in the periodic table. For example, Cl has 17 electrons. Adding an electron to fill out the outer shell makes it have 18 and that is isoelectronic with Ar, the next element in the table. Likewise, oxygen, #16, gains two electrons to make it 18 and like Ar. I am not sure what you mean about the p level electrons; please rephrase that part of the question. I hope this helps and is what you had in mind; if it isn't rephrase and repost.
The noble gas configuration is s2p6, except for helium which is s2.
I don't understand your second question.
My second question is that sometimes I have seen some configurations like Au = [Xe]6s24f145d9. I don't understand how come there is no "p" in the configuration.
The reason that there is no 6p in it is that there are no electrons there. After 6s, then 4f is filled, then 5d. After 5d10, comes 6p.
The configuration you mentioned for gold (Au) - [Xe]6s24f145d9 - is correct. The noble gas configuration for Au starts with [Xe], which represents the electron configuration of the noble gas xenon. This means that all the electrons from the previous noble gas, xenon, are included in the configuration.
Then, the configuration continues with 6s24f145d9. This indicates that there are 2 electrons in the 6s orbital, 14 electrons in the 4f orbital, 10 electrons in the 5d orbital, and 9 electrons in the 5d orbital. The 6p orbital is skipped because it is not yet filled.
The reason for this order is based on the Aufbau principle, which states that electrons occupy the lowest energy levels available before filling higher energy levels. In the case of gold, the 6s and 4f orbitals have lower energy levels than the 6p orbital. Therefore, the 6s and 4f orbitals are filled first before moving on to the 6p orbital.
It's important to note that the noble gas configuration does not always include the specific filling of p orbitals. This is because the order in which electron orbitals are filled can vary depending on the specific element. In the case of gold, the 6p orbital is filled after 6s, 4f, and 5d.