5x7=35, then 3-1=2, so 35+2=37
1s 2s 3s 3p 4s 3d 4p
The ground state configuration of 1s²2s²2p²3s²3p¹ is [Ne]3s²3p¹. This notation represents the electron configuration in shorthand form, where [Ne] represents the electron configuration of the noble gas neon (1s²2s²2p⁶).
It's in the tables of 1s, 3s, 9s, and 27s .
4s 3p 3s 2p 1s This is probably one of the easiest chemistry problems in the book, you should probably look it up.
The electron configurations provided are: 1s² 2s² 2p⁶ 3s² 3p⁶ 1s² 2s² 2p⁶ 3s² 3p³ 1s² 2s² 2p⁶ 3s² 3p⁴ The electron configuration that does not belong to the same group or family as the others is (2) 1s² 2s² 2p⁶ 3s² 3p³, as it represents a different element with a different number of valence electrons compared to the other configurations.
The principal quantum number (n) distinguishes between different subshells. For example, the 1s subshell has an n value of 1, while the 3s subshell has an n value of 3. The higher the n value, the higher the energy level of the subshell.
The electron configuration of CCl4 is 1s^2 2s^2 2p^6 3s^2 3p^2. This means that the carbon atom has 2 electrons in the 1s orbital, 2 electrons in the 2s orbital, 6 electrons in the 2p orbital, 2 electrons in the 3s orbital, and 2 electrons in the 3p orbital.
Its energy level must be increased.
1s^2 2s^2 2p^6 3s^2 3p^2
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
In a silicon atom, there are four filled orbitals. Specifically, there are two filled in the 1s orbital and two filled in the 2s orbital.
The M orbital, there's only 1 electron in it.