Ca
The element with 2 electrons in the 4s sublevel is calcium (Ca), as it has an electron configuration of [Ar] 4s2.
Calcium is the element that has 2 electrons in the 4s sublevel.
The elements that have 2 electrons in the 4s sublevel are calcium (Ca) and scandium (Sc).
The element with its outermost electrons in an S sublevel is found in Group 1 and Group 2 of the periodic table. These elements have their outermost electrons in the S sublevel before transitioning to the D sublevel in subsequent groups.
There are 2 electrons in the 2p sublevel of carbon.
The number of electrons found in each sublevel is given by the formula 2n^2, where n is the principal quantum number. For example, the s sublevel can hold a maximum of 2 electrons, the p sublevel can hold a maximum of 6 electrons, the d sublevel can hold a maximum of 10 electrons, and the f sublevel can hold a maximum of 14 electrons.
Calcium is the element that has 2 electrons in the 4s sublevel.
Ca
The elements that have 2 electrons in the 4s sublevel are calcium (Ca) and scandium (Sc).
Ca
The number of electrons found in each sublevel is given by the formula 2n^2, where n is the principal quantum number. For example, the s sublevel can hold a maximum of 2 electrons, the p sublevel can hold a maximum of 6 electrons, the d sublevel can hold a maximum of 10 electrons, and the f sublevel can hold a maximum of 14 electrons.
The electron structure given is 1s2 2s2 2p6 3s2 3p2. Adding up the electrons in each level gives 2 + 2 + 6 + 2 + 2 = 14 electrons. The third principal energy level corresponds to n=3, so the number of electrons in the third level is 2 + 2 + 6 = 10.
An element cannot have 4 electrons in the 2 s level. The s subshell can hold only TWO electrons. Carbon has 4 electrons in the 2p level, however, if that's what you meant.
The p sublevel consists of three orbitals, each of which can hold up to 2 electrons. This totals to a maximum of 6 electrons in the p sublevel. In contrast, the s sublevel consists of only one orbital, which can hold a maximum of 2 electrons due to the rules of electron configuration in an atom.
There are 1 orbital in the g sublevel. Each orbital can hold up to 2 electrons. Therefore, the g sublevel can hold a maximum of 2 electrons.
In actuality Mn has SEVEN valence electrons, not really 2 as might be predicted. The reason for this is that Mn is [Ar]3d5 4s2, and as a transition element, not only are the 4s electrons available for bonding, but so are those in the d orbital. So, the 5 electrons in 3d and the 2 electrons in 4s are all considered as valence electrons.
An element with atomic number 56 would have 2 electrons in the first energy level and 8 electrons in the second energy level, totaling 10 valence electrons.
There are 2 electrons in the 2p sublevel of carbon.