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26 sigma 7 pi
Two electrons can occupy the 2s subshell, and 8 electrons can occupy the 3d subshell.
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The third energy level contains one s orbital and three p orbitals.
24
26 sigma 7 pi
There are 6 Chlorine has 7 valence electrons, and since 2 of them can occupy one s orbital, there needs to be 5 p orbitals for everything else. (5+1=6)
5 electrons in p orbitals in the outer shell. Cl has an electronic configuration of [Ne] 3s2, 3p5 In level 2 there a further 6 electrons in p orbitals making 11 electrons in total occupying p orbitals
two and both must be of opposite spin to each other
Multiply the orbitals in that sublevel by 2. The s sublevel has one orbital and can contain 2 electrons. The p sublevel has three orbitals and can contain 6 electrons. The d sublevel has five orbitals and can contain 10 electrons. The f sublevel has seven orbitals and can contain 14 electrons.
6 degenerate orbitals allows for seven electrons, five of which are unpaired. ans is 6
Every orbital is different. 2 can occupy the first orbital then 8 can occupy mostly the rest. When you start getting really low on the periodic table orbitals start holding 16, but not till u get really low
17. The electronic configuration of bromine is 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 4p5
Arsenic has three electrons occupying the three 4p orbitals in its valence shell. Hund's first rule tells us that they will each occupy separate orbitals before they start to pair up. So there are three half-filled orbitals in an arsenic atom.
Two electrons can occupy the 2s subshell, and 8 electrons can occupy the 3d subshell.
for the case of n=4 the available orbitals include 1s 3p and 5d, a total of 9 electron orbitals which can occupy 18 electrons. There are 18 elements in the 4th row which coincides with the 9 available orbitals.