s contains one orbital with a maximum of 2 electrons
p contains three orbitals with a maximum of 6 electrons
d contains five orbitals with a maximum of 10 electrons
f contains seven orbital with a maximum of 14 electrons
The third period of the periodic table can hold a maximum of 18 electrons. This includes filling the 3s, 3p, and 3d sublevels with a total of 8, 6, and 4 electrons respectively.
By the first principle energy level I assume you are referring to the lowest atomic orbital or ta principal quantum number of 1. This orbital holds 1 pair of 2 electrons.
The maximum number of electrons that can exist in 4f orbitals is 14.-pg. 110 Modern Chemistry table 2:)
The maximum number of electrons in any energy level is given by 2n2. Any more would be energetically unfavorable. So in the fourth is would be 2 x 42 = 32 4s2 4p6 4d10 4f14 So a total of 2+6+10+14 = 32
Sublevels of elements refer to the energy levels within an atom where electrons are found. These sublevels are designated by the letters s, p, d, and f. Each sublevel has a maximum number of electrons it can hold (2 for s, 6 for p, 10 for d, and 14 for f) and they are arranged in order of increasing energy within an atom.
The 2s sublevel can hold a maximum of 2 electrons.
The maximum number of electrons in the fourth energy level is 32. This level can hold up to 32 electrons distributed among its various sublevels (s, p, d, and f).
In the third principal quantum number (n=3), there are a maximum of 18 electrons that can be accommodated in different sublevels within that energy level (s, p, d).
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The s, p, d, and f are sublevels within an electron energy level. Each sublevel can hold a specific maximum number of electrons based on their shapes and orientations. Electrons fill these sublevels based on the Aufbau principle, Pauli exclusion principle, and Hund's rule, which dictate the order and orientation in which electrons occupy the sublevels.
The third period of the periodic table can hold a maximum of 18 electrons. This includes filling the 3s, 3p, and 3d sublevels with a total of 8, 6, and 4 electrons respectively.
In the ground state of a chlorine atom, there are 3 occupied sublevels: 1s, 2s, and 2p. Each sublevel can hold a maximum of 2 electrons, giving a total of 2 + 2 + 6 = 10 electrons.
The fourth energy level can hold a maximum of 32 electrons. This energy level consists of 4 sublevels: s, p, d, and f. Each sublevel can hold a different number of electrons, with the s sublevel holding a maximum of 2, p holding 6, d holding 10, and f holding 14 electrons.
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By the first principle energy level I assume you are referring to the lowest atomic orbital or ta principal quantum number of 1. This orbital holds 1 pair of 2 electrons.
18 electrons can occupy the third energy levelIt is like this3s- 2 electrons3p- 6 electrons3d- 10 electrons
The letter designations for the first four sublevels and their maximum number of electrons are as follows: s sublevel: can hold a maximum of 2 electrons. p sublevel: can hold a maximum of 6 electrons. d sublevel: can hold a maximum of 10 electrons. f sublevel: can hold a maximum of 14 electrons.