the d-sub shell has five orbitals
Each of the p orbitals can hold 2 electrons due to the Pauli exclusion principle. Because there are 3 p orbitals in a given subshell, the overall p subshell can hold 6 electrons.
If m sub l is three, then there can be 7 orbitals, since the l value (the one that corresponds to the orbitals) would be 3 (denoting the f orbital).
Assuming you mean two sets of p orbitals on adjacent atoms only one sigma bond can be formed, by the p orbitals that point between the atoms to form an axial bond. The lobes that are at right angles , ( two unused p orbitals on each atom) could form pi bonds.
the p subshell has 3 orbitals. Each Orbital can hold 2 electrons with opposite spins. therefore the p subshell can hold a maximum of 6 electrons.
There are 2, the 2s and 2p subshells. The s subshell contains just one orbital and can hold only two electrons (of opposite spin) The p subshell contains 3 orbitals each of which can hold just 2 electrons (of opposite spin) making 6 electrons in all
d
i have no idea hahahaha but it could be s p f or d
Each of the p orbitals can hold 2 electrons due to the Pauli exclusion principle. Because there are 3 p orbitals in a given subshell, the overall p subshell can hold 6 electrons.
You can differentiate between a 2s and a 2p subshell based on their shape. The 2s subshell is spherically symmetric and has one orbital. On the other hand, the 2p subshell has a dumbbell shape and consists of three orbitals: px, py, and pz, each oriented along separate axes.
The electrons themselves are all identical to any other electron. Their distribution about the nucleus will be approximately spherical, with twelve electrons in s orbitals of various sizes, twenty-four in p orbitals, twenty-five in d orbitals, and fourteen in f orbitals. As for the shapes of the individual orbitals, s orbitals are spherical, p orbitals have two teardrop shaped lobes pointing 180 degrees away from each other (e.g. up and down), d orbitals have four teardrop shaped lobes pointing 90 degrees away from each other (e.g. up, down, left and right), and f orbitals have six teardrop shaped lobes, also pointing 90 degrees from each other (e.g. up, down, left, right, forward, and back). All these shapes overlap with each other to provide a roughly spherical electron distribution.
6 electrons in 3 orbitals of p-sublevel: px, py and pz
If m sub l is three, then there can be 7 orbitals, since the l value (the one that corresponds to the orbitals) would be 3 (denoting the f orbital).
Assuming you mean two sets of p orbitals on adjacent atoms only one sigma bond can be formed, by the p orbitals that point between the atoms to form an axial bond. The lobes that are at right angles , ( two unused p orbitals on each atom) could form pi bonds.
the p subshell has 3 orbitals. Each Orbital can hold 2 electrons with opposite spins. therefore the p subshell can hold a maximum of 6 electrons.
There are 2, the 2s and 2p subshells. The s subshell contains just one orbital and can hold only two electrons (of opposite spin) The p subshell contains 3 orbitals each of which can hold just 2 electrons (of opposite spin) making 6 electrons in all
The second energy level (n =2 ) has 1 s orbtial, and 3 p orbitals. The s contains 2 electrons, and each p contains 2 electrons (for a total of 6 electrons in the 3 p orbitals). Thus, the second energy level can hold a maximum of EIGHT (8) electrons.
s = 2 electrons p = 6 electrons d = 10 electrons f = 14 electrons Each single s orbital has two electrons in it. Each p orbital has two electrons in it and as there are three of these orbitals in a p subshell, the total electron number is six. d has five orbitals in its subshell, containing ten electrons (two in each orbital) when full, which form a dumbell-esque shape. f has seven orbitals each containing two electrons.