How many electrons can fill the 4th Shell?
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| Shell | Subshell | Total Number of Electrons in Shell |
|---|---|---|
| 1st Shell | 1s | 2 |
| 2nd Shell | 2s, 2p | 2 + 6 = 8 |
| 3rd Shell | 3s, 3p, 3d | 2 + 6 + 10 = 18 |
| 4th Shell | 4s, 4p, 4d, 4f | 2 + 6 + 10 + 14 = 32 |
How many electrons are in 4s?
Maximum number of electron in an energy level (2n2)
| Principal Energy Level (n) | sublevels | total electrons |
|---|---|---|
| 2 | 2s 2p | 8 |
| 3 | 3s 3p 3d | 18 |
| 4 | 4s 4p 4d 4f | 32 |
| 5 | 5s 5p 5d 5f 5g | 50 |
Which element would end with 2 electrons in the 4s orbital?
scandium atom
What element is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1?
So, an antimony atom with charge +2 has an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p1.
Why is s more stable than P?
s orbitals are closer to the nucleus than p orbitals are. So electrons that are in s orbitals will be closer to the nucleus than electrons in p orbitals – and therefore, lower in energy (“opposite charges attract”).
Are higher orbitals more stable?
Energy-Level Diagrams A bonding molecular orbital is always lower in energy (more stable) than the component atomic orbitals, whereas an antibonding molecular orbital is always higher in energy (less stable).
Why do d and f orbitals have poor shielding effect?
The electrons in the s-orbital have maximum probability of being found near the nucleus and this probability goes on decreasing in case of p,d and f orbitals. For example 5f orbital has poor shielding effect than 4f orbital. This is because 5f orbitals are farther from nucleus as compared to the 4f orbitals.