Looking at the electron configuration of carbon (at. no. 6) you have 1s2 2s2 2p2. In the 2 p subshell, you have 1 electron in the 2px orbital, and 1 electron in the 2py orbital and no electrons in the 2pz orbital. So, the answer is that there are TWO half filled orbitals in the carbon atom. This is the case BEFORE hybridization. After hybridization, there are FOUR half filled orbitals which are called sp3 hybrids.
When in a bond, carbon will always have 4 half-filled orbitals. When writing the electron configuration for carbon you would probably write it like C 1s22s22p2
But in a bond, carbon changes to C 1s22s12p3
One electron from the 2p orbital jumps up to the 3p orbital
First shell- two electrons (filled)
Second shell s orbital- one electron (half filled)
Second shell, first p orbital- one electron (half filled)
Second shell, second p orbital- one electron (half filled)
Second shell, third p orbital (half filled)
It does this because filled and half-filled orbitals are exceptionally stable.
2
Ne has three p-orbitals.
3
n=2 has 3 2p orbitals.
24
Carbon IS an atom. I presume you mean how many electrons there are. There are 6 electrons, 6 protons and 6 neutrons in every un-bonded Carbon atom.
Shells: 3 Orbitals: 9
1s22s22p6
4
1
the answer is 3
One.
Ne has three p-orbitals.
2 full orbitals, S and P
4
There are 9 occupied orbitals in a phosphorus atom's ground state: one 1s orbital, one 2s orbital, three 2p orbitals, one 3s orbital, and three 3p orbitals.
some atoms have 5, some have none. the max is 5
1