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 outermost electrons of sodium fill the 3s orbital. Sodium has an electron configuration of 1s² 2s² 2p⁶ 3s¹.