Oxygen is in period 2 of the Periodic Table, telling you that it has n=2 or 2 orbits. The number of orbitals would be 1 in n=1 and 4 in n=2 for a total of 5 orbitals, if that is what you mean. Looking at it another way: for n=1, there is 1s (1 orbital); for n=2, there is 2s (1 orbital) and 2p (3 orbitals). The electron configuration is 1s2 2s2 2p4
there are 8 electrons in a atom of oxygen!
six valence electrons
Just one.
sodium
2
All p sublevels contain three orbitals, including the 4p sublevel.
There are 7 orbitals in the F-block
It needs two electrons. Then it would have ten electrons, which would mean full s- and p-orbitals.
P and S both have 'd' orbitals in outermost shell while N and O do not.
oxygen is para magnetic in nature. Due to the presence of 2 unpaired electron ^Py and ^Pz anti bonding orbitals. which account for the para magnetic behavior of oxygen
5 orbitals
7 Orbitals
16 orbitals
Ne has three p-orbitals.
Always three!
Shells: 3 Orbitals: 9
Helium doesn't combine with oxygen. Helium is chemically inert because it has completely filled valence orbitals.
All p sublevels contain three orbitals, including the 4p sublevel.
No..It is hybridised to be precise.. See oxygen forms 3 sp2 hybrid orbitals with two half filled orbitals and one orbital filled with the lone pair.. hence the half filled orbitals are each filled by the hydrogen atoms respectively( as hydrogen requires only one atom for stability)..
There are 4 orbitals in H2O , one s and 3 p
There are 7 orbitals in the F-block
2 full orbitals, S and P