The elements belonging to Group IA and IIA.
In an argon atom, the outermost principle level is the third principle level (n=3). The sublevels that are occupied in this principle level are the s, p, and d sublevels. The s sublevel can hold a maximum of 2 electrons, the p sublevel can hold a maximum of 6 electrons, and the d sublevel can hold a maximum of 10 electrons.
The maximum number of electrons that can enter each type of sublevel in an atom are as follows: s sublevel: 2 electrons p sublevel: 6 electrons d sublevel: 10 electrons f sublevel: 14 electrons
The outermost s sublevel of the representative elements is filled first, followed by the p sublevel. This results in the outermost electron configuration being in the s and p sublevels.
s-sublevels holds only two electrons in maximum.
Multiply the orbitals in that sublevel by 2. The s sublevel has one orbital and can contain 2 electrons. The p sublevel has three orbitals and can contain 6 electrons. The d sublevel has five orbitals and can contain 10 electrons. The f sublevel has seven orbitals and can contain 14 electrons.
one electron
The alkaline earth metals have two electrons in their outermost s sublevel.
If you tell me what an f block element is i can help you out. I aced chemistry last semester and ill probably be tutoring it next semester. are u referring to the families in the periodic table?
In an argon atom, the outermost principle level is the third principle level (n=3). The sublevels that are occupied in this principle level are the s, p, and d sublevels. The s sublevel can hold a maximum of 2 electrons, the p sublevel can hold a maximum of 6 electrons, and the d sublevel can hold a maximum of 10 electrons.
The valence electrons in group 2 elements are found in the s sublevel. These elements are known as alkaline earth metals and have 2 valence electrons, which occupy the s sublevel of their outermost electron shell.
The maximum number of electrons that can enter each type of sublevel in an atom are as follows: s sublevel: 2 electrons p sublevel: 6 electrons d sublevel: 10 electrons f sublevel: 14 electrons
The outermost s sublevel of the representative elements is filled first, followed by the p sublevel. This results in the outermost electron configuration being in the s and p sublevels.
s-sublevels holds only two electrons in maximum.
If you're talking about any s sublevel at all, then any element except hydrogen would fit that. If you're talking specifically about elements that have the s orbital as their valence (outermost) orbital, and also have that valence s orbital filled with 2 electrons, then helium and anything in the second column of the periodic table will all fit that description. (He, Be, Mg, Ca, Sr, Ba, Ra)
Multiply the orbitals in that sublevel by 2. The s sublevel has one orbital and can contain 2 electrons. The p sublevel has three orbitals and can contain 6 electrons. The d sublevel has five orbitals and can contain 10 electrons. The f sublevel has seven orbitals and can contain 14 electrons.
there are two electons in the s sublevel. It is the number of electrons that fit in the first orbital around an atom.
For noble gases, the outermost s and p sublevels are already filled with electrons. This is what gives them their stable configuration and makes them generally unreactive.