Ca
Ca
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.
The element with that electron configuration has 4 electrons in the third level. There are 2 electrons in the 3s sublevel and 2 more electrons in the 3p sublevel. This means 4 valence electrons total. This element is silicon (Si, #14).
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.
Ca
Ca
Ca
Ca
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.
The element with that electron configuration has 4 electrons in the third level. There are 2 electrons in the 3s sublevel and 2 more electrons in the 3p sublevel. This means 4 valence electrons total. This element is silicon (Si, #14).
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.
because sublevel p has 3 orbital and each orbital can hold up to 2 electrons meanwhile sublevel s only has 1 orbital and each can hold 2 electrons therefore sublevel p can hold more
There are 9 orbitals in a g sublevel. (there is 1 in an s sublevel, 3 in a p sublevel, 5 in a d sublevel, 7 in an f sublevel, 9 in a g sublevel, 11 in an h sublevel, etc.)
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.
The element with atomic number 56 is barium, a group 2 alkaline earth metal. Its atoms have two valence electrons in the 6s sublevel.
Carbon is the group 14, period 2 chemical element. Its electron configuration is 1s2 2s2 2p2. Thus, carbon has 2 electrons in its 2p subshell.